Answer:
1.6 ×[tex]10^{-7}[/tex]M
Explanation:
[tex]K_{sp}[/tex] for calcium diphosphate is 8.64x10^(-13)
concentration of the calcium cations = 2.2955 x 10^−3M
[tex]Ca_{2}P_{2} O_{7}_(s)[/tex] ⇄[tex]2Ca_{2}_(aq)[/tex] + [tex]P_{2}O^{4-} _{7}_(aq)[/tex]
[tex]K_{sp}[/tex] = [tex][Ca^{2+}]^{2}[/tex]×[tex][P_{2} O^{4-}_7][/tex]
converting the concentration of the calcium cations from 9.2mg/dL to moles per liter , we get 2.2955 x [tex]10^{-3}[/tex]M
[tex][P_{2} O^{4-}_7][/tex] = [tex]\frac{K_{sp} }{[Ca^{2+}]^{2} }[/tex]
[tex][P_{2} O^{4-}_7][/tex] = [tex]\frac{8.64 . 10^{-13} }{[2.2955 . 10^{-3}]^{2} }[/tex]
=1.6 ×[tex]10^{-7}[/tex]M
Specific heat is used to explain why different substances
a) sink or float
b) change temp. at different rates
c) vaporize or condense at different temp.’s
d) melt and freeze at the same temp.
Answer:
change temperature at different rates
The specific heat is used to explain why different substances change the temperature at different rates.
Specific Heat:
It is the amount of heat that is required to increase the temperature of 1 kg of a substance by 1^oc. It is measured in the [tex]\bold {J/g/^oC }[/tex].
The specific heat capacity of water is [tex]\bold { 4.184 J/g/^oC.}[/tex]If the heat capacity is it takes more time to heat or cool it down. If specific heat capacity of a substance is low, then it takes less time to heat or cool it down.Therefore, the specific heat is used to explain why different substances change the temperature at different rates.
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What is the only force that acts between particles of helium gas?
Answer: The only force that acts between particles of helium gas is Vanderwaal forces.
Explanation:
When molecules are uncharged in nature but still combined together due to the dipole moment of elements then this force holding the molecules together is known as Vanderwaal forces.
This force is weak in nature.
For example, particles of helium gas has Vanderwaal force between its atoms.
Thus, we can conclude that the only force that acts between particles of helium gas is Vanderwaal forces.
14.2 grams of Na2 so4 is dissolved in water to make a 2.50 L solution.What is molarity of solution?
Answer:
The answer to your question is 0.04 M
Explanation:
Data
mass of Na₂SO₄ = 14.2 g
volume = 2.50 l
Molarity = ?
Process
1.- Calculate the molar mass of Na₂SO₄
Na₂SO₄ = (23 x 2) + (32 x 1) + (16 x 4) = 46 + 32 + 64 = 142 g
2.- Calculate the number of moles of Na₂SO₄
142 g of Na₂SO₄ ------------------- 1 mol
14.2 g of Na₂SO₄ ------------------ x
x = (14.2 x 1) / 142
x = 0.1 moles
3.- Calculate the molarity
Molarity = moles /volume
-Substitution
Molarity = 0.1 / 2.5
-Result
Molarity = 0.04
It is common for students to overshoot the endpoint, meaning they add too much NaOH(aq) from the buret, which causes the solution to turn bright pink. What specific impact does this mistake have on the percent of acetic acid result?
Answer: the percentage of acetic acid will be low.
Explanation: The major aim during titration of acids and bases is to determine the endpoint , that is exact point where the acid in the beaker changes colour, (in this case, pink )with an additional drop from the burette containing the base, since it is usually difficult to mark the equivalence point that tells us when all the substrate in the beaker has been neutralized completely with the buretted substance.
Overshooting the end point is an error which can occur when the person involved in the the titration accidently goes beyond this endpoint by adding too much of the substance(base) from the burette into the beaker missing the exact endpoint.
This implies that the person has added too much of the burreted liquid, ie the base than required , making the acid in the beaker to continue to react resulting to a lower concentration of the acid (acetic acid) with excess base.(NaOH)
What type of reaction occurs between amines and carboxylic acids at room temperature?
Answer:
Acid-base equilibrium.
Explanation:
At low temperatures the amines react with carboxylic acids as bases and not as nucleophiles. This acid-base reaction is disadvantageous on heating, with the nucleophilic attack that will form the amide prevailing under these conditions.
Of the reactions below, which one is not a combination reaction?Immersive Reader (2 Points) 2N2 + 3H2 → 2NH3 2Mg + O2 → 2MgO 2CH4 + 4O2 → 2CO2 + 4H2O C + O2 → CO2 CaO + H2O → Ca(OH)2
Answer: [tex]2CH_4+4H_2O\rightarrow 2CO_2+4H_2O[/tex] is not a combination reaction.
Explanation:
Synthesis reaction or combination reaction is defined as the reaction where two or more substances combine to form a single product.
[tex]2N_2+3H_2\rightarrow 2NH_3[/tex]
[tex]2Mg+O_2\rightarrow 2MgO[/tex]
[tex]CaO+H_2O\rightarrow Ca(OH)_2[/tex]
Combustion is a chemical reaction in which hydrocarbons are burnt in the presence of oxygen to give carbon dioxide and water.
[tex]2CH_4+4H_2O\rightarrow 2CO_2+4H_2O[/tex]
Among the provided reactions, the reaction 2CH4 + 4O2 → 2CO2 + 4H2O is not a combination reaction, but rather a combustion reaction.
Explanation:In the given reactions, the reaction 2CH4 + 4O2 → 2CO2 + 4H2O is not a combination reaction. In a combination reaction, two or more substances (either elements or compounds) combine to form a single compound. However, the mentioned reaction is actually an example of a combustion reaction where methane (CH4) undergoes combustion in the presence of oxygen (O2) to form carbon dioxide (CO2) and water (H2O).
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Nascar fans love race day when they get a chance to cheer on there favorite racer if a driver was able to travel 600 miles in 3 hours what was his average speed ( in miles per hour
Answer:
200 mph
Explanation:
600/3=200
What is the best method for removing water from a hydrated compound?
Answer:
Heating is the best method
Explanation:
When a mass of crystals containing Water of crystallization is heated sufiiciently to a high temperature, water vapor may be driven off the crystals by the action of heat alone.
Answer:
Heating to remove water of crystallizationPassing through a drying agent (deliquescent or hygroscopic substances)Explanation:
If solid/crystals, compound can be dried by applying heat to remove the water of crystallization.
Drying agents are also utile in removing moisture from compounds in a dessicator. Substances which absorb water from air can be used as drying agents for gases. For instance, [tex]CaCl_{2}[/tex], CaO or silica gel is suitable for drying gases, depending on reactivity of the substance.
How much heat is required to vaporize a 3 g ice cube initially at 0◦C? The latent heat of fusion of ice is 80 cal/g and the latent heat of vaporization of water is 540 cal/g. The specific heat of water is 1 cal/(g · ◦ C). Answer in units of cal.
Answer : The amount of heat required is, 2160 cal.
Explanation :
The process involved in this problem are :
[tex](1):H_2O(s)(0^oC)\rightarrow H_2O(l)(0^oC)\\\\(2):H_2O(l)(0^oC)\rightarrow H_2O(l)(100^oC)\\\\(3):H_2O(l)(100^oC)\rightarrow H_2O(g)(100^oC)[/tex]
The expression used will be:
[tex]Q=[m\times \Delta H_{fusion}]+[m\times c_{p,l}\times (T_{final}-T_{initial})]+[m\times \Delta H_{vap}][/tex]
where,
[tex]Q[/tex] = heat required for the reaction = ?
m = mass of ice = 3 g
[tex]c_{p,l}[/tex] = specific heat of liquid water = [tex]1cal/g^oC[/tex]
[tex]\Delta H_{fusion}[/tex] = enthalpy change for fusion = [tex]80cal/g[/tex]
[tex]\Delta H_{vap}[/tex] = enthalpy change for vaporization = [tex]540cal/g[/tex]
Now put all the given values in the above expression, we get:
[tex]Q=[3g\times 80cal/g]+[3g\times 1cal/g^oC\times (100-0)^oC]+[3g\times 540cal/g][/tex]
[tex]Q=2160cal[/tex]
Therefore, the amount of heat required is, 2160 cal.
To vaporize a 3 g ice cube initially at 0°C, a total heat of 2160 cal is required. This includes the heat required to melt the ice, heat the melted ice to water's boiling point, and vaporize the water.
Explanation:The process to vaporize a 3 g ice cube at 0°C consists of three steps. First, the ice cube needs to melt. This requires an amount of heat given by Q = mass x latent heat of fusion. i.e., Q = 3 g x 80 cal/g = 240 cal.`
Then, the water obtained from melted ice at 0°C needs to be heated up to 100°C. The required heat is Q = mass x specific heat x ΔT, i.e., Q = 3 g x 1 cal/g°C x (100°C-0°C) = 300 cal.
Finally, the 100°C water needs to be vaporized. This requires an amount of heat given by Q = mass x latent heat of vaporization. i.e., Q = 3 g x 540 cal/g = 1620 cal.
So, the total heat required to vaporize a 3 g ice cube initially at 0°C is 240 cal + 300 cal + 1620 cal = 2160 cal.
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Acetic acid has a Ka of 1.8 * 10-5. Three acetic acid/acetate buffer solutions, A, B, and C, were made using varying concentrations: acetic acid ten times greater than acetate, acetate ten times greater than acetic acid, and acetate=acetic acid.
Match each buffer to the expected pH. pH = 3.74 ; pH = 4.74 ; pH = 5.74
Part B: How many grams of dry NH4Cl need to be added to 2.30 L of a 0.600 M solution of ammonia, NH3, to prepare a buffer solution that has a pH of 8.71? Kb for ammonia is 1.8 * 10-5.
Express your answer with the appropriate units.
Answer:
A) acetic acid ten times greater than acetate pH = 3.74
B) acetate ten times greater than acetic acid pH = 5.74
C) For solution 3: acetate=acetic acid pH = 4.74
Mass NH4Cl = 40.30 grams
Explanation:
Step 1: Data given
Ka is: 1.8 * 10^-5
Solution 1: acetic acid ten times greater than acetate
Solution 2: acetate ten times greater than acetic acid
Solution 3: acetate=acetic acid
Step 2: The pH formula
pH = pKa + log[CH3COO-]/[CH3COOH]
For solution 1: acetic acid ten times greater than acetate this means ) [[CH3COO-]/[CH3COOH]) has a value of 1/10
pH = pKa + log[CH3COO-]/[CH3COOH]
pH = -log(1.8*10^-5) + log(1/10)
pH = 4.74 -1
pH = 3.74
For solution 2: acetate ten times greater than acetic acid
pH = pKa + log[CH3COO-]/[CH3COOH]
pH = -log(1.8*10^-5) + log(10)
pH = 4.74 + 1
pH = 5.74
For solution 3: acetate=acetic acid
pH = pKa + log[CH3COO-]/[CH3COOH]
pH = -log(1.8*10^-5) + log(1)
pH = 4.74 + 0
pH = 4.74
Part B: Calculate molarity
pOH = pKb + log [H
5.29= -log (1.8*10^-5) + log [BH+]/[0.600 M]
5.29 = 4.744 + log [BH+]/[0.600 M]
0.546 = [BH+]/0.600
[BH+] = 0.3276 M
Moles NH4+ = 0.3276 M * 2.30 L
Moles NH4+ = 0.75348 moles
Moles NH4Cl = 0.75348 moles
Mass NH4Cl = 0.75348 moles * 53.49 g/mol
Mass NH4Cl = 40.30 grams
A container holds 20.4 L of CO2 at 1.58 atm, what is the volume at STP?
Answer:
32.232 L
Explanation:
-Given the volume at 1.58atm is 20.4 L
-At standard pressure, the pressure is 1.00atm
-We apply Charle's Law to find the volume at STP:
[tex]P_1V_1=P_2V_2\\\\\\1.58\ atm\times 20.4\ L=1.00\ atm\times V_2\\\\V_2=\frac{1.58\times 20.4}{1.00}\\\\\\\\=32.232\ L[/tex]
Hence, the volume of the gas at STP is 32.232 L
When the system is at equilibrium, it contains NO 2 at a pressure of 0.817 atm , and N 2 O 4 at a pressure of 0.0667 atm . The volume of the container is then reduced to half its original volume. What is the pressure of each gas after equilibrium is reestablished
Final answer:
When the system is at equilibrium with specific initial pressures and the volume of the container is reduced by half, the pressure of each gas changes accordingly.The pressure of NO₂ will be 1.634 atm, and the pressure of N₂O₄ will be 0.1334 atm.
Explanation:
When the system is at equilibrium, it contains NO₂at a pressure of 0.817 atm, and N₂O₄ at a pressure of 0.0667 atm. If the volume of the container is reduced to half its original volume, the pressure of each gas will change.
According to the ideal gas law, the pressure of each gas will double when the volume is reduced by half. So, after re-establishing equilibrium, the pressure of NO₂ will be 1.634 atm, and the pressure of N₂O₄ will be 0.1334 atm.
The pressure on a 200 milliliter sample of CO2 (g) at constant temperature is increased from
600 mmHg to 1200 mmHg. What is the new volume?
(1 Point)
100 mL
300 mL
400 ml
600 mL
The answer for the following problem is mentioned below.
Therefore the final volume of the gas is 100 ml.Explanation:
Given:
Initial pressure ([tex]P_{1}[/tex]) = 600 mm of Hg
Final pressure ([tex]P_{2}[/tex]) = 1200 mm of Hg
Initial volume ([tex]V_{1}[/tex]) = 200 ml
To find:
Final volume ([tex]V_{2}[/tex])
We know;
According to the ideal gas equation,
P × V = n × R × T
Where;
P represents the pressure of the gas
V represents the volume of the gas
n represents the no of moles of the gas
R represents the universal gas constant
T represents the temperature of the gas
So,
From the above mentioned equation,
P × V = constant
[tex]\frac{P_{1} }{P_{2} }[/tex] = [tex]\frac{V_{1} }{V_{2} }[/tex]
Where,
([tex]P_{1}[/tex]) represents the initial pressure of the gas
([tex]P_{2}[/tex]) represents the final pressure of the gas
([tex]V_{1}[/tex]) represents the initial volume of the gas
([tex]V_{2}[/tex]) represents the final volume of the gas
So;
[tex]\frac{600}{1200}[/tex] = [tex]\frac{V_{2} }{200}[/tex]
[tex]V_{2}[/tex] = 100 ml
Therefore the final volume of the gas is 100 ml.
Final answer:
Using Boyle's Law, which states that the product of pressure and volume for a gas is constant at a fixed temperature, it is calculated that the new volume of the CO2 (g) sample when the pressure is doubled to 1200 mmHg at constant temperature is 100 mL.
Explanation:
The question asks about the change in volume of a gas sample when the pressure is increased while keeping the temperature constant. This scenario is described by Boyle's Law, which states that for a given mass of gas at constant temperature, the volume of the gas varies inversely with the pressure. The initial condition for the CO2 (g) is 200 mL at 600 mmHg, and after the pressure is increased to 1200 mmHg, we want to find the new volume.
Boyle's Law can be expressed as P1V1 = P2V2, where P1 and V1 are the initial pressure and volume, and P2 and V2 are the final pressure and volume, respectively. Using this relationship, when P1 = 600 mmHg, V1 = 200 mL, P2 = 1200 mmHg, we need to solve for V2. When we plug these values into the equation, we get V2 = (P1 * V1) / P2 = (600 mmHg * 200 mL) / 1200 mmHg = 100 mL.
Therefore, the new volume of the CO2 (g) sample when the pressure is increased to 1200 mmHg at constant temperature is 100 mL.
1. What mass of the following chemicals is needed to make the solutions indicated?
a. 1.0 liter of a 1.0 M mercury (II) chloride (HgCl2) solution
b. 2.0 liters of a 1.5 M sodium nitrate (NaNO3) solution
c. 5.0 liters of a 0.1 M Ca(OH)2 solution
d. 100 mL of a 0.5 M (NH4)3PO4 solution
2. Calculate the molarity of the following solutions.
a. 12 g of lithium hydroxide (LiOH) in 1.0 L of solution
b. 198 g of barium bromide (BaBr2) in 2.0 L of solution
c. 54 g of calcium sulfide (CaS) in 3.0 L of solution
3. Calculate the volume of each solution, in liters.
a. a 1.0 M solution containing 85 g of silver nitrate (AgNO3)
b. a 0.5 M solution containing 250 g of manganese (II) chloride (MnCl2)
c. a 0.4 M solution containing 290 g of aluminum nitrate (Al(NO3)3)
The following questions are answered below
Explanation:
1.a. 1.0 liter of a 1.0 M mercury (II) chloride (HgCl2) solution
1.0 L 1 mol 271.49 g
L 1 L 1 mol
= 271.49 g
= HgCl₂ = 271.49 g HgCl₂
1.b. 2.0 liters of a 1.5 M sodium nitrate (NaNO3) solution
[tex]\frac{2.0 L}{1}[/tex][tex]\frac{1.5 mol}{L}[/tex][tex]\frac{85.01 g}{1 mol}[/tex]
= 255.03 g
= 255 g NaNo₃
1.c. 5.0 liters of a 0.1 M Ca(OH)2 solution
= 37 g Ca(OH)2
1.d. 100 mL of a 0.5 M (NH4)3PO4 solution
= 7.5 g (NH₄)₃PO₄
2. To find the molarity of the following solutions
2.a. 12 g of lithium hydroxide (LiOH) in 1.0 L of solution
= 0.50 m (LiOH)
2.b. 198 g of barium bromide (BaBr2) in 2.0 L of solution
= 0.33 m (BaBr₂)
2.c. 54 g of calcium sulfide (CaS) in 3.0 L of solution
= 0.25 m (CaS)
3. To find the volume of each solution
3.a. 1.0 M solution containing 85 g of silver nitrate (AgNO3)
= 0.50 L (AgNO₃)
3.b. 0.5 M solution containing 250 g of manganese (II) chloride (MnCl2)
= 4.0 L MnCl2
3.c. 0.4 M solution containing 290 g of aluminum nitrate (Al(NO3)3)
= 3.4 L (Al(NO₃)₃)
__________ is a numerical value assigned to each element to indicate the number of electrons that might be lost, gained, or shared by an atom of that element when it bonds with an ion or an atom of another element to form a compound.
Answer:
oxidation number
Explanation:
Describes the degree of oxidation of an atom in a chemical compound.
A balloon is filled to a volume of 600 mL at a temperature of 20°C . The balloon is been called to a temperature of 100 K. What is the final volume of the balloon
Answer:
204.78 mL
Explanation:
- use Charle's law and rearrange formula
- change C to K
- Hope this helped! Let me know if you need further explanation.
A solution containing 1.0 M NiCl2 and 1.0 M SnBr2 undergoes electrolysis by passing a current between two platinum electrodes. What are the most likely first products to be formed? Cl2 (aq) + 2e- → 2Cl- (aq) ℰ°= 1.36 V Br2 (aq) + 2e- → 2Br- (aq) ℰ° =1.08 V Sn2+ (aq) + 2e- → Sn(s) ℰ° = -0.14 V Ni2+ (aq) + 2e- → Ni(s) ℰ°= -0.24 V
Answer:
Sn2+ (aq) + 2e- → Sn(s) ℰ° = -0.14 V
Explanation:
A close look at all the options shows that the most feasible first reaction is the reduction of tin II ion to ordinary metallic tin.
Given the two half cells, nickel is oxidized in one half cell to Ni II while in the second half cell, tin II ion is reduced to metallic tin. The platinum electrodes simply act as electron conduits in the cell.
A student went to the dentist and found out that he had a cavity. He always brushes his teeth twice a day, so he didn't understand how he got a cavity. The dentist told him that drinking things every day that are acidic, such as lemonade, can contribute to cavities. He didn't drink lemonade but does drink a variety of other drinks.
The next day he brought in a sample of each drink and asked his science teacher to borrow a pH probe to test each liquid. The pH of Drink A is 11.9, Drink B is 7.0, Drink C is 5.3, Drink D is 9.8, Drink E is 2.4. Explain which drink(s) the student should avoid if he wants to protect his teeth from further damage.
In your response, be sure to include:
1. an explanation of what pH measures
2. which drinks are acidic, basic, and neutral.
Answer:E is an acidic
Explanation:
Soo he should avoid the drink E and in pH measurement the more acidic is below 7 and the the more alkali is above 7 and the neutral drink is B and it may a water ...
A shallow river dries up is an example of
Condensation
Evaporation
Precipitation
Runoff
Answer:
Evaporation
Explanation:
Evaporation is when liquid becomes a gas which is how the river dried up
In photosynthesis, carbon dioxide and water are converted into glucose and oxygen in the presence of chlorophyll and light energy. If 1.0 mole of water is available with an excess of carbon dioxide, how many moles of glucose (C6H12O6) can be produced
Answer:
0.17 mole of glucose is formed.
Explanation:
Step 1:
The equation for the reaction. This is given below:
CO2 + H2O —> C6H12O6 + O2
Step 2:
Balancing the equation.
The equation can be balanced as follow:
CO2 + H2O —> C6H12O6 + O2
There are 6 atoms of C on the right side and 1 atom on the left side. It can be balance by putting 6 in front of CO2 as shown below:
6CO2 + H2O —> C6H12O6 + O2
Therefore are 12 atoms of H on the right side and 2 atoms on the left side. It can be balance by putting 6 in front of H2O as shown below:
6CO2 + 6H2O —> C6H12O6 + O2
There are a total of 8 atoms of O the right side and a total of 18 atoms on the left. It can be balance by putting 6 in front of O2 as shown below:
6CO2 + 6H2O —> C6H12O6 + 6O2
Now the equation is balanced.
Step 3:
Determination of the number of mole of glucose (C6H12O6) produced by 1 mole of water.
This is illustrated below:
6CO2 + 6H2O —> C6H12O6 + 6O2
From the balanced equation above,
6 moles of H2O produced 1 mole of C6H12O6.
Therefore, 1 mole of H2O will produce = 1/6 = 0.17 mole of C6H12O6.
Answer:
IF 1.0 mol of water is available, 0.167 moles of glucose (C6H12O6) will be produced
Explanation:
Step 1: Data given
Number of moles of water = 1.0 moles
Carbon dioxide is in excess
Step 2: The balanced equation
6CO2 + 6H2O → C6H12O6 + 6O2
Step 3: Calculate moles of glucose
For 6 moles CO2 we need 6 moles H2O to produce 1 mol glucose and 6 moles O2
For 1.0 moles of water we'll have 1.00 / 6 = 0.167 moles of glucose
IF 1.0 mol of water is available, 0.167 moles of glucose (C6H12O6) will be produced
How many dozens of doughnuts are in 48 doughnuts
Final answer:
There are 4 dozens in 48 doughnuts, as a dozen is a group of 12 objects. This quantity would require four boxes with a volume of 324 cubic inches each to hold all the doughnuts.
Explanation:
To find out how many dozens of doughnuts are in 48 doughnuts, we can simply divide the total number of doughnuts by the number in a dozen. Since a dozen refers to 12 objects, we divide 48 by 12.
48 ÷ 12 = 4
Therefore, there are 4 dozens in 48 doughnuts. When buying items like doughnuts, it is common to acquire them in groups, like a dozen, because it is more convenient and efficient.
Let's consider the dimensional aspect for a moment. If you have a 9x9x4 inch box for a dozen doughnuts, this box would have a volume of 324 cubic inches. For 48 doughnuts, which we have established are 4 dozens, we would need four of these boxes, equating to 4 × 324 in3 or 1296 in3 in total to hold all of them.
How would you describe an electron
Answer:
an electron is part of the 3 things that are in an atom, it has a negative charge
what was the purpose of running a tlc of ferrocene, the acetylferrocene product mixture, and co-spot (an overlay of ferrocene and the product mixture) prior to conducting the column chromatography portion of the experiment?a. All of the belowb. To determine the elution in a chromatography column of the starting material and productsc. To determine if there was starting material still present in the reactiond. To identify the number of products of the reaction
Answer:
a. All of the below
Explanation:
Column chromatography in chemistry is a chromatography method used to isolate a single chemical compound from a mixture.
TLC can be used to analyze a chemical reaction to determine if the reactants have been consumed and a new product has formed. Running a tlc of ferrocene, the acetylferrocene product mixture, and co-spot, when you view the TLC plate under a UV light, you will notice that acetylferrocene product is on the right-most lane, this shows that the reaction appears to be a success: the higher spot of ferrocene has been consumed), and a new product spot is present. From these we can observe that the we can use this to identify the number of products of the reaction, determine if the starting material is still present in the reaction and the elution in a chromatography column of the starting material and products. Therefore, all the choices are correct.
Complete the following two statements regarding quantum-mechanical concepts associated with the Bohr model of the atom and refinements that resulted from the wave-mechanical atomic model. " Two important quantum-mechanical concepts associated with the Bohr model of the atom are that electrons are particles moving in _______
Enter your answer for the missing word between words "moving in" and "orbitals" in accordance to the question statement discrete orbitals, and electron energy is quantized into
Enter your answer for the missing word after words "quantized in" in accordance to the question statement levels .
(b) Two important refinements resulting from the wave-mechanical atomic model are that the electron position is described in terms of a Enter your answer for the missing words after words "in terms of a" in accordance to the question statement electron cloud , and electron energy is quantized into both shells and subshells--each electron is characterized by Enter your answer for the missing word after words "is characterized by" in accordance to the question statement quantum numbers."
Answer:
Two important quantum-mechanical concepts associated with the Bohr model of the atom are (1) that electrons are particles moving in discrete orbitals, and (2) electron energy is quantized into shells. (b) Two important refinements resulting from the wave-mechanical atomic model are (1) that electron position is described in terms of a probability distribution, and (2) electron energy is quantized into both shells and subshells--each electron is characterized by four quantum numbers.
Explanation:
Part A:
The two important quantum-mechanical concepts associated with the Bohr model of the atom are:
(1) Electrons are particles moving in discrete orbitals.
(2) Electron energy is quantized into shells.
Part B:
The two important refinements resulting from the wave-mechanical atomic model are:
That electron position is described in terms of a probability distribution.The electron energy is quantized into both shells and subshells each electron is characterized by four quantum numbers.Learn more :
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Assuming that there is a constant partial pressure for oxygen, according to Le Châtelier’s Principle which of the following occurs when body temperature decreases during hypothermia?
Answer:
B. The amount of oxygen will decreases
Explanation:
According to Le Châtelier’s Principle, when the condition of the system changes the equilibrium will shift to compensate for the changes. When temperature decrease, the pressure will also decrease and this will shift the equilibrium to the side with exothermic reaction or less molecule count.
The question is not giving the equilibrium reaction of oxygen, so I assume its
O2 + Hb = HbO2
Since the number of molecules in the right side is lower, then the number of oxygen will decrease since the reaction will shift to the right.
An equivalent is:___________
a) an equivalent is the amount of ion that has a 1+ charge.
b) 1 mole of an ionic compound.
c) 1 mole of any ion. the amount of ion that carries 1 mole of electrical charge.
d) the amount of ion that has a 1- charge.
Answer:
The amount of ion that carries 1 mole of electrical charge
Explanation:
One equivalent: In reaction stoichiometry, the amount of one substance that reacts with one mole of another substance. This will often (but not always) be a 1:1 mole ratio.
An equivalent is the amount of ion that carries 1 mole of electrical charge.
An equivalent is the amount of a substance that reacts with one mole of another substance in a given chemical reaction.
It is a unit of measurement in Stoichiometry that helps to describe the amount of ion that carries 1 mole of electrical charge.
Examples include:
1 mole of Na⁺ = 1 Eq1 mole of Cl⁻ = 1 Eq1 mole of Ca²⁺ = 2 EqThus, we can conclude that an equivalent is the amount of ion that carries 1 mole of electrical charge.
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A chemistry student needs 75 g of thiophene foran experiment. He has available 0.50 kg of a 29.3% w/w solution of thiophene in carbon tetrachloride.
Calculate the mass of solution the student should use. Ifthere's not enough solution, press the "No solution" button.
Answer: The mass of solution the student should use is 256 g
Explanation:
Given : 29.3 % w/w which means that 29.3 g of solute is present in 100 g of solution
Thus 100 g of solution contains = 29.3 g of solute
0.50 kg or 500 g of solution contains = [tex]\frac{29.3}{100}\times 500=146.5[/tex] g of solute (1kg=1000g)
146.5 g of solute is available in = 500 g of solution
Thus 75 g of solute is available in = [tex]\frac{500}{146.5}\times 75 g=256g[/tex] of solution
Thus the mass of solution the student should use is 256 g
what equation represents a chemical equilibrium?
The equation which represents the chemical equilibrium is 2 NO₂ ⇄ N₂0₄
Explanation:
The equation which represents the chemical equilibrium is2 NO₂ ⇄ N₂0₄.
A chemical reaction is in equilibrium at the combinations of reactants and products are even and their ratio does not change In other words, the equilibrium can be defined as the system is in equilibrium when the forward and backwards reactions happen at regular rates.The idea of chemical equilibrium was formed after Berthollet found that some chemical reactions are reversible.If'substance X is a liquid, substance Y is a gas, and substance Z is a solid, and all are at the
same temperature and pressure, then the order of increasing strength of their intermolecular
forces would be
The answer is Y < X < Z
Final answer:
The order of increasing strength of intermolecular forces for substance X (liquid), Y (gas), and Z (solid) is: Y < X < Z, with the gas having the weakest and the solid having the strongest intermolecular forces.
Explanation:
If we consider substances X, Y, and Z, which are a liquid, a gas, and a solid respectively, and they are all at the same temperature and pressure, the order of increasing strength of their intermolecular forces can be determined based on their states of matter. Given that substances with stronger intermolecular forces are more likely to be a solid at room temperature and will have a higher boiling point, it follows that the solid will have the strongest forces, followed by the liquid, and then the gas. Consequently, substance Z (the solid) would have the strongest intermolecular forces, substance X (the liquid) would have intermediate forces, and substance Y (the gas) would have the weakest forces.
18.53 For CaO, the ionic radii for Ca2 and O2 ions are 0.100 and 0.140 nm, respectively. If an externally applied electric field produces a 5% expansion of the lattice, compute the dipole moment for each Ca2O2pair. Assume that this material is completely unpolarized in the absence of an electric field.
Answer:
[tex] = 1.92*10^-^3^0 C.m[/tex]
Explanation:
Given:
[tex] r_ca_^2_^+ = 0.100 nm[/tex]
[tex] r_o_^2_^- = 0.14 nm [/tex]
Let's find the distance of separation between cation and anion when there is no applied electric field with the formula:
[tex] d = r_ca_^2_^+ + r_o_^2_^- [/tex]
d = 0.100 nm + 0.140 nm
= 0.240 nm
Let's also calculate the distance of separation between anion and cation when there is an applied electric field.
We use the formula:
∆d = 5%d => 0.05d
= 0.05 * 0.024 nm
∆d = 0.0120 nm
[tex]0.120* 10^-^9m[/tex]
[tex]= 1.20*10^-^1^1m[/tex]
Given magnitude of each dipole= [tex]1.602*10^-^1^9 C [/tex]
Let's find the dipole moment, with the formula:
p = q∆d
Substituting figures in the formula, we have:
[tex]p = 1.602*10^-^1^9 * 12*10^-^2^1 [/tex]
[tex] = 1.92*10^-^3^0 C.m[/tex]
Answer:
Explanation:
Answer:
= 1.92*10^-^3^0 C.m
Explanation:
Given:
r_ca_^2_^+ = 0.100 nm
r_o_^2_^- = 0.14 nm
Let's find the distance of separation between cation and anion when there is no applied electric field with the formula:
d = 0.100 nm + 0.140 nm = 0.240 nm
Let's also calculate the distance of separation between anion and cation when there is an applied electric field.
We use the formula:
∆d = 5%d => 0.05d
= 0.05 * 0.024 nm
∆d = 0.0120 nm
0.120* 10^-^9m
= 1.20*10^-^1^1m
Given magnitude of each dipole= 1.602*10^-^1^9 C
Let's find the dipole moment, with the formula:
p = q∆d
Substituting figures in the formula, we have:
p = 1.602*10^-^1^9 * 12*10^-^2^1
= 1.92*10^-^3^0 C.m