AnswersTX-Chemistry B-CRGas Stoichiometry

Gas Stoichiometry Answers

14 verified answers
1
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What is the molar volume of a gas at standard temperature and pressure?

A
1.0 L
B
2.4 L
C
11.2 L
D
22.4 L
2
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Consider the balanced chemical equation for the combustion of methane (CH4).Given that the molar mass of CO2 is 44.01 g/mol, how many liters of oxygen is required at STP to produce 88.0 g of CO2 from this reaction?

Question illustration
A
44.8 L
B
45.00 L
C
89.55 L
D
89.6 L
3

Consider the reaction.Which statement is true at STP? (The atomic mass of Zn is 65.39 u.)

Question illustration
A
2 mol of HCl produce 1 L of H2 gas.
B
1 L of Zn produces 1L of H2 gas.
C
65.39 g of Zn produce 22.4 L of H2 gas.
D
1 L of HCl produces 1 mol of H2 gas.
4

Under which conditions does the molar volume of a gas decrease?

A
at 273 K and at 2.0 atm
B
at 273 K and at 0.5 atm
C
at 409.5 K and at 1.0 atm
D
at 546 K and at 2.0 atm
5

Decomposition of potassium chlorate (KClO3) produces potassium chloride (KCl) and pure oxygen (O2). The balanced equation for the reaction is as follows.What volume of oxygen gas is released at STP if 10.0 g of potassium chlorate is decomposed? (The molar mass of KClO3 is 122.55 g/mol.)

Question illustration
A
0.914 L
B
1.83 L
C
2.74 L
D
3.66 L
6

Consider the reaction.How many grams of methane should be burned in an excess of oxygen at STP to obtain 5.6 L of carbon dioxide?

Question illustration
A
2.0 g
B
4.0 g
C
16.0 g
D
32.0 g
7

What volume would 3.01•1023 molecules of oxygen gas occupy at STP?

A
11.2 mL
B
22.4 mL
C
11.2 L
D
22.4 L
8

Consider the reaction.How many grams of N2 are required to produce 100.0 L of NH3 at STP?

Question illustration
A
6.25 g
B
12.5 g
C
62.5 g
D
125.0 g
9

Magnesium reacts with hydrochloric acid (HCl) as follows.How many milliliters of hydrogen gas are produced by the reaction 0.020 mol of magnesium with excess of hydrochloric acid at STP? Make sure to use the correct number of significant digits.

Question illustration
A
0.448 mL
B
0.45 mL
C
448 mL
D
450 mL
10

Nitrogen reacts with hydrogen to produce ammonia gas as follows.How many moles of nitrogen would react with excess hydrogen to produce 520 mL of ammonia?

Question illustration
A
0.0116 mol
B
0.012 mol
C
0.0232 mol
D
0.024 mol
11

most likely

I
It will double.
I
It will decrease.
I
It will increase slightly.
I
It will remain the same.
12

The gases listed are at standard temperature and pressure:· 1 mol of CO2 gas· 1 mol of N2 gas· 2 mol of O2 gasWhich statement is correct?

T
The volume of 1 mol of CO2 is greater than that of 2 mol of O2 .
T
The volume of 1 mol of CO2 is greater than that of 1 mol of N2 .
T
The volumes of 2 mol of O2 and 1 mol of N2 gases are the same.
T
The volumes of 1 mol of CO2 and 1 mol of N2 gases are the same.
13

A scientist is examining a mixture of nitrogen, hydrogen, and ammonia. The individual pressures that are exerted by nitrogen and hydrogen are 0.26 atm and 0.28 atm, respectively. If the total pressure is 0.90 atm, what is the partial pressure of ammonia?Use .

Question illustration
0
0.27 atm
0
0.36 atm
0
0.54 atm
0
0.90 atm
14

The ideal gas constant, R has several different values that could be used. Which quantity causes these differences?

p
pressure
t
temperature
v
volume
m
moles
15

Which law is described by saying that when the pressure of a gas in a sealed container is cut in half, the gas will double in volume at a steady temperature?

B
Boyle’s law
C
Charles’s law
D
Dalton’s law
G
Gay-Lussac’s law
16

A tire at 21°C has a pressure of 0.82 atm. Its temperature decreases to –3.5°C. If there is no volume change in the tire, what is the pressure after the temperature change?Use .

Question illustration
0
0.75 atm
0
0.89 atm
1
1.1 atm
1
1.3 atm
17

Consider the reaction.Which statement is true at STP? (The atomic mass of Mg is 24.31 u.)

Question illustration
3
3.0 g of Mg produce 3.0 L of H2 gas.
3
3.0 g of Mg produce 22.4 L of H2 gas.
2
24.31 g of Mg produce (3 22.4) L of H2 gas.
Option 2
(
(3 24.31) g of Mg produce (3 22.4) L of H2 gas.
Option (
18

Which quantity is held constant when working with Boyle’s, Charles’s, and Gay-Lussac’s laws?

v
volume
m
moles
p
pressure
t
temperature
19

Consider the reaction.How many grams of carbon should be burned in an excess of oxygen at STP to obtain 2.21 L of carbon dioxide?

Question illustration
1
1.18 g
2
2.21 g
4
4.12 g
4
4.34 g
20

Which proportionality shows the result of combining Avogadro’s law with Boyle’s law?

Question illustration
A
Option
Option A
B
Option
Option B
C
Option
Option C
D
Option
Option D

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