Answer: A. There are two hydrogen atoms and one oxygen atom per water molecule.
Explanation:
The chemical formular for water "H2O", means it contain 2 hydrogen atoms and one oxygen atom per molecule.
Final answer:
The molecular formula H2O indicates that there is a ratio of two hydrogen atoms to one oxygen atom in each water molecule, which makes option A the correct answer.
Explanation:
The formula of water, H2O, indicates several things about water molecules. The most direct interpretation is that for each water molecule, there are two hydrogen atoms and one oxygen atom. Therefore, the correct option in the provided question is A: there are two hydrogen atoms and one oxygen atom per water molecule. Although oxygen has a greater mass than hydrogen, the molecular formula does not reflect mass directly but rather the ratio of atoms within the molecule. Looking at the molecular mass, we know that the mass of an oxygen atom is approximately 16 times that of a hydrogen atom. Thus, while there are two atoms of hydrogen for every one of oxygen, oxygen contributes more to the overall mass of a molecule due to its greater atomic mass.
Smooth muscle lines the walls of many of the
organs that make up the digestive system. The
smooth muscle contracts in ways to move the
food through the digestive system in a
process called peristalsis. The smooth muscle
found in the walls of the stomach and
intestines is considered which of the
following?
A. cell
B. organ
C. organism
D. tissue
Answer:
B. organ
Explanation:
Smooth muscle is found in the walls of hollow organs like your intestines and stomach. They work automatically without you being aware of them. Smooth muscles are involved in many 'housekeeping' functions of the body.
Try using Zn (solid) with Cu(NO3)2 in one cell and Cu(s) with Zn(NO3)2 solution in another cell. Note down the voltage value. Explain what you are seeing for voltage value and use redox reaction to justify the process.
Answer:
See below
Explanation:
When a strip of zinc metal is placed into a blue solution of copper(II) nitrate, a reaction immediately begins as the zinc strip begins to darken. If left in the solution for a longer period of time, the zinc will gradually decay due to oxidation to zinc ions.
Stoichiometry! :) Please note:
- Use 6.022x1023 for avogadro’s number
- Ignore sig figs and do not round the final answer.
- Keep it to 1 decimal place.
Answer:
18.5 grams
Explanation:
The first step is to balance the equation.
2LiOH+CO2⇒Li2CO3+H2O+ some extra oxygen
For CO2, carbon has a molar mass of about 12, and oxygen has a molar mass of about 16, so the total is 44. Now that the equation is balanced and there are two LiOH's, it's molar mass is now doubled and it effectively has a molar mass of 48. 12/48=0.25 moles of both original substances used, and 0.25 moles of the final products. Li2CO3 has a molar mass of 7*2+12+16*3=74, and multiplying this by the 0.25 moles yields 18.5 grams. Hope this helps!
Answer:
18.5 grams [tex]Li_{2}CO_{3}[/tex]
Explanation:
First, we'll need to balance the equation:
[tex]LiOH_{s} + CO_{2(g)}[/tex] → [tex]Li_{2}CO_{3(s)} + H_{2}O_{(l)}[/tex]
There is one (Li) on the left and two on the right, so let's add a 2 coefficient on the left.
[tex]2LiOH_{s} + CO_{2(g)}[/tex] → [tex]Li_{2}CO_{3(s)} + H_{2}O_{(l)}[/tex]
Now there are 2 (Li) on the left, and 2 on the right, 4 (O) on both sides, 1 (C) on both sides, and 2 (H) on both sides. The equation is balanced!
Step 1: Find the limiting reactant
To find the limiting reactant, we need to convert the given masses of each reactant into moles. Multiply the given masses by the molar masses.
12g 2LiOh × [tex]\frac{1 mol}{48 g}[/tex](double the molar mass because you have two molecules) = 0.25 moles
12g CO₂ × [tex]\frac{1 mol}{44.01 g}[/tex] = 0.272 moles
We'll test both reactants to see which one limits us.
Given 0.25 mole LiOH × [tex]\frac{1 mole CO_{2}}{2 moles LiOH}[/tex] = .125 moles CO₂ neededGiven 0.272 moles CO₂ x [tex]\frac{2 moles LiOH}{1 mole CO_{2}}[/tex] = 0.545 moles LiOH neededSince we don't have enough CO₂ to use all of our LiOH, CO₂ is the limiting reactant. We will use all of the CO₂ to perform our reaction and ignore the excess LiOH.
Step 2: Calculating the mass of the product
You can find the mass of either product with a mole ratio. (Remember, we have too much CO₂, so we'll need to use the given LiOH to perform this calculation)
0.25 moles LiOH × [tex]\frac{1 mole CO_{2}}{1 mole Li_{2}CO_{3}}[/tex] = 0.25 moles [tex]Li_{2}CO_{3}[/tex]
Now we convert back to grams!
0.25 moles [tex]Li_{2}CO_{3}[/tex] × [tex]\frac{74 g}{1 mole}[/tex] = 18.5 grams
Calculate the thermometer in an air-conditioned room reads 20.0°C what is the temperature of the room In degrees Fahrenheit and in kelvins? Show your work
Answer:
A. 68°F
B. 293K
Explanation:
The temperature (celsius) = 20.0°C
A. Conversion of the temperature in celsius to fahrenheit.
This is illustrated below:
°F = 9C/5 + 32
C = 20°C
°F = 9C/5 + 32
°F = 9x20/5 + 32
°F = 36 + 32
°F = 68°F
B. Temperature (Kelvin) = temperature (celsius) + 273
Temperature (celsius) = 20°C
Temperature (Kelvin) = 20°C + 273
Temperature (Kelvin) = 293K
Final answer:
To convert the temperature from Celsius to Fahrenheit, use the formula F = (C * 1.8) + 32. To convert the temperature from Celsius to Kelvin, add 273.15 to the Celsius temperature.
Explanation:
To convert the temperature from Celsius to Fahrenheit, we can use the formula:
F = (C * 1.8) + 32
where F is the temperature in Fahrenheit and C is the temperature in Celsius. Plugging in the given temperature of 20.0°C:
F = (20.0 * 1.8) + 32 = 68.0°F
To convert the temperature from Celsius to Kelvin, we simply add 273.15 to the Celsius temperature:
K = C + 273.15
Therefore, the temperature in Kelvin would be:
K = 20.0 + 273.15 = 293.15K
Calculate the enthalpy of the formation of butane, C4H10, using the balanced chemical equation and the standard value below:
4C(s) + 5H2(g) => C4H10(g)
Standard enthalpy of formation values:
(Delta Triangle)H^0 of C(s)= -393.5kJ/mol
(Delta triangle)H^0f of H2(g)=-285.8 kJ/mol
(Delta triangle)H^0f of C4H10(g)=-2877.6kJ/mol
Answer:
+125.4 KJmol-1
Explanation:
∆H C4H10(g) = -2877.6kJ/mol
∆H C(s)=-393.5kJ/mol
∆H H2(g) = -285.8
∆H reaction= ∆Hproducts - ∆H reactants
∆H reaction= (-2877.6kJ/mol) - [4(-393.5kJ/mol) +5(-285.8)]
∆H reaction= +125.4 KJmol-1
The volume of a gas at 155.0 kPa changes from 22.0 L to 10.0 L. What
is the new pressure if the temperature remains constant?
Answer:
V1P1=V2P2
155(22L)=P(10L0
P=341kPg
Explanation:
The following format is copied directly from your notes for how to solve these!!!
1) Analyze problem statement to find knowns and unknowns for each gas variable
V1 = 22.0 L P1 = 155.0 kPa T1 = T2 n = constant (same sample of gas)
V2= 10.0 L P2 = ? kPa T2 = T1 temperature is constant
2) Decide which of the gas laws to use and write its formula.
Only P and V are given, so Boyle's law is used P1V1 = P2V2
3) Change any temperature values to Kelvin (if T is needed) not needed
4) Plug in the knowns - INCLUDING UNITS!!
P1V1 = P2V2
(155.0 kPa) (22.0 L) = P2 (10.0 L)
P2 = (155.0 kPa)(22.0 L) = 341 kPa
(10.0 L)The following format is copied directly from your notes for how to solve these!!!
1) Analyze problem statement to find knowns and unknowns for each gas variable
V1 = 22.0 L P1 = 155.0 kPa T1 = T2 n = constant (same sample of gas)
V2= 10.0 L P2 = ? kPa T2 = T1 temperature is constant
2) Decide which of the gas laws to use and write its formula.
Only P and V are given, so Boyle's law is used P1V1 = P2V2
3) Change any temperature values to Kelvin (if T is needed) not needed
4) Plug in the knowns - INCLUDING UNITS!!
P1V1 = P2V2
(155.0 kPa) (22.0 L) = P2 (10.0 L)
P2 = (155.0 kPa)(22.0 L) = 341 kPa
(10.0 L)
Final answer:
By applying Boyle's law, which states the inverse relationship between volume and pressure at constant temperature, we can calculate the new pressure of a gas when its volume changes. The new pressure is of 341.0 kPa.
Explanation:
The question provided discusses the behavior of gases under different conditions of pressure, volume, and temperature. This is a chemistry concept known as Boyle's law when temperature is constant, or Gay-Lussac's law when pressure is constant, or the combined gas law when neither are constant.
With the information given, we are asked to calculate the new volume or pressure of a gas sample when one of the other variables changes, while holding the other constant.
If the temperature remains constant (Boyle's law), the pressure of a gas is inversely proportional to its volume (P1V1 = P2V2). In the first example, to find the new pressure when the volume decreases from 22.0 L to 10.0 L, while starting at 155.0 kPa, the formula is rearranged to P2 = (P1V1) / V2.
Thus the new pressure is (155.0 kPa × 22.0 L) / 10.0 L, resulting in a new pressure of 341.0 kPa.
Effects of warm tropical waters meeting with cool air.
The effect of warm tropical waters meeting with cool air is hurricane.
What is a hurricane?A hurricane is formed when warm tropical water meet with air that is cool and humid. This creates a zone of pressure over the warm water causing the air to rotate.
Hence, the effect of warm tropical waters meeting with cool air is hurricane.
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Clasificar las siguientes mezclas como homogéneas o heterogéneas a. Un balde con bolas de diferente color ( ) b. Arena de playa ( ) c. Una muestra de sal con agua ( ) d. Aire ( ) e. Sangre ( ) f. Una ensalada de frutas ( ) g. Cubos de hielo con agua( ) h. Vidrio de una ventana ( ) i. Agua de charca ( ) j. La sopa ( ) l. La madera ( ) m. Gasolina ( ) n. Polvo ( ) o. Naranja ( ) p. Cemento ( ) q. Aceite para motor ( ) r. Algodón ( ) s. Papel ( ) t. Aceite y v. Vinagre ( ) k. Smog ( ) m. Gasolina ( ) n. Polvo ( ) o. Naranja ( ) p. Cemento ( ) q. Aceite para motor ( ) r. Algodón ( ) s. Papel ( ) t. Aceite y v. Vinagre ( )
Answer:
Classify the following mixtures as homogeneous or heterogeneous
a. A bucket with balls of different color heterogeneous mixture
b. Beach sand homogeneous mixture
c. A sample of salt with water homogeneous mixture
d. Air homogeneous mixture
e. Blood homogeneous mixture
f. A fruit salad heterogeneous mixture
g. Ice cubes with water heterogeneous mixture
h. Window glass homogeneous mixture
i. Pond water homogeneous mixture
j. The soup heterogeneous mixture
l. Wood homogeneous mixture
m. Gasoline homogeneous mixture
n. Powder homogeneous mixture
o. Orange heterogeneous mixture
p. Cement homogeneous mixture
q. Engine oil homogeneous mixture
r. Cotton homogeneous mixture
s. Paper homogeneous mixture
t. Oil and Vinegar heterogeneous mixture
k. Smog homogeneous mixture
Explanation:
In homogeneous mixtures, the elements are united in such a way that they are not distinguishable, while in heterogeneous mixtures, these are observable.
A gas occupies a volume of 1.00 L at 25.0°C. What volume will the gas occupy at 1.00 x10^2 °C?
Answer : The volume of gas occupy at [tex]1.00\times 10^2^oC[/tex] is, 1.25 L
Explanation :
Charles' Law : It states that volume of the gas is directly proportional to the temperature of the gas at constant pressure and number of moles.
Mathematically,
[tex]\frac{V_1}{T_1}=\frac{V_2}{T_2}[/tex]
where,
[tex]V_1\text{ and }T_1[/tex] are the initial volume and temperature of the gas.
[tex]V_2\text{ and }T_2[/tex] are the final volume and temperature of the gas.
We are given:
[tex]V_1=1.00L\\T_1=25.0^oC=(25.0+273)K=298K\\V_2=?\\T_2=1.00\times 10^2^oC=((1.00\times 10^2)+273)K=373K[/tex]
Putting values in above equation, we get:
[tex]\frac{1.00L}{298K}=\frac{V_2}{373K}\\\\V_2=1.25L[/tex]
Therefore, the volume of gas occupy at [tex]1.00\times 10^2^oC[/tex] is, 1.25 L
In which species does nitrogen have the highest oxidation number?
Select one:
a. NH3
b. N2
c. NaNO3
d. NO2-
e. HNO2
Answer:
NaNO3
Explanation:
The species where nitrogen has the highest oxidation number is NaNO3, where nitrogen has an oxidation number of +5.
Explanation:The species where nitrogen has the highest oxidation number is NaNO3. In this compound, the oxidation number of nitrogen is +5. We can determine this by understanding that the oxidation number for oxygen is usually -2, and for sodium it is usually +1. Therefore, to balance the charge in the compound NaNO3(sodium nitrate), nitrogen must have an oxidation state of +5.
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Which compound is soluble in water PbS BaS Na2S Fe2S3
Answer:
The answer to your question is Na₂S, if you need to choices the other one is BaS
Explanation:
As a general rule, all the compounds that have sulfur, are insoluble in water, but the are some exceptions.
-Molecules with ammonia
-If the molecule has alkali metals is soluble
-If the molecule has Ca⁺², Sr⁺² and Ba⁺² is soluble in water.
From the compounds given, following the rules, the compound that is soluble in is Na₂S and perhaps BaS.
Among PbS, BaS, Na2S, and Fe2S3, Na2S is the compound that is soluble in water, as sodium is a Group I element and its sulfide does not follow the general rule of insolubility for sulfides.
Explanation:The question concerns the solubility of compounds in water, which is a topic in Chemistry. Among the compounds listed (PbS, BaS, Na2S, Fe2S3), Na2S (sodium sulfide) is the one that is soluble in water. This is because Na+ is a Group I element, and as per solubility rules, sulfides are generally insoluble except for those of Group I elements and also calcium, strontium, and barium to a lesser extent. Despite barium being part of the exception, BaS tends to hydrolyze and form Ba(OH)2 and H2S, making it not truly soluble in water for practical purposes. On the other hand, PbS (lead sulfide), Fe2S3 (iron(III) sulfide), and BaS (barium sulfide) are typically insoluble due to their placement on the periodic table as transition metals or heavy metals, which generally form insoluble sulfides.
Hbr(aq)+h2o(l)→h3o+(aq)+br−(aq) express your answers as a chemical expressions. enter your answers in order given in the question separated by commas.
This is an incomplete question, here is a complete question.
For each reaction, identify the Bronsted-Lowry acid, the Bronsted-Lowry base, the conjugate acid, and the conjugate base.
[tex]HBr(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+Br^-(aq)[/tex]
Express your answers as a chemical expressions. Enter your answers in order given in the question separated by commas.
Answer : The given equilibrium reaction will be,
[tex]HBr(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+Br^-(aq)[/tex]
Acid Base Conjugate Conjugate
acid base
Explanation :
According to the Bronsted Lowry concept, Bronsted Lowry-acid is a substance that donates one or more hydrogen ion in a reaction and Bronsted Lowry-base is a substance that accepts one or more hydrogen ion in a reaction.
Or we can say that, conjugate acid is proton donor and conjugate base is proton acceptor.
The given equilibrium reaction will be,
[tex]HBr(aq)+H_2O(l)\rightleftharpoons H_3O^+(aq)+Br^-(aq)[/tex]
Acid Base Conjugate Conjugate
acid base
In this reaction, [tex]HBr[/tex] is an acid that donate a proton or hydrogen to [tex]H_2O[/tex] base and it forms [tex]Br^-[/tex] and [tex]H_3O^+[/tex] are conjugate base and acid respectively.
The formula HBr(aq)+H2O(l)→H3O+(aq)+Br−(aq) represents a Brønsted-Lowry Acid-Base reaction where HBr donates a proton to H2O, forming H3O+ and Br-. This is an acid-base reaction in an aqueous solution.
Explanation:The provided chemical reaction between Hydrobromic acid and water is a characteristic of Brønsted-Lowry Acid-Base reaction. In this reaction, HBr (Hydrobromic acid) donates a proton (H+) to H2O (water), which is a proton acceptor. This process results in the formation of Hydronium Ion (H3O+) and Bromide Ion (Br-).
Expressing the reaction step by step, we start with HBr(aq)+H2O(l), wherein the Hydrobromic acid dissociates into a proton (H+) and a bromide ion (Br-). Similarly, water dissociates into Hydronium Ion (H3O+). Hence, HBr(aq)+H2O(l)→H3O+(aq)+Br−(aq). This is an example of an acid-base reaction in aqueous solutions.
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18. A balloon contains 7.2 L of He. The pressure is reduced to
|| 2.00 atm and the
balloon expands to occupy a volume of 25.1 L. What was
the initial pressure
exerted on the balloon?
Answer:
The initial pressure exerted on the balloon is 7.0 atm.
Explanation:
To calculate the new volume, we use the equation given by Boyle's law. This law states that pressure is inversely proportional to the volume of the gas at constant temperature.
The equation given by this law is:
[tex]P_1V_1=P_2V_2[/tex]
where,
[tex]P_1\text{ and }V_1[/tex] are initial pressure and volume.
[tex]P_2\text{ and }V_2[/tex] are final pressure and volume.
We are given:
Initial pressure of helium gas in balloon = [tex]P_1=?[/tex]
Initial volume of helium gas in balloon = [tex]V_1=7.2 L[/tex]
Final pressure of helium gas in balloon = [tex]P_2=2.00 atm[/tex]
Final volume of helium gas in balloon = [tex]V_2=25.1 L[/tex]
Putting values in above equation, we get:
[tex]P_1\times 7.2 L=2.00 atm\times 25.1 L[/tex]
[tex]P_1=\frac{2.00 atm\times 25.1 L}{7.2 L}=6.97 atm\approx 7.0 atm[/tex]
Hence, the initial pressure exerted on the balloon is 7.0 atm.
A can of coke contains 25 mL of carbon dioxide gas at 100kPa. If you take it on a hike up Mount Everest and the pressure decreases to 50 kPa, what will the new volume of the carbon dioxide gas in your coke can be?
Answer:
50 mL
Explanation:
We can solve this problem by using Boyle's Law, which states that:
"For a fixed mass of an ideal gas kept at constant temperature, the pressure of the gas is inversely proportional to its volume"
Mathematically:
[tex]p\propto \frac{1}{V}[/tex]
where
p is the pressure of the gas
V is the volume of the gas
The equation can be rewritten as
[tex]p_1 V_1 = p_2 V_2[/tex]
where in this problem:
[tex]p_1 = 100 kPa[/tex] is the initial pressure of the gas in the coke
[tex]V_1=25 mL[/tex] is the initial volume
[tex]p_2=50 kPa[/tex] is the final pressure
Solving for V2, we find the final volume:
[tex]V_2=\frac{p_1 V_1}{p_2}=\frac{(100)(25)}{50}=50 mL[/tex]
The pressure of a gas is reduced from 1200 torr to 760 torr as the volume of its container is increased from 0.650 L to 1.1 L. What would the final temperature be in Celsius if the original temperature was 15 C?
Answer:
The final temperature would be 308.7 K or 35.7 °C
Explanation:
Step 1: Data given
The initial pressure = 1200 torr
The pressure is reduced to 760 torr
The initial volume = 0.650 L
The increased volume is 1.1 L
The initial temperature is 15 °C = 288 K
Step 2: Calculate the new temperature
(P1*V1)/T1 = (P2*V2)/T2
⇒with P1 = the initial pressure = 1200 torr
⇒with V1 = the initial volume = 0.650 L
⇒with T1 = initial temperature is 15 °C = 288 K
⇒with P2 = the reduced pressure = 760 torr
⇒with V2 = the increased volume = 1.1 L
⇒with T2 = the final temperature = TO BE DETERMINED
(1200 torr * 0.650 L) / 288 K = (760 torr * 1.1 L) / T2
T2 = (760 * 1.1 * 288) / (1200 * 0.650)
T2 = 308.7 K
The final temperature would be 308.7 K or 35.7 °C
Answer:
-272.99K = 0.0032°C
Explanation:
Applying (P1V1)/T1 = (P2V2)/T2
(1200×0.65)/288 = (760 × 1.1)/T2
Simplify
T2 = 0.0032°C
According to the periodic table carbon has a tendency to bond covalently with
Answer:
Carbon tends to bond covalently with Hydrogen
Answer:
All the carbon group atoms, having four valence electrons, form covalent bonds with nonmetal atoms; carbon and silicon cannot lose or gain electrons to form free ions, whereas germanium, tin, and lead do form metallic ions but only with two positive charges.
Explanation:
The brown solid that formed is zinc copper oxygen iron
Answer: Copper
Explanation:
Just took it on Edgen
Answer:
copper
Explanation:
can someone please answer this I’ll give you 10 points!!
what is the volume of 3.00 mole of ideal gas at 100.0 C and 2.00 kPa
Answer:
The volume for the ideal gas is: 4647.5 Liters
Explanation:
Formula for the Ideal Gases Law must be applied to solve this question:
P . V = n . R . T
We convert the T° to K → 100°C + 273 = 373 K
We convert pressure value from kPa to atm.
2 kPa . 1atm/101.3 kPa = 0.0197 atm
We replace data in the formula.
V = ( n . R . T) / P → (3 mol . 0.082 . 373K) / 0.0197 atm =
The volume for the ideal gas is: 4647.5 Liters
Which of the following is true for a gas under conditions of very low temperature?
PV > nRT, because the actual volume of the gas would be more than its ideal value.
PV < nRT, because the volume is smaller due to significant intermolecular force effects.
PV = nRT, because the actual volume of the gas molecules becomes considerable.
PV = nRT, because all gases behave ideally at very low temperatures.
Answer:
D)
Explanation:
PV/nRT=1, because particles are unable to overcome intermolecular attractions
Answer:
PV < nRT, because the volume is smaller due to significant intermolecular force effects.
Explanation:
FLVS exam states that this is correct because gasses change their "ideal" behaviors at lower temperatures.
Place the capillary tube, still attached
to the ruler, in the water bath.
600 ml
x
com
COMPLETE
Temperature of gas: 44
X = 3 °C Height of the column of gas: 400
= 5.7 cm
Volume of gas (V = serh):
Temperature of gas:
cm3 DONE
Intro
Answer:
Temperature of gas: 3 °C Height of the column of gas: 5.7 cm Temperature of gas: 276k Volume of gas: .72 cm^3
Explanation:
edge 2021
The value of Temperature is 276K
and of Volume is 0.71592 [tex]cm^{3}[/tex]
How to calculate temperature?As per the formula of conversion of degree Celsius to kelvin temperature
1°C=273K
∴23 °c +273= 276 K
How to calculate volume?V=π[tex]r^{2}[/tex]h
V= volume
r = radius of capillary tube =0.2 cm
h=height of column=5.7 cm
∴V=3.14×[tex](0.2)^{2}[/tex]×5.7
∴V=0.71592[tex]cm^{3}[/tex]
Hence, the value of temperature and volume are 276K and 0.71592[tex]cm^{3}[/tex], respectively.
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This is a type of symbiotic relationship where both organisms benefit.
Answer:
Mutualism
Explanation:
In Mutualism, both parties benefit.
If the density of mercury is 13.53g/cm^3 and you have 62.5 cm^3 of mercury, how many: grams of mercury do you have? moles of mercury do you have? atoms of mercury do you have?
Answer:
The answer to your question is below
Explanation:
Data
density = 13.53 g/cm³
volume = 62.5 cm³
mass = ?
moles = ?
atoms = ?
Process
1.- Calculate the mass of mercury
formula
density = mass/volume
-Solve for mass
mass = density x volume
-Substitution
mass = 13.53 x 62.5
-Result
mass = 845.63 grams
2.- Calculate the moles of mercury
Atomic mass = 200.6 g
200.6 g of mercury --------------------- 1 mol
845.63 g of mercury -------------------- x
x = (845.63 x 1) / 200.6
x = 4.22 moles of mercury
3.- Calculate the number of atoms
1 mol -------------------- 6 .023 x 10 ²³ atoms
4.22 moles ------------- x
x = (4.22 x 6.023 x 10²³) / 1
x = 2.54 x 10²³ atoms
To prepare a solution of BF4-(aq), HF(g) is bubbled into a solution containing 50.0 g of H3BO3 in a 1 L reaction vessel. Calculate the maximum number of moles of BF4-(aq) that can be produced.
Answer:
Explanation:
The chemical reaction involved is as follows
H₃BO₃ + 4HF = HBF₄ + 3H₂O
1 mol 1 mol
mol weight of H₃BO₃ is 61.84 gm
50g = 50 / 61.84 mol.
= 0.8 mol.
.8 mol of H₃BO₃ will form .8 mol of BF₄⁻ ion .
What volume of neon gas occupies a container if 322 grams of neon is at 0.955 atm and -28.0 degrees Celsius?
Answer:
The volume occupies of neon gas is 335, 7 L
Explanation:
We use the formula PV=nRT. We convert the unit temperature Celsius into Kelvin: 0°C=273 K---> -28°C= -28+273= 245K. We calculate the number of mols in 322 grams of neon:
20,18 g---1 mol neon
322g---x= (322g x 1 mol neon)/ 20, 18g=15, 96 mol neon
PV=nRT ----> V= (nRT)/P
V= (15,96 mol x 0,082 l atm/K mol x 245 K)/ 0,955 atm= 335, 7 L
What is the temperature of 4.75 moles of a substance at a pressure of 1.2 atm and a volume of 0.125 L? Use 0.0821 for R and significant digits (2 in this case). Report your answer in Kelvin.
Answer:
T = 0.38 K
Explanation:
Given data:
Number of moles = 4.75 mol
Pressure = 1.2 atm
Volume = 0.125 L
R = 0.0821 atm.L /mol.K
Temperature = ?
Solution:
Formula:
PV = nRT
T = PV/nR
T = 1.2 atm × 0.125 L / 4.75 mol × 0.0821 atm.L /mol.K
T = 0.15 / 0.39 /K
T = 0.38 K
The ideal gas constant, R, can be found using which of the following equations?
A.R=(nP)/(VT)
B.R = (PV)/(nT)
C.R=(nT)/(PV)
D.R = (PT)/(nv)
E.R = (nV)/(PT)
Answer:
B.
Explanation:
gas equation is PV = nRT
R = PV/nT
Final answer:
The ideal gas constant R is calculated from the ideal gas law PV = nRT as R = (PV)/(nT) by dividing both sides of the equation by n and T. THus, option B is correct.
Explanation:
The ideal gas constant, denoted as R, is a factor in the ideal gas law, which is expressed as PV = nRT. To find the value of R, we can rearrange this equation to solve for R. Therefore, the correct equation to calculate R using the ideal gas law would be R = (PV)/(nT). This rearrangement comes from simply dividing both sides of the ideal gas law by n and T to isolate R.
10.6 grams if NA2CO3 is dissolved in water to make 1.25 liters of solution. What is the molarity of the solution?
Answer::Molarity = 0.08 MExplanation:Given data:Mass of sodium carbonate = 10.6 gVolume of water = 1.25 LMolarity of solution = ?Solution:First of ... 10.6 grams of Na2CO3 is dissolved in water to make 1.25 liters of solution.
If 24.2 g of hydrogen react with excess oxygen and 198 g of water are produced what is the percent yield? *
Your answer
Answer:
The percent yield of the reaction is 90.9%.
Explanation:
Mass of hydrogen gas = 24.2 g
Moles of hydrogen = [tex]\frac{24.2 g}{2g/mol}=12.1 mol[/tex]
[tex]2H_2+O_2\rightarrow 2H_2O[/tex]
According to reaction, 2 moles of hydrogen gas gives 2 moles of water , then 12.1 moles of hydrogen will give:
[tex]\frac{2}{2}\times 12.1mol=12.1mol[/tex] water
Mass of 12.1 moles of water
= 12.1 mol × 18 g/mol = 217.8 g
Theoretical yield of water = 217.8 g
Experimental yield of water = 198 g
The percentage yield of reaction:
[tex]=\frac{\text{Experimental yield}}{\text{Theoretical yield}}\times 100[/tex]
[tex]=\frac{198 g}{217.8 g}\times 100=90.9\%[/tex]
The percent yield of the reaction is 90.9%.
According to Le châtelier’s principle, what happens if heat is added to a system
It depends on whether the system is endothermic or exothermic. If it is endothermic, then adding heat to the system will cause the equilibrium to shift right. Additionally, the k value will increase. Likewise, if the reaction is exothermic, adding heat will cause the equilibrium to shift left. Increasing temperature in an exothermic reaction cause k to decrease.
Le Châtelier's principle explains how a system at equilibrium responds to added heat by shifting to consume the heat, helping predict changes in a chemical equilibrium due to temperature disturbances.
Le Châtelier's principle states that if heat is added to a system at equilibrium, the system will shift to consume the heat. For example, in a liquid-vapor equilibrium, adding heat will cause the system to convert liquid to vapor, increasing the equilibrium vapor pressure.
When a system at equilibrium is disturbed by a change in temperature, it will respond in a way to counteract the disturbance, following Le Châtelier's principle. This principle helps predict how changing conditions like temperature, pressure, or concentration can affect a chemical equilibrium.
Shifting Equilibria: Systems at equilibrium can be disturbed by changes in temperature, concentration, volume, or pressure; Le Châtelier's principle describes how the system will respond to these disturbances to establish a new equilibrium.