Answer:
0.64 kW
Explanation:
The potential energy of a mass (M) at some height (h) is computed from ...
PE = Mgh
At 1 kg/liter, the available power is the rate at which that energy is available ...
(490 kg/min)×(1 min/(60 s))×(9.8 m/s²)(8 m) ≈ 640.3 kg·m²/s³
= 640.3 W
In kilowatts, that is 0.64 kW.
Final answer:
The water wheel could have produced approximately 0.641 kW of power by converting the gravitational potential energy of water. This is calculated using the water's mass flow rate and the height of the wheel, considering the density of water is 1000 kg/m³.
Explanation:
The power that the water wheel could have produced can be calculated using the principles of mechanical energy and gravitational potential energy (GPE). The formula for GPE is given by mgh, where m is the mass of the water, g is the acceleration due to gravity (9.8 m/s²), and h is the height.
The flow rate of water is 490 liters per minute, which we convert to cubic meters per second (m³/s) for our calculations, as 490 liters per minute is equal to 0.49 m³/min or 0.00817 m³/s, given that 1 cubic meter equals 1000 liters. Using the density of water, which is 1000 kg/m³, the mass flow rate of water is calculated as the product of the flow rate by the density (0.00817 m³/s * 1000 kg/m³ = 8.17 kg/s).
Thus, the power (P) in watts (W) is P = mgh which translates into P = 8.17 kg/s * 9.8 m/s² * 8 m. Upon calculation, this gives a power of approximately 640.88 watts, which we convert to kilowatts (kW) by dividing by 1000, resulting in approximately 0.641 kW.
hotosynthesis can be represented by 6CO2(g)+6H2O(l)⇌C6H12O6(s)+6O2(g) Which of the following will be false when the photosynthesis reaction reaches equilibrium?
a.The rate of formation of O2 is equal to the rate of formation of CO2.
b.The concentration of O2 will begin decreasing.
c.The concentrations of CO2 and O2 will not change.
d.The concentrations of CO2 and O2 will be equal.
Answer: Option (b) and (d) are correct.
Explanation:
An equilibrium reaction is defined as the reaction in which rate of forward reaction equals rate of backward reaction.
A photosynthesis reaction is the reaction in which plants in the presence of sunlight, water, and carbon dioxide make their own food.
The amount of carbon dioxide consumed will be equal to the rate of formation of oxygen into the atmosphere.Hence, the statement rate of formation of [tex]O_{2}[/tex] is equal to the rate of formation of [tex]CO_{2}[/tex] is true.
Concentration of oxygen may remain constant but it will not decrease. Hence, the statement concentration of [tex]O_{2}[/tex] will begin decreasing, is false.As both oxygen and carbon dioxide are present in an equilibrium reaction, So, their concentration will not change.Hence, the statement concentrations of [tex]CO_{2}[/tex] and [tex]O_{2}[/tex] will not change, is true.
Concentration of carbon dioxide and oxygen will also depend on the limiting reagent. So, it is not necessary that the concentrations of [tex]CO_{2}[/tex] and [tex]O_{2}[/tex] will be equal.Some amount of carbon dioxide might escape out into the air.
Hence, the statement concentrations of [tex]CO_{2}[/tex] and [tex]O_{2}[/tex] will be equal, is false.
You can identify a metal by carefully determining its density. A 8.44 g piece of an unknown metal is 1.25 cm long, 2.50 cm wide, and 1.00 cm thick. What is a possible identity of the element?Aluminum, 2.70 g/cm3Titanium, 4.54 g/cm3Zirconium, 6.51 g/cm3Chromium, 7.20 g/cm3Nickel, 8.90 g/cm3
Answer: Aluminum, [tex]2.70 g/cm^3[/tex]
Explanation:
Density is defined as the mass contained per unit volume. It is characteristic of a substance.
[tex]Density=\frac{mass}{Volume}[/tex]
Given : Mass of object = 8.44 grams
Volume of object=[tex]length\times breadth\times height=1.25cm\times 2.50cm\times 1.0cm=3.125cm^3[/tex]
Putting in the values we get:
[tex]Density=\frac{8.44g}{3.125cm^3}=2.70g/cm^3[/tex]
Thus density of the object will be [tex]2.70 g/cm^3[/tex] which matches that of aluminium.
Answer: Nickel
Explanation:
They have the same density as each other
The Heat transferred through wave energy (electromagnetic waves) is: A. Sublimation B. Conduction C. Radiation D. Nuclear Fusion
Answer:
C. Radiation
Explanation:
The Heat transferred through wave energy (electromagnetic waves) is Radiation.
The Heat transferred through wave energy (electromagnetic waves) is Radiation.
The reaction converting glycerol to glycerol-3-phosphate (energetically unfavorable) can be coupled with the conversion of ATP to ADP (energetically favorable): glycerol+HPO42−ATP+H2O⟶⟶glycerol-3-phosphate+H2OADP+HPO42−+H+ Part A What are the net products of the coupled reactions above?
Answer:
glycerol-3-phosphate, ADP, H⁺
Explanation:
The reaction of converting glycerol to glycerol-3-phosphate which makes is unfavorable and is coupled with the second reaction which involves conversion of ATP to ADP which is high energetically favorable.
Reaction 1: Glycerol + HPO₄²⁻ ⇒ Glycerol-3-phosphate + water
Reaction 2: ATP + H₂O ⇒ ADP + HPO₄²⁻ + H⁺
The coupled reaction of both the reactions become favorable. Thus, the overall coupled reaction is:
Glycerol + ATP ⇒ Glycerol-3-phosphate + ADP + H⁺
The net products are = glycerol-3-phosphate, ADP, H⁺
The net products of the coupled reactions as described are; glycerol-3-phosphate, ADP and H+.
According to the reaction;
According to the reaction;We are required to determine the net products of the coupled reactions above.The reactions given is as follows;
glycerol + (HPO4)²− + ATP+H2O ⟶⟶ glycerol-3-phosphate+H2O ADP+(HPO4)²- + H+
Since, the (HPO4)²- cancels out on both sides of the equation; the net products of the coupled reactions above are; glycerol-3-phosphate, ADP and H+.
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What volume (in liters) of carbon monoxide gas, measured at a temperature of 212 K and a pressure of 676 mm Hg, is required to synthesize 19.3 g of methanol. How many liters of oxygen (at STP) are required to form 12.5 g of H2O ? Show your work
Answer:
For 1: The volume of carbon monoxide required to produce given amount of methanol is 11.9 L.
For 2: The volume of oxygen required to form given amount of water is 7.77 L.
Explanation:
For 1:To calculate the number of moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex] ......(1)
For methanol:
Given mass of methanol = 19.3 g
Molar mass of methanol = 32 g/mol
Putting values in above equation, we get:
[tex]\text{Moles of methanol}=\frac{19.3g}{32g/mol}=0.603mol[/tex]
The chemical reaction of formation of methanol from carbon monoxide follows:
[tex]CO+2H_2\rightarrow CH_3OH[/tex]
By Stoichiometry of the reaction:
1 mole of methanol is produced from 1 mole of carbon monoxide.
so, 0.603 moles of methanol will be produced from = [tex]\frac{1}{1}\times 0.603=0.603mol[/tex] of carbon monoxide.
To calculate the volume of carbon monoxide, we use the equation given by ideal gas:
PV = nRT
where,
P = Pressure of carbon monoxide = 676 mmHg
V = Volume of carbon monoxide = ? L
n = Number of moles of carbon monoxide = 0.603 mol
R = Gas constant = [tex]62.3637\text{ L.mmHg }mol^{-1}K^{-1}[/tex]
T = Temperature of carbon monoxide = 212 K
Putting values in above equation, we get:
[tex]676mmHg\times V=\frac{19.3}{32g/mol}\times 62.3637\text{ L.mmHg }mol^{-1}K^{-1}\times 212K\\\\V=11.79L[/tex]
Hence, the volume of carbon monoxide required to produce given amount of methanol is 11.9 L.
For 2:Calculating the moles of water by using equation 1, we get:
Given mass of water = 12.5 g
Molar mass of water = 18 g/mol
Putting values in equation 1, we get:
[tex]\text{Moles of water}=\frac{12.5g}{18g/mol}=0.694mol[/tex]
The chemical reaction of formation of water from oxygen and hydrogen follows:
[tex]O_2+2H_2\rightarrow 2H_2O[/tex]
By Stoichiometry of the reaction:
2 moles of water is produced from 1 mole of oxygen gas.
so, 0.694 moles of water will be produced from = [tex]\frac{1}{2}\times 0.694=0.347mol[/tex] of oxygen gas.
At STP:
1 mole of a gas occupies 22.4 L of volume.
So, 0.347 moles of oxygen gas will occupy = [tex]\frac{22.4L}{1mol}\times 0.347mol=7.77L[/tex]
Hence, the volume of oxygen required to form given amount of water is 7.77 L.
A sample of oxygen gas was collected via water displacement. Since the oxygen was collected via water displacement, the sample is saturated with water vapor. If the total pressure of the mixture at 26.4 °C is 805 torr, what is the partial pressure of oxygen? The vapor pressure of water at 26.4 °C is 25.81 mm Hg.
Answer : The partial pressure of oxygen is, 799.19 torr
Solution :
According to the Dalton's law, the total pressure of the gas is equal to the sum of the partial pressure of the mixture of gasses.
[tex]P_T=p_{H_2O}+p_{O_2}[/tex]
where,
[tex]P_T[/tex] = total partial pressure = 805 torr
[tex]P_{O_2}[/tex] = partial pressure of oxygen gas = ?
[tex]P_{H_2O}[/tex] = partial pressure of water = 25.81 mm Hg = 25.81 torr
Now put all the given values is expression, we get the partial pressure of the oxygen gas.
[tex]805\text{ torr}=25.81\text{ torr}+p_{O_2}[/tex]
[tex]p_{O_2}=779.19\text{ torr}[/tex]
Therefore, the partial pressure of oxygen gas is, 799.19 torr
A piston-cylinder device contains 257 grams of R134a at 60 kPa and -20°C. The R134a is heated until its temperature reaches 100°C. Determine the total change of volume.
Answer : The total change of volume is, 41.883 liters.
Explanation :
R134a is a 1,1,1,2-tetrafluoroethane. It is a hydro-fluorocarbon and haloalkane gaseous refrigerant.
First we have to calculate the volume at [tex]-20^oC[/tex].
Using ideal gas equation:
[tex]PV=nRT\\\\PV=\frac{w}{M}\times RT[/tex]
where,
n = number of moles
w = mass of R134a = 257 g
P = pressure of the gas = 60 Kpa
T = temperature of the gas = [tex]-20^oC=273+(-20)=253K[/tex]
M = molar mass of R134a = 102.03 g/mole
R = gas constant = 8.314 Kpa.L/mole.K
V = initial volume of gas
Now put all the given values in the above equation, we get :
[tex](60Kpa)\times V=\frac{257g}{102.03g/mole}\times (8.314Kpa.L/mole.K)\times (253K)[/tex]
[tex]V=88.305L[/tex]
Now we have to calculate the volume at [tex]100^oC[/tex] by using Charles's law.
Charles' Law : It is defined as the volume of gas is directly proportional to the temperature of the gas at constant pressure and number of moles.
[tex]V\propto T[/tex]
or,
[tex]\frac{V_1}{V_2}=\frac{T_1}{T_2}[/tex]
where,
[tex]V_1[/tex] = initial volume of gas = 88.305 L
[tex]V_2[/tex] = final volume of gas = ?
[tex]T_1[/tex] = initial temperature of gas = 253 K
[tex]T_2[/tex] = final temperature of gas = [tex]100^oC=273+100=373K[/tex]
Now put all the given values in the above formula, we get the final volume of the gas.
[tex]\frac{88.305L}{V_2}=\frac{253K}{373K}[/tex]
[tex]V_2=130.188L[/tex]
Now we have to calculate the total change of volume.
[tex]V_2-V_1=130.188-88.305=41.883L[/tex]
Therefore, the total change of volume is, 41.883 liters.
A mixture of helium and nitrogen gases at a total pressure of 641 mm mm Hg. If the gas mixture contains 0.399 grams of helium, how many grams of nitrogen are present? Hg contains helium at a partial pressure of 231 g
Answer : The mass of nitrogen present are, 4.965 grams.
Explanation :
According to the Raoult's law,
[tex]p_{He}=X_{He}\times p_T[/tex]
where,
[tex]p_{He}[/tex] = partial pressure of gas = 231 mmHg
[tex]p_T[/tex] = total pressure of gas = 641 mmHg
[tex]X_{He}[/tex] = mole fraction of helium gas = ?
Now put all the given values in this formula, we get the mole fraction of helium gas.
[tex]231mmHg=X_{He}\times 641mmHg[/tex]
[tex]X_{He}=0.36[/tex]
Now we have to calculate the mole fraction of nitrogen gas.
[tex]X_{He}+X_{N_2}=1[/tex]
[tex]X_{N_2}=1=0.36=0.64[/tex]
Now we have to calculate the mass nitrogen gas.
[tex]\frac{X_{He}}{X_{N_2}}=\frac{n_{He}}{n_{N_2}}[/tex]
[tex]\frac{X_{He}}{X_{N_2}}=\frac{\frac{w_{He}}{M_{He}}}{\frac{w_{N_2}}{M_{N_2}}}[/tex]
where,
n = moles, w = mass, M = molar mass
Now put all the given values in this expression, we get:
[tex]\frac{0.36}{0.64}=\frac{\frac{0.399}{4}}{\frac{w_{N_2}}{28}}[/tex]
[tex]w_{N_2}=4.965g[/tex]
Therefore, the mass of nitrogen present are, 4.965 grams.
Which of the following has the greatest number of particles? Which of the following has the greatest number of particles? 22.990 g of Na 1 mole of Na 9.012 g of Be 1 mole of Be All are the same.
Answer: All the given options have the same number of particles.
Explanation:
For the given options:
Option 1: 22.990 g of NaAccording to mole concept:
1 mole of an atom contains [tex]6.022\times 10^{23}[/tex] number of atoms.
If, 22.99 g of sodium metal contains [tex]6.022\times 10^{23}[/tex] number of atoms.
So, 22.990 g of sodium metal will contain [tex]\frac{6.022\times 10^{23}}{22.99}\times 22.990=6.022\times 10^{23}[/tex] number of atoms.
Number of particles = [tex]6.022\times 10^{23}[/tex]
Option 2: 1 mole of NaAccording to mole concept:
1 mole of an atom contains [tex]6.022\times 10^{23}[/tex] number of atoms.
So, 1 mole of sodium element will also contain [tex]6.022\times 10^{23}[/tex] number of atoms.
Number of particles = [tex]6.022\times 10^{23}[/tex]
Option 3: 9.012 g of BeAccording to mole concept:
1 mole of an atom contains [tex]6.022\times 10^{23}[/tex] number of atoms.
If, 9.01 g of beryllium metal contains [tex]6.022\times 10^{23}[/tex] number of atoms.
So, 9.012 g of beryllium metal will contain [tex]\frac{6.022\times 10^{23}}{9.01}\times 9.012=6.022\times 10^{23}[/tex] number of atoms.
Number of particles = [tex]6.022\times 10^{23}[/tex]
Option 4: 1 mole of BeAccording to mole concept:
1 mole of an atom contains [tex]6.022\times 10^{23}[/tex] number of atoms.
So, 1 mole of beryllium element will also contain [tex]6.022\times 10^{23}[/tex] number of atoms.
Number of particles = [tex]6.022\times 10^{23}[/tex]
Hence, all the options have same number of particles which is [tex]6.022\times 10^{23}[/tex]
Both 1 mole of sodium (Na) and 1 mole of beryllium (Be) contain the greatest number of particles, which is Avogadro's Number or 6.02×1023 particles. The other listed quantities, 22.990 g of Na and 9.012 g of Be, contain fewer particles as they are less than one mole of their respective elements.
Explanation:To determine which of the given options has the greatest number of particles, we must refer to Avogadro's Number and the concept of molar mass. Avogadro's Number, which is 6.02×1023 mol-1, represents the number of particles in one mole of a substance. The molar mass is the mass of one mole of representative particles of a substance and is equivalent numerically to the atomic mass of an element in grams. For instance, the atomic mass of sodium (Na) is approximately 23 g/mol, which means that 1 mole of Na has a mass of approximately 23 grams and contains 6.02×1023 particles of Na.
Therefore, 1 mole of any substance, whether Na or beryllium (Be), will always contain 6.02×1023 particles. Comparing the options given:
22.990 g of Na - This is less than 1 mole of Na, so it contains fewer than 6.02×1023 particles.1 mole of Na - This contains 6.02×1023 particles.9.012 g of Be - This is less than 1 mole of Be (given that Be has a molar mass around 9.012 g/mol), so it also has fewer than 6.02×1023 particles.1 mole of Be - This too contains 6.02×1023 particles.All are the same - This is incorrect since the options with amounts less than 1 mole (22.990 g of Na and 9.012 g of Be) have fewer particles.Both 1 mole of Na and 1 mole of Be have the greatest number of particles, which is Avogadro's Number of particles. The quantities that are less than one mole have fewer particles in comparison.
A more experienced colleague mentions to you that you should aim for a dissolved oxygen concentration around 1.0 mg/L at day 5 of the experiment. They show you data from a similar wastewater spill that happened last year, in which the BOD5 of the stream water was 60 mg/L. From your previous experiment, you found that the dissolved oxygen concentration at day 0 was 10 mg/L. Based on this information, what dilution factor, P, should you try in your reactor?
Answer:
3
Explanation:
Lt= Loe^(-kt)
Data:
Lo = 10 mg/mL
Assume k = 0.23/da
1. Calculate L5
L5 = 10e^(-5×0.23) = 10e^-1.15 = 10 × 0.317 = 3.17 mg/mL
2. Calculate the dilution factor
You expect to find L5 to be about 3
You want L5 to be about 1.
You should use a dilute your sample by a factor of 3.
P = 3
The chemical formula for ferric sulfate is Fe(SO4)3. Determine the following:
a) the number of sulfur atoms in 1.75 mole of Fe(SO4)3
b) the mass in grams of 2.65 mol of Fe(SO4)3
c) the number of moles of Fe(SO4)3 in 3.45 grams of Fe(SO4)3.
d)the mass in grams of 3 formula unit of Fe(SO4)3
Answer :
(a) The number of sulfur atoms are, [tex]31.61\times 10^{23}[/tex].
(b) The mass of the mass of [tex]Fe_2(SO_4)_3[/tex] is, 1059.682 grams.
(c) The number of moles of [tex]Fe_2(SO_4)_3[/tex] is, [tex]8.63\times 10^{-3}mole[/tex]
(d) The mass of the mass of [tex]Fe_2(SO_4)_3[/tex] is, [tex]19.95\times 10^{-22}g[/tex]
Explanation :
(a) As we are given the number of moles of [tex]Fe_2(SO_4)_3[/tex] is, 1.75 mole. Now we have to calculate the number of sulfur atoms.
In the [tex]Fe_2(SO_4)_3[/tex], there are 2 iron atoms, 3 sulfur atoms, 12 oxygen atoms.
As, 1 mole of [tex]Fe_2(SO_4)_3[/tex] contains [tex]3\times 6.022\times 10^{23}[/tex] number of sulfur atoms.
So, 1.75 mole of [tex]Fe_2(SO_4)_3[/tex] contains [tex]1.75\times 3\times 6.022\times 10^{23}=31.61\times 10^{23}[/tex] number of sulfur atoms.
The number of sulfur atoms are, [tex]31.61\times 10^{23}[/tex]
(b) As we are given the number of moles of [tex]Fe_2(SO_4)_3[/tex] is, 2.65 mole. Now we have to calculate the mass of [tex]Fe_2(SO_4)_3[/tex].
[tex]\text{Mass of }Fe_2(SO_4)_3=\text{Moles of }Fe_2(SO_4)_3\times \text{Molar mass of }Fe_2(SO_4)_3[/tex]
The molar mass of [tex]Fe_2(SO_4)_3[/tex] = 399.88 g/mole
[tex]\text{Mass of }Fe_2(SO_4)_3=2.65mole\times 399.88g/mole=1059.682g[/tex]
The mass of the mass of [tex]Fe_2(SO_4)_3[/tex] is, 1059.682 grams.
(c) As we are given the mass of [tex]Fe_2(SO_4)_3[/tex] is, 3.45 grams. Now we have to calculate the moles of [tex]Fe_2(SO_4)_3[/tex].
[tex]\text{Mass of }Fe_2(SO_4)_3=\text{Moles of }Fe_2(SO_4)_3\times \text{Molar mass of }Fe_2(SO_4)_3[/tex]
The molar mass of [tex]Fe_2(SO_4)_3[/tex] = 399.88 g/mole
[tex]3.45g=\text{Moles of }Fe_2(SO_4)_3\times 399.88g/mole[/tex]
[tex]\text{Moles of }Fe_2(SO_4)_3=8.63\times 10^{-3}mole[/tex]
The number of moles of [tex]Fe_2(SO_4)_3[/tex] is, [tex]8.63\times 10^{-3}mole[/tex]
(d) As we are given the formula unit of [tex]Fe_2(SO_4)_3[/tex] is, 3. Now we have to calculate the mass of [tex]Fe_2(SO_4)_3[/tex].
As we know that 1 mole of [tex]Fe_2(SO_4)_3[/tex] contains [tex]6.022\times 10^{23}[/tex] formula unit.
Formula used :
[tex]\text{Formula unit of }Fe_2(SO_4)_3=\text{Moles of }Fe_2(SO_4)_3\times 6.022\times 10^{23}[/tex]
[tex]3=\text{Moles of }Fe_2(SO_4)_3\times 6.022\times 10^{23}[/tex]
[tex]\text{Moles of }Fe_2(SO_4)_3=4.989\times 10^{-24}mole[/tex]
Now we have to calculate the mass of [tex]Fe_2(SO_4)_3[/tex].
[tex]\text{Mass of }Fe_2(SO_4)_3=\text{Moles of }Fe_2(SO_4)_3\times \text{Molar mass of }Fe_2(SO_4)_3[/tex]
The molar mass of [tex]Fe_2(SO_4)_3[/tex] = 399.88 g/mole
[tex]\text{Mass of }Fe_2(SO_4)_3=4.989\times 10^{-24}mole\times 399.88g/mole=19.95\times 10^{-22}g[/tex]
The mass of the mass of [tex]Fe_2(SO_4)_3[/tex] is, [tex]19.95\times 10^{-22}g[/tex]
Final answer:
The key parts of solving chemistry problems include understanding chemical formulas and conducting mole-mass calculations. Using the formula for ferric sulfate, Fe(SO₄)₃, this response walks through how to find the number of atoms, mass of substance, and moles given specific quantities, showcasing the essential chemical calculations involved.
Explanation:
The chemical formula for ferric sulfate is Fe(SO₄)₃. Let's solve each part of the question:
a) The number of sulfur atoms in 1.75 mole of Fe(SO₄)₃: There are 3 sulfur atoms in one formula unit of Fe(SO₄)₃. Therefore, in 1.75 moles of Fe(SO₄)₃, there are 1.75 moles * 3 sulfur atoms per mole = 5.25 moles of sulfur atoms.
b) The mass in grams of 2.65 mol of Fe(SO₄)₃: First, we need to calculate the molar mass of Fe(SO₄)₃ (Fe = 55.85, S = 32.06, O = 16.00). The molar mass of Fe(SO₄)₃ is 399.88 g/mol. Thus, 2.65 moles * 399.88 g/mol = 1059.68 grams of Fe(SO₄)₃.
c) The number of moles of Fe(SO₄)₃ in 3.45 grams of Fe(SO₄)₃: Using the molar mass of Fe(SO₄)₃, 3.45 g / 399.88 g/mol = 0.00863 moles of Fe(SO₄)₃.
d) The mass in grams of 3 formula unit of Fe(SO₄)₃: The mass of one mole of Fe(SO₄)₃ is 399.88 g. Since one mole contains Avogadro's number (6.022 x 10²³) of formula units, 3 formula units' mass can be calculated as (3 / 6.022 x 10²³) * 399.88 g, which equals approximately 1.99 x 10⁻²² grams of Fe(SO₄)₃.
Assume the diameter of a neutral helium atom is 1.40 × 102 pm. Suppose that we could line up helium atoms side by side in contact with one another. How many atoms would it take to make the distance 6.20 cm from end to end?
Answer:
[tex]4.4285\times 10^8 [/tex] many atoms would it take to make the distance 6.20 cm from end to end.
Explanation:
Diameter of the helium atom = [tex]d=1.40\times 10^2 pm[/tex]
Let the number of atoms required to make the distance 6.20 cm be n.
[tex]d\times n= 6.20 cm =6.20\times 10^{10} pm[/tex]
[tex]1.40\times 10^2 pm\times n=6.20\times 10^{10} pm[/tex]
[tex]n=\frac{6.20\times 10^{10} pm}{1.40\times 10^2 }=4.4285\times 10^8 [/tex]
[tex]4.4285\times 10^8 [/tex] many atoms would it take to make the distance 6.20 cm from end to end.
To find the number of helium atoms needed to span 6.20 cm, convert the atom's diameter to centimeters and divide 6.20 cm by the atom's diameter. After calculation, you will get the number of helium atoms required.
We first need to convert the diameter of a helium atom from picometers to centimeters: 1.40 × 102 pm is equivalent to 1.40 × 10-10 cm. Then, we divide the total length required, 6.20 cm, by the diameter of one helium atom in centimeters to find the number of atoms required:
Number of atoms = Total distance / Diameter of one atom = 6.20 cm / (1.40 × 10-10 cm)
After calculating this expression, we would arrive at the number of helium atoms needed to span the distance of 6.20 cm.
The ionization energies of rubidium and silver are 4.18 and 7.57 eV, respectively. Calculate the ionization energies of an H atom with its electron in the same outermost orbitals as in these two atoms and account for the differences in values in these different elements.
Answer:
0.544 eV; Ag is a smaller atom.
Explanation:
1. Ionization energy of hydrogen
The outermost electrons in Rb and Ag are in 5s orbitals.
The formula for the energy of an electron in a hydrogen atom is
E = -13.6/n² eV
For a hydrogen atom in a 5s orbital,
E = -13.6/5² = -13.6/25 = -0.544 eV
The ionization energy would be 0.544 eV.
2. Rb vs Ag
The first electrons to be removed from Rb and Ag are in 5s orbitals.
The atomic radius of Ag is less than that of Rb because, as you go from left to right across the Row, you are adding 10 protons to the nucleus and 10 electrons to the outer shell.
The added electrons do not effectively shield each other from the attraction of the nucleus, so the 5s electron of Ag is closer in.
It takes more energy to remove the electron from silver, so the ionization energy of Ag is greater than that of Rb.
Rubidium's and silver's higher ionization energies arise from effective nuclear charge, quantum defect, and relativistic effects.
The ionization energies of rubidium and silver are 4.18 and 7.57 eV, respectively. To calculate the ionization energies of an H atom with its electron in the same outermost orbitals as in these two atoms, we must consider the effective nuclear charge experienced by the outermost electron in each atom.
For hydrogen, the ionization energy is given by the formula:
[tex]\[ IE = \frac{13.6 \text{ eV}}{n^2} \][/tex]
where n is the principal quantum number of the electron's orbital.
For rubidium (Rb), the outermost electron is in the 5s orbital, which corresponds to n = 5. Therefore, the ionization energy for a hydrogen-like atom with an electron in the 5s orbital is:
[tex]\[ IE_{\text{H, Rb-like}} = \frac{13.6 \text{ eV}}{5^2} = \frac{13.6 \text{ eV}}{25} \approx 0.544 \text{ eV} \][/tex]
For silver (Ag), the outermost electron is in the 5s orbital as well, which also corresponds to n = 5. Thus, the ionization energy for a hydrogen-like atom with an electron in the 5s orbital is the same as for the rubidium-like case:
[tex]\[ IE_{\text{H, Ag-like}} = \frac{13.6 \text{ eV}}{5^2} = \frac{13.6 \text{ eV}}{25} \approx 0.544 \text{ eV} \][/tex]
However, the actual ionization energies of rubidium and silver are much higher than the calculated values for hydrogen-like atoms because of the following reasons:
1. Penetration Effect:
The inner electrons shield the outermost electron from the nucleus. In a multi-electron atom, the effective nuclear charge [tex](\( Z_{\text{eff}} \))[/tex] is less than the actual nuclear charge due to this shielding.
The outermost electron in rubidium and silver experiences a [tex]\( Z_{\text{eff}} \)[/tex] that is less than the full nuclear charge.
2. Quantum Defect:
The quantum defect accounts for the difference in energy levels between hydrogen-like atoms and many-electron atoms due to the presence of inner electrons.
This defect is more significant for atoms with higher atomic numbers, like silver.
3. Relativistic Effects:
For heavier atoms like silver, relativistic effects become significant.
The mass of the electron increases as it moves at a significant fraction of the speed of light, which increases the electron's binding energy to the nucleus, thus increasing the ionization energy.
4. Full d Subshell:
Silver has a full 4d subshell, which provides additional stability and pulls the 5s orbital closer to the nucleus, increasing the ionization energy.
Due to these effects, the actual ionization energies of rubidium and silver are much higher than those calculated for a hydrogen-like atom.
The differences in values between rubidium and silver are primarily due to the increased nuclear charge, the presence of filled d subshells in silver, and relativistic effects, which are more pronounced in silver due to its higher atomic number.
The depletion of ozone (O3) in the stratosphere has been a matter of great concern among scientists in recent years. It is believed that ozone can react with nitric oxide (NO) that is discharged from the high-altitude jet plane, the SST. The reaction is O3 + NO longrightarrow O2 + NO2 If 0.781 g of O3 reacts with 0.589 g of NO, how many grams of NO2 will be produced?
Answer: 0.736 g
Explanation:
[tex]O_3+NO\rightarrow O_2+NO2[/tex]
To calculate the moles, we use the equation:
[tex]\text{Number of moles}=\frac{\text{Given mass}}{\text{Molar mass}}[/tex]
[tex]\text{Number of moles of}O_3=\frac{0.781g}{48g/mol}=0.016moles[/tex]
[tex]\text{Number of moles of}NO=\frac{0.589g}{30g/mol}=0.019moles[/tex]
By Stoichiometry:
1 mole of ozone [tex]O_3[/tex] reacts with 1 mole of nitric oxide [tex]NO[/tex] to form 1 mole of nitrogen dioxide [tex]NO_2[/tex]
0.016 moles of ozone reacts with=[tex]\frac{1}{1}\times 0.016=0.016moles[/tex] of nitric oxide to form 0.016 mole of [tex]NO_2[/tex]
Thus ozone is the limiting reagent as it limits the formation of products and nitric oxide is the excess reagent as (0.019-0.016) g= 0.003 g remains as such.
Mass of [tex]NO_2=moles\times {\text{Molar mass}}=0.016\times 46=0.736g[/tex]
0.736 g of [tex]NO_2[/tex] will be produced.
0.748 grams of [tex]\( \text{NO}_2 \)[/tex] will be produced when 0.781 grams of [tex]\( \text{O}_3 \)[/tex] reacts with 0.589 grams of NO, as [tex]\( \text{O}_3 \)[/tex] is the limiting reactant.
To determine how many grams of [tex]\( \text{NO}_2 \)[/tex] will be produced from the reaction of [tex]\( \text{O}_3 \)[/tex] with NO, we need to follow these steps:
1. Write the balanced chemical equation:
[tex]\text{O}_3 + \text{NO} \longrightarrow \text{O}_2 + \text{NO}_2[/tex]
2. Calculate the moles of reactants:
Moles of [tex]\( \text{O}_3 \)[/tex]:
[tex]\text{Molar mass of } \text{O}_3 = 3 \times 16.00 \, \text{g/mol} = 48.00 \, \text{g/mol}[/tex]
[tex]\text{Moles of } \text{O}_3 = \frac{0.781 \, \text{g}}{48.00 \, \text{g/mol}} = 0.01627 \, \text{mol}[/tex]
Moles of NO:
[tex]\text{Molar mass of } \text{NO} = 14.01 \, \text{g/mol} + 16.00 \, \text{g/mol} = 30.01 \, \text{g/mol}[/tex]
[tex]\text{Moles of } \text{NO} = \frac{0.589 \, \text{g}}{30.01 \, \text{g/mol}} = 0.01963 \, \text{mol}[/tex]
3. Determine the limiting reactant:
The balanced equation shows that 1 mole of [tex]\( \text{O}_3 \)[/tex] reacts with 1 mole of NO.
Compare the moles of each reactant:
[tex]0.01627 \, \text{mol} \, \text{O}_3 \quad \text{and} \quad 0.01963 \, \text{mol} \, \text{NO}[/tex]
Since [tex]\( \text{O}_3 \)[/tex] has fewer moles, it is the limiting reactant.
4. Calculate the moles of [tex]\( \text{NO}_2 \)[/tex] produced:
From the balanced equation, 1 mole of [tex]\( \text{O}_3 \)[/tex] produces 1 mole of [tex]\( \text{NO}_2 \)[/tex].
Therefore, moles of [tex]\( \text{NO}_2 \)[/tex] produced = moles of [tex]\( \text{O}_3 \)[/tex] reacted:
[tex]\text{Moles of } \text{NO}_2 = 0.01627 \, \text{mol}[/tex]
5. Convert moles of [tex]\( \text{NO}_2 \)[/tex] to grams:
Molar mass of [tex]\( \text{NO}_2 \)[/tex]:
[tex]\text{Molar mass of } \text{NO}_2 = 14.01 \, \text{g/mol} + 2 \times 16.00 \, \text{g/mol} = 46.01 \, \text{g/mol}[/tex]
Grams of [tex]\( \text{NO}_2 \)[/tex]:
[tex]\text{Mass of } \text{NO}_2 = 0.01627 \, \text{mol} \times 46.01 \, \text{g/mol} = 0.748 \, \text{g}[/tex]
Lithium hydrogen carbonate, LiHCO3, decomposes when heated to form Li2O, CO2, and H2O. How many moles of H2O are formed when 0.50 mol LiHCO3 decomposes?
Answer:
0.25 mol of water
Explanation:
The starting point is writing out a balanced chemical equation
[tex]2LiHCO_{3} --->Li_{2}O +2CO_{2} +H_{2}O[/tex]
From here we can see that 2 moles of Lithium hydrogen carbonate produce 1 mole of water. It follows that 0.5 moles of Lithium hydrogen carbonate will produce half of that too, which is 0.25 moles. The ratio is always mantained.
Final answer:
When 0.50 mol of lithium hydrogen carbonate (LiHCO3) decomposes, it produces 0.25 mol of water (H2O).
Explanation:
You asked how many moles of H2O are formed when 0.50 mol LiHCO3 decomposes. The decomposition reaction for LiHCO3 to produce Li2O, CO2, and H2O is:
2 LiHCO3(s) → Li2O(s) + 2 CO2(g) + H2O(g)
According to the balanced equation, 2 moles of LiHCO3 produce 1 mole of H2O. Therefore, when 0.50 mole of LiHCO3 decomposes, you would get half of that ratio in moles of water:
(0.50 mol LiHCO3) / (2 mol LiHCO3) = 0.25 mol H2O
Therefore, the decomposition of 0.50 mol of LiHCO3 will produce 0.25 mol of H2O.
The equilibrium constant, Kc, for the following reaction is 77.5 at 600 K. CO(g) + Cl2(g) COCl2(g) Calculate the equilibrium concentrations of reactant and products when 0.442 moles of CO and 0.442 moles of Cl2 are introduced into a 1.00 L vessel at 600 K. [CO] = M [Cl2] = M [COCl2] = M
To calculate the equilibrium concentrations of reactant and products, we use the equilibrium constant (Kc) and the initial concentrations of the reactants and products. Using the stoichiometry of the reaction, we can determine the change in concentrations. Solve for x in the equilibrium constant expression to find the equilibrium concentrations.
Explanation:To calculate the equilibrium concentrations of reactant and products, we need to use the equilibrium constant (Kc) and the initial concentrations of the reactants and products. In this case, we have 0.442 moles of CO and 0.442 moles of Cl2 in a 1.00 L vessel at 600 K. Using the stoichiometry of the reaction, we can determine the change in concentrations. Let's denote the change in concentration of COCl2 as x.
The initial concentration of CO is [CO] = 0.442 M, so the change in concentration is -x (due to the decrease in CO).
The initial concentration of Cl2 is [Cl2] = 0.442 M, so the change in concentration is -x (due to the decrease in Cl2).
The initial concentration of COCl2 is [COCl2] = 0 M, so the change in concentration is +x (due to the formation of COCl2).
Using the equilibrium constant expression Kc = [COCl2] / ([CO][Cl2]), we can set up the following equation: 77.5 = x / (0.442 * 0.442)
Solving for x, we get x = 0.442 * 0.442 * 77.5 = 15.558 M. Therefore, the equilibrium concentrations are: [CO] = 0.442 - 15.558 = -15.116 M (neglecting the negative sign), [Cl2] = 0.442 - 15.558 = -15.116 M (neglecting the negative sign), and [COCl2] = 15.558 M.
Liquid octane will react with gaseous oxygen to produce gaseous carbon dioxide and gaseous water . Suppose 97. g of octane is mixed with 150. g of oxygen. Calculate the maximum mass of water that could be produced by the chemical reaction. Round your answer to significant digits.
Answer: 61 grams
Explanation:
To calculate the number of moles, we use the equation:
[tex]\text{Number of moles of octane}=\frac{\text{Given mass}}{\text{Molar mass}}=\frac{97g}{114g/mol}=0.85moles[/tex]
[tex]\text{Number of moles of oxygen}=\frac{\text{Given mass}}{\text{Molar mass}}=\frac{150g}{32g/mol}=4.69moles[/tex]
The chemical equation for the combustion of octane in oxygen follows the equation:
[tex]2C_8H_{18}+25O_2\rightarrow 16CO_2+18H_2O[/tex]
By stoichiometry of the reaction;
25 moles of oxygen react with 2 moles of octane
4.69 moles of oxygen react with=[tex]\frac{2}{25}\times 4.69=0.37[/tex] moles of octane
Thus, oxygen is the limiting reagent as it limits the formation of product and octane is the excess reagent.
25 moles of oxygen produce 18 moles of water
4.69 moles of oxygen produce=[tex]\frac{18}{25}\times 4.69=3.38[/tex] moles of water.
Mass of water produced=[tex]moles\times {\text{Molar mass}}=3.38\times 18g/mol=61g[/tex]
The maximum mass of water that could be produced by the chemical reaction is 61 grams.
To determine the maximum mass of water produced from the combustion of octane, one must first calculate the moles of octane and water using the balanced chemical equation. The stoichiometry shows that for every 2 moles of octane, 18 moles of water are produced. The final mass of water is calculated by considering the limiting reagent, which could be either octane or oxygen.
Explanation:To calculate the maximum mass of water that could be produced from the combustion of octane, we should start with the balanced chemical equation for octane (C8H18):
2 C8H18(l) + 25 O2(g) → 16 CO2(g) + 18 H2O(g)
First, we determine the moles of octane based on the given mass:
Mass of octane = 97.0 gMolar mass of octane = 114.23 g/molMoles of octane = Mass / Molar mass = 97.0 g / 114.23 g/molNext, we calculate the moles of water produced per mole of octane using the stoichiometry of the reaction:
From the equation, 2 moles of octane produce 18 moles of water.Thus, 1 mole of octane will produce 18 / 2 = 9 moles of water.Now, we find the mass of water produced using the moles of octane we calculated:
Molar mass of water = 18.02 g/molMaximum moles of water = Moles of octane × 9Maximum mass of water = Maximum moles of water × Molar mass of waterFinally, we check if oxygen is the limiting reagent by comparing moles of oxygen provided with the moles required based on the moles of octane we have. To calculate this, use the molar mass of oxygen (O2) which is 32.00 g/mol and the stoichiometry of the equation. If the available moles of oxygen are less than required, we must recalculate the maximum mass of water based on the moles of the limiting reagent (oxygen).
Note that we haven't provided actual numerical results, and you will need to perform the calculations to find the maximum mass of water that can be produced. Remember to round your final answer to the correct number of significant digits based on the given data in the question.
A scientist wants to make a solution of tribasic sodium phosphate, Na3PO4, for a laboratory experiment. How many grams of Na3PO4 will be needed to produce 375 mL of a solution that has a concentration of Na+ ions of 1.50 M ?
The mass of sodium phosphate needed to make 375 mL of a solution with a molarity of sodium ions of 0.900 M is indeed 18.45 grams.
Given:
Volume of solution (V) = 375 mL = 0.375 L
Molarity of sodium ions (c) = 0.900 M
Using the formula for molarity: c = n/V
Since each mole of sodium phosphate produces 3 moles of sodium ions:
Effective molarity of sodium phosphate solution = c / 3 = 0.300 M
Number of moles of sodium phosphate (n) = c * V = 0.300 M * 0.375 L = 0.1125 mol
Molar mass of sodium phosphate (M) = 164 g/mol
Mass of sodium phosphate (m) = n * M = 0.1125 mol * 164 g/mol = 18.45 g
Therefore, the mass of sodium phosphate needed to make 375 mL of a solution with a molarity of sodium ions of 0.900 M is indeed 18.45 grams.
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To make a solution of tribasic sodium phosphate with a concentration of 1.50 M Na+ ions in 375 mL, you will need 276.38 grams of Na3PO4.
Explanation:To calculate the grams of Na3PO4 needed, we need to use the equation relating moles, volume, and concentration:
Moles of Na+ ions = Molarity of Na+ ions x Volume of solution (in L)
Moles of Na3PO4 = 3 x Moles of Na+ ions
First, convert the volume in mL to L (375 mL = 0.375 L). Then, substitute the values into the equation:
Moles of Na+ ions = 1.50 M x 0.375 L = 0.5625 mol
Moles of Na3PO4 = 3 x 0.5625 mol = 1.6875 mol
Finally, convert moles to grams using the molar mass of Na3PO4 (163.94 g/mol):
Mass of Na3PO4 = 1.6875 mol x 163.94 g/mol = 276.38 g
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What mass of Cu(s) would be produced if 0.40 mol of Cu2O(s) was reduced completely with excess H2(g) ?
Answer:
50.8g
Explanation:
Given parameters:
Nubmer of mole of Cu₂O = 0.4mol
Unknown:
Mass of Cu produced = ?
Solution:
The balanced reaction equation:
Cu₂O + H₂ ⇄ 2Cu + H₂O
From the reaction, we know that:
1 mole of Cu₂O produced 2 moles of Cu
0.4 mol of Cu₂O would give 0.8mol of Cu
Now we know the number of moles of Cu produced because the limiting reactant here is Cu₂O. It was used up in the reaction in which the hydrogen gas was in excess.
To find the mass of Cu produced, we use the equation below :
Mass of Cu = Number of moles of Cu x molar mass of Cu
Molar mass of Cu = 63.5gmol⁻¹
Mass of Cu = 0.8 x 63.5 = 50.8g
If [tex]0.40[/tex] mol of [tex]Cu_2O(s)[/tex] is reduced completely with excess [tex]H_2(g)[/tex], approximately [tex]50.84[/tex] grams of [tex]Cu(s)[/tex] would be produced.
The balanced chemical equation for the reduction of [tex]Cu_2O(s)[/tex] with [tex]H_2(g)[/tex] is:
[tex]\[ \text{Cu}_2\text{O}(s) + \text{H}_2(g) \rightarrow \text{Cu}(s) + \text{H}_2\text{O}(l) \][/tex]
From the balanced equation, we can see that [tex]1[/tex] mole of [tex]Cu_2O[/tex] produces [tex]2[/tex] moles of [tex]Cu[/tex].
Given that we have [tex]0.40[/tex] mol of [tex]Cu_2O[/tex], we can use the stoichiometry of the reaction to find the amount of [tex]Cu[/tex] produced:
[tex]\[ \text{mol of Cu} = 0.40 \, \text{mol Cu}_2\text{O} \times \frac{2 \, \text{mol Cu}}{1 \, \text{mol Cu}_2\text{O}} \][/tex]
[tex]\[ \text{mol of Cu} = 0.40 \times 2 \][/tex]
[tex]\[ \text{mol of Cu} = 0.80 \, \text{mol} \][/tex]
Now, we need to convert the moles of [tex]Cu[/tex] to grams using the molar mass of copper ([tex]Cu[/tex]), which is approximately [tex]63.55 g/mol[/tex]
[tex]\[ \text{mass of Cu} = \text{mol of Cu} \times \text{molar mass of Cu} \][/tex]
[tex]\[ \text{mass of Cu} = 0.80 \, \text{mol} \times 63.55 \, \text{g/mol} \][/tex]
[tex]\[ \text{mass of Cu} = 50.84 \, \text{g} \][/tex]
Antacids, such as Alka-Seltzer, use the reaction of sodium bicarbonate with citric acid in water solution to produce a fizz as follows: 3NaHCO3 + C6H8O7 → 3CO2 + 3H2O + Na3C6H5O7 If 4.11 g of the citric acid (C6H8O7, MW = 192 g/mol) react with excess sodium bicarbonate (NaHCO3), how many grams of carbon dioxide (CO2, MW = 44 g/mol) are formed as the solution fizzes?
When 4.11 g of citric acid reacts with sodium bicarbonate, 2.82 g of carbon dioxide gas is produced according to the provided chemical reaction.
Explanation:In the given chemical reaction, 3NaHCO3 + C6H8O7 → 3CO2 + 3H2O + Na3C6H5O7, specifically between sodium bicarbonate and citric acid, it's clear that for every one molecule of citric acid, three molecules of carbon dioxide are formed. Given that you have 4.11 g of citric acid, and knowing that the molecular weight of citric acid is 192 g/mol, first we calculate the number of moles of citric acid by dividing the mass by the molecular weight: 4.11 g/192 g/mol = 0.0214 moles. Since each mole of citric acid react to produce 3 moles of carbon dioxide, then 0.0214 moles of citric acid would produce 0.0214 moles x 3 = 0.0642 moles of CO2. To find the mass of CO2 formed (since its molar mass is 44 g/mol), multiply the resulting moles of CO2 by its molar mass: 0.0642 moles x 44 g/mol = 2.82 g. Therefore, when 4.11 g of citric acid reacts with sodium bicarbonate, 2.82 g of carbon dioxide will form.
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Give the percentage and whether w/w, w/v, or v/v of the following: 10g of NaoH + 90g solvent.
Answer:
The w/w 5 of the solution is 10 %.
Explanation:
w/w % : The percentage mass or fraction of mass of the of solute present in total mass of the solution.
[tex]w/w\%=\frac{\text{Mass of solute}}{\text{Mass of solution}}\times 100[/tex]
w/v %: The percentage of mass of the of solute present in total volume of the solution.
[tex]w/v\%=\frac{\text{Mass of solute}}{\text{Volume of solution}}\times 100[/tex]
v/v % : The percentage volume of the of solute present in total volumeof the solution.
[tex]v/v\%=\frac{\text{Volume of solute}}{\text{Volume of solution}}\times 100[/tex]
Mass of solution = Mass of solute + Mass of solvent
Mass of solute= 10 g of NaOH
Mass of solvent = 90 g
Mass of solution = 10 g + 90 g = 100 g
[tex]w/w\%=\frac{10 g}{100 g}\times 100 =10\%[/tex]
The w/w 5 of the solution is 10 %.
Given the following compounds and their vapor pressures (VP). Arrange them in increasing (lowest to highest) order of boiling points.ethane (C2H6); VP= 841 mm Hgpentane (C5H12); VP=420 mm Hgisopropyl alcohol (C3H5OH); VP=31.5 mm Hgacetone (C3H6O); VP=185 mm HgIsopropyl alcohol < acetone < pentane < ethaneEthane < pentane < isopropyl alcohol < acetoneEthane < pentane < acetone < isopropyl alcoholAcetone < isopropyl alcohol < pentane < ethaneThe strength of the intermolecular forces is also needed to determine the order.
Answer:
Increasing order of boiling point
isopropyl alcohol > acetone > pentane > ethane
Explanation:
Vapor pressure - the pressure exerted the gaseous molecules , on the walls of the container is called the vapor pressure.
Boiling point - the temperature at which the the vapor pressure of the liquid equals the external atmospheric pressure.
Both boiling point and vapor pressure are linked by the inter molecular forces between the atoms.
The compound with stronger inter molecular forces are tightly held , hence more amount of energy is required to vaporize. Therefore, higher boiling point , and in turn the vapor pressure will be lower .
And the compound with weaker inter molecular forces are loosely held , hence less amount of energy is required to vaporize. Therefore, lower boiling point , and in turn the vapor pressure will be higher .
Therefore,
The vapor pressure and boiling point will have an inverse relation.
Given , The vapor pressure of the compound in increasing order -
isopropyl alcohol < acetone < pentane < ethane .
Hence, the order of boiling point will be exactly reverse.
So , the Increasing order of boiling point,
isopropyl alcohol > acetone > pentane > ethane
When silver nitrate reacts with barium chloride, silver chloride and barium nitrate are formed. How many grams of silver chloride are formed when 10.0 g of silver nitrate reacts with 15.0 g of barium chloride? When silver nitrate reacts with barium chloride, silver chloride and barium nitrate are formed. How many grams of silver chloride are formed when 10.0 g of silver nitrate reacts with 15.0 g of barium chloride? 18.8 g 8.44 g 11.9 g 9.40 g
Answer : The mass of silver chloride formed are, 8.44 grams.
Explanation : Given,
Mass of [tex]AgNO_3[/tex] = 10.0 g
Mass of [tex]BaCl_2[/tex] = 15.0 g
Molar mass of [tex]AgNO_3[/tex] = 169.87 g/mole
Molar mass of [tex]BaCl_2[/tex] = 208.23 g/mole
Molar mass of [tex]AgCl[/tex] = 143.32 g/mole
First we have to calculate the moles of [tex]AgNO_3[/tex] and [tex]BaCl_2[/tex].
[tex]\text{Moles of }AgNO_3=\frac{\text{Mass of }AgNO_3}{\text{Molar mass of }AgNO_3}=\frac{10g}{169.87g/mole}=0.0589moles[/tex]
[tex]\text{Moles of }BaCl_2=\frac{\text{Mass of }BaCl_2}{\text{Molar mass of }BaCl_2}=\frac{15g}{208.23g/mole}=0.072moles[/tex]
Now we have to calculate the limiting and excess reagent.
The balanced chemical reaction is,
[tex]2AgNO_3+BaCl_2\rightarrow 2AgCl+Ba(NO_3)2[/tex]
From the balanced reaction we conclude that
As, 2 moles of [tex]AgNO_3[/tex] react with 1 mole of [tex]BaCl_2[/tex]
So, 0.0589 moles of [tex]AgNO_3[/tex] react with [tex]\frac{0.0859}{2}=0.0295[/tex] moles of [tex]BaCl_2[/tex]
From this we conclude that, [tex]BaCl_2[/tex] is an excess reagent because the given moles are greater than the required moles and [tex]AgNO_3[/tex] is a limiting reagent and it limits the formation of product.
Now we have to calculate the moles of [tex]AgCl[/tex].
As, 2 moles of [tex]AgNO_3[/tex] react to give 2 moles of [tex]AgCl[/tex]
So, 0.059 moles of [tex]AgNO_3[/tex] react to give 0.059 moles of [tex]AgCl[/tex]
Now we have to calculate the mass of [tex]AgCl[/tex].
[tex]\text{Mass of }AgCl=\text{Moles of }AgCl\times \text{Molar mass of }AgCl[/tex]
[tex]\text{Mass of }AgCl=(0.0589mole)\times (143.32g/mole)=8.44g[/tex]
Therefore, the mass of silver chloride formed are, 8.44 grams.
The mass of silver chloride (AgCl) formed when 10.0 g of silver nitrate reacts with 15.0 g of barium chloride is 8.44 g. The correct option is the second option 8.44 g
First, we will write a balanced chemical equation for the reaction between silver nitrate and barium chloride
2AgNO₃ + BaCl₂ → 2AgCl + Ba(NO₃)₂
This means, 2 moles of AgNO₃ will react with 1 mole of BaCl₂ to produce 2 moles of AgCl and 1 mole of Ba(NO₃)₂
From the question,
10.0 g of silver nitrate reacts with 15.0 g of barium chloride
First, we will determine the number of moles present in each reactant
For silver nitrate (AgNO₃)Mass = 10.0 g
Molar mass = 169.87 g/mol
Using the formula
[tex]Number \ of \ moles = \frac{Mass}{Molar \ mass}[/tex]
Then,
[tex]Number \ of\ moles\ of\ silver\ nitrate = \frac{10.0}{169.87}[/tex]
Number of moles of AgNO₃ = 0.05887 moles
For Barium chloride (BaCl₂)Mass = 15.0 g
Molar mass of BaCl₂ = 208.23 g/mol
∴ [tex]Number \ of\ moles\ of\ barium \ chloride= \frac{15.0}{208.23}[/tex]
Number of moles of BaCl₂ = 0.072036 moles
From the balanced chemical equation
2 moles of AgNO₃ will react with 1 mole of BaCl₂
∴ 0.05887 moles AgNO₃ will react with [tex]\frac{0.05887}{2}[/tex] mole of BaCl₂
[tex]\frac{0.05887}{2} = 0.029435[/tex]
This means only 0.029435 moles of BaCl₂ will react
(NOTE: AgNO₃ is the limiting reagent while BaCl₂ is the excess reagent)
Now,
Since 2 moles of AgNO₃ will react with 1 mole of BaCl₂ to produce 2 moles of AgCl
That means,
0.05887 moles AgNO₃ will react with 0.029435 moles of BaCl₂ to produce 0.05887 moles of AgCl
∴ The number of moles of silver chloride (AgCl) produced is 0.05887 moles
Now, to determine the mass (in grams) of silver chloride that are formed
From the formula,
Mass = Number of moles × Molar mass
Molar mass of AgCl = 143.32 g/mol
∴ Mass of silver chloride, AgCl, formed = 0.05887 moles × 143.32 g/mol
Mass of silver chloride formed = 8.4372484 g
Mass of silver chloride formed ≅ 8.44 g
Hence, the mass of silver chloride (AgCl) formed when 10.0 g of silver nitrate reacts with 15.0 g of barium chloride is 8.44 g. The correct option is the second option 8.44 g
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Two compounds with general formulas A2X and AX3 have Ksp=1.5×10−5M. Part A Which of the compounds has the higher molar solubility? Which of the compounds has the higher molar solubility? A2X AX3
Hey there!:
To get to the molar solubility from the Ksp, you have to think about the how Ksp is calculated, and what it means.
For a compound that forms 2 ions, Ksp = X^2 where X is the molar solubility. For a compound that forms 3 ions, Ksp = 4X^3, where again, X is the molar solubility.
If you calculate the molar solubilities of each of your compounds, you will see that A2X has the higher molar solubilty
Hope this helps!
Answer:
A₃X
Explanation:
In order to find the molar solubility (S) of a compound, we will use an ICE Chart.
A₂X
Let's consider the solution of A₂X.
A₂X(s) ⇄ 2 A⁺(aq) + X²⁻(aq)
I 0 0
C +2S +S
E 2S S
The solubility product (Kps) is:
Kps = 1.5 × 10⁻⁵ = [A⁺]².[X²⁻] = (2S)².S = 4S³
S = 0.016 M
A₃X
Let's consider the solution of A₃X.
A₃X ⇄ 3 A⁺(aq) + X³⁻(aq)
I 0 0
C +3S +S
E 3S S
The solubility product (Kps) is:
Kps = 1.5 × 10⁻⁵ = [A⁺]³.[X³⁻] = (3S)³.S = 27 S⁴
S = 0.027 M
A₃X has a higher molar solubility than A₂X.
The reform reaction between steam and gaseous methane (CH4) produces "synthesis gas," a mixture of carbon monoxide gas and dihydrogen gas. Synthesis gas is one of the most widely used industrial chemicals, and is the major industrial source of hydrogen.
Suppose a chemical engineer studying a new catalyst for the reform reaction finds that 924. liters per second of methane are consumed when the reaction is run at 261.°C and 0.96atm. Calculate the rate at which dihydrogen is being produced. Give your answer in kilograms per second. Round your answer to 2 significant digits.
Answer:
The rate at which dihydrogen is being produced is 0.12 kg/sec.
Explanation:
[tex]CH_4+H_2O\rightarrow CO+3H_2[/tex] Haber reaction
Volume of methane consumed in a second = 924 L
Temperature at which reaction is carried out,T= 261°C = 538.15 K
Pressure at which reaction is carried out, P = 0.96 atm
Let the moles of methane be n.
Using an Ideal gas equation:
[tex]PV=nRT[/tex]
[tex]n=\frac{PV}{RT}=\frac{0.96 atm\times 924 L}{0.0821 atm l/mol K\times 538.15 K}=20.0769 mol[/tex]
According to reaction , 1 mol of methane gas produces 3 moles of dihydrogen gas.
Then 20.0769 mol of dihydrogen will produce :
[tex]\frac{3}{1}\times 20.0769 mol=60.2307 mol[/tex] of dihydrogen
Mass of 24.3194 moles of ammonia =24.3194 mol × 2 g/mol
=120.46 g=0.12046 kg ≈ 0.12 kg
924 L of methane are consumed in 1 second to produce 0.12 kg of dihydrogen in 1 second. So the rate at which dihydrogen is being produced is 0.12 kg/sec.
How many moles of oxygen are formed when 58.6 g of KNO3 decomposes according to the following reaction? 4 KNO3(s) → 2 K2O(s) + 2 N2(g) + 5 O2(g)
Answer:
0.725 mol
Explanation:
Moles are calculated as the given mass divided by the molecular mass.
i.e. ,
moles = ( mass / molecular mass )
since,
mass of KNO₃ = 58.6 g ( given )
Molecular mass of KNO₃ = 101 g / mol
Therefore,
moles of KNO₃ = 58.6 g / 101 g / mol
moles of KNO₃ = 0.58 mol
From the balanced reaction ,
4 KNO₃ (s) ---> 2K₂O (s) + 2N₂ (g) + 5O₂ (g)
By the decomposition of 4 mol of KNO₃ , 5 mol of O₂ are formed ,
hence, unitary method is used as,
1 mol of KNO₃ gives 5 / 4 mol O₂
Therefore,
0.58 mol of KNO₃ , gives , 5 / 4 * 0.58 mol of O₂
Solving,
0.58 mol of KNO₃ , gives , 0.725 mol of O₂
Therefore,
58.6g of KNO₃ gives 0.725 mol of O₂.
The titration of 10.00 mL of an HCl solution of unknown concentration requires 120.54 mL of a 0.100 M NaOH solution to reach the equivalence point. What is the concentration of the unknown HCl solution?
Answer:
Concentration of HCl is 1.2054 M
Explanation:
Acid-base titration is a type of qualitative analysis in which the concentration of the unknown acid/base is determined by treating it with a known concentration of base/acid. Indicators are used to determine the end point or the equivalence point (when all the acid/base is neutralized by base/acid).
At the end point,
Moles of acid = Moles of base
Since,
Molarity of a solution is given by the moles of solute per liter of the solution
i.e.,
Molarity = moles of solute / volume of solution (in L)
moles = Molarity * Volume
moles = M * V
M₁V₁ ( acid )= M₂V₂( base )
Where,
M₁ is the molarity of the acid
V₁ is the volume of the acid
M₂ is the molarity of the base
V₂ is the total volume of the base
From the question,
M₁ = ?
M₂ = 0.100 M
V₁ = 10.00 mL
V₂ = 120.54 mL
Using the above mentioned formula
M₁V₁ ( acid )= M₂V₂( base )
M₁ * 10.00mL = 0.100 M * 120.54 mL
M₁ = 1.2054 M
Hence, the concentration of of HCl is 1.2054 M
The concentration of the HCl solution is calculated by the formula c1v1 = c2v2, deriving from the one-to-one reaction between NaOH and HCl. The resulting concentration of the HCl solution is determined to be 1.21 M.
Explanation:The subject of this question is a chemistry concept related to acid-base titration. In this context, you're given that 10.00 mL of an HCl solution is titrated with 120.54 mL of a 0.100 M NaOH solution to reach the equivalence point. From this, we can figure out the concentration of the unknown HCl solution using the formula c1v1 = c2v2, where c represents concentration and v represents volume. The reaction between NaOH and HCl is one-to-one, so the number of moles of NaOH that react will be equal to the number of moles of HCl initially present in the solution.
To calculate the number of moles of NaOH used in the reaction, you multiply the volume of NaOH solution used (in liters) by its molarity. Here, that is (120.54 mL / 1000 mL/L) * 0.100 mol/L = 0.012054 mol NaOH. Since the moles of NaOH must equal the moles of HCl, the molarity (M) of the HCl solution is the moles of HCl divided by the volume of HCl solution in liters. Therefore, the concentration of HCl is 0.012054 mol / (10.00 mL / 1000 mL/L) = 1.21 M.
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A pressure gauge on a welder's tank gives a reading of barometric pressure is 28.6 in Hg. Calculate the absolute pressure in the tank in 1. Ib/ft 2. in Hg 8
Hey there!:
1 in. Hg = 0.4911 psi
=> Absolute pressure in psi = 22.4 + 28.6 x 0.4911 = 36.445 psi
a) 1 psi = 144 lb/ft²
36.445 psi = 5248.15 lb/ft²
b) 1 psi = 2.036 in. Hg
36.445 psi = 74.21 in. Hg
Hope this helps!
1 in. Hg = 0.4911 psi
Absolute pressure in psi = 22.4 + 28.6 x 0.4911 = 36.445 psi
a) 1 psi = 144 lb/ft²
36.445 psi = 5248.15 lb/ft²
b) 1 psi = 2.036 in. Hg
36.445 psi = 74.21 in. Hg
What is effect of pressure on rate of reaction?Pressure plays a important role in rate of reaction to increase the pressure it increases the rate of reaction by increasing the collision.Pressure increase the concentration of gases it means that it increases the number of molecules per unit volume due to this collision of gases increases this will increase the temperature.
This increase of temperature will increase the rate of reaction. So we can say that the increases of pressure will increase the rate of reaction. Density is defined as the mass per unit volume it means that mass present in 1 meter cube is called density. The S.I unit of density is kg/m^3 and in C.G.S it is gram/cm^3
So In above statement we can understand that density, mass, and volume all are convert to each other it means that if we know any two variable then third one will be calculated easily.
Therefore, a) 1 psi = 144 lb/ft²
36.445 psi = 5248.15 lb/ft²
b) 1 psi = 2.036 in. Hg
36.445 psi = 74.21 in. Hg
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Be sure to answer all parts. When baking soda (sodium bicarbonate or sodium hydrogen carbonate, NaHCO3) is heated, it releases carbon dioxide gas, which is responsible for the rising of cookies, donuts, and bread. Write a balanced equation for the decomposition of the compound (one of the three products is Na2CO3). Do not include states of matter in your balanced equation. Calculate the mass of NaHCO3 required to produce 27.0 g of CO2. g NaHCO3
Answer: 1. [tex]2NaHCO_3\rightarrow Na_2CO_3+CO_2+H_2O[/tex]
2. 100.8 grams
Explanation:
According to the law of conservation of mass, mass can neither be created nor be destroyed. Thus the mass of products has to be equal to the mass of reactants. The number of atoms of each element has to be same on reactant and product side. Thus chemical equations are balanced.
Balanced equation for the decomposition of the compound sodium hydrogen carbonate is:
[tex]2NaHCO_3\rightarrow Na_2CO_3+CO_2+H_2O[/tex]
According to avogadro's law, 1 mole of every substance weighs equal to its molecular mass and contains avogadro's number [tex]6.023\times 10^{23}[/tex] of particles.
moles of [tex]CO_2=\frac{\text {given mass}}{\text {molar mass}}=\frac{27.0g}{44g/mol}=0.6moles[/tex]
According to stoichiometry:
1 mole of [tex]CO_2[/tex] is produced from 2 moles of [tex]NaHCO_3[/tex]
Thus 0.6 moles of [tex]CO_2[/tex] is produced from =[tex]\frac{2}{1}\times 0.6=1.2[/tex] moles of [tex]NaHCO_3[/tex]
Mass of [tex]NaHCO_3=moles\times {\text {Molar mass}}=1.2\times 84=100.8g[/tex]
Thus the mass of [tex]NaHCO_3[/tex] required to produce 27.0 g of [tex]CO_2[/tex] is 100.78 grams.
The balanced equation for the decomposition of sodium bicarbonate is 2 NaHCO3 → Na2CO3 + CO2 + H2O. To produce 27.0 g of CO2, you would need approximately 51.0 g of NaHCO3.
Explanation:The balanced chemical equation for the decomposition of sodium bicarbonate or baking soda is 2 NaHCO3 → Na2CO3 + CO2 + H2O. When heated, sodium bicarbonate decomposes into sodium carbonate, carbon dioxide, and water. This CO2 is what makes baked goods rise.
To calculate the mass of NaHCO3 required to produce 27.0 g of CO2, we use molar mass and stoichiometry. The molar mass of NaHCO3 is about 84 g/mol, and that of CO2 is about 44 g/mol. Since the reaction produces one mole of CO2 for every two moles of NaHCO3, we can set up the equation: (27g CO2 / 44 g/mol CO2) * (2 mol NaHCO3 / 1 mol CO2) * (84 g NaHCO3 / 1 mol NaHCO3) = 51.0 g NaHCO3
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An analytical balance was used to weigh 200.01 mg of dry solid sodium acetate {NaC2H3O2 ~ NaAc MW = 82.0343, pKa (HC2H3O2 ~ HAc) = 4.76} which was transferred to a 100.00 mL volumetric flask that was then filled to the line with carbonate-free water and mixed well. Determine the pH of each of the solutions below.
A.) The original sodium acetate solution
B.) A 25.00 mL aliquot of the NaAc solution plus 25.00 mL of 0.100 M aqueous acetic acid (HAc) solution
C.) A 25.00 mL aliquot of the NaAc solution plus 15.00 mL of 0.100 M aqueous hydrogen chloride solution