Question 1

A gas of twice the molecular weight as CO2 will pass through a small hole how much faster than CO2?

Accepted Answer

A)   1/2 as fast
B)   2 times as fast
C)   2 will pass through a small hole how much faster than CO2? 
A)   1/2 as fast 
B)   2 times as fast 
C)     as fast 
D)   (1/   )  as fast 
E)   4 times as fast" class="answers-bank-image d-inline" rel="preload" > as fast
D)   (1/ 2 will pass through a small hole how much faster than CO2? 
A)   1/2 as fast 
B)   2 times as fast 
C)     as fast 
D)   (1/   )  as fast 
E)   4 times as fast" class="answers-bank-image d-inline" rel="preload" > )  as fast
E)   4 times as fastF) A) and D)
G) C) and D)

Question 2

53.5 g of an ideal gas of molecular weight = 30.5 g/mol is confined at a pressure of 133 mmHg. The density of the gas is 0.228 g/L. Compute the temperature of the gas in degrees Celsius.

Accepted Answer

A)   261°C
B)   12.°C
C)   -57°C
D)   285°C
E)   -12.°CF) B) and C)
G) D) and E)

Question 3

Calculate the height in meters of a column of liquid ethanol (density = 0.7893 g/cm3)  required to exert the same pressure as 760 mmHg (d = 13.60 g/cm3) .

Accepted Answer

A)   1.31 × 104 m
B)   13.1 m
C)   70.8 m
D)   0.0708 m
E)   44.1 mF) A) and D)
G) A) and C)

Question 4

In the reaction 2 Na + 2 H2O → 2 NaOH + H2, how many liters of hydrogen at STP are produced from 50.0 grams of sodium (Na = 23.0, O = 16.0, H = 1.0 g/mol) ?

Accepted Answer

A)   (55.0/18.0) (22.4)  L
B)   (50.0/23.0) (22.4/2)  L
C)   (50.0/23.0) (2) (22.4)  L
D)   (50.0/23.0) (22.4)  L
E)   (55.0/23.0) (22.4)  LF) A) and D)
G) C) and E)

Question 5

The ideal gas equation connects three basic variables: volume, amount, and temperature of a gas.

Accepted Answer

A) True 
 B)False

Question 6

The volume in L H2(g)  (measured at 22°C and 745 mmHg)  required to react with 30.0 L CO(g)  (measured at 0 °C and 760 mmHg)  in the reaction 3 CO(g)  + 7 H2(g)  → C3H8(g)  + 3 H2O(l)  is:

Accepted Answer

A)   63.5 L
B)   74.1 L
C)   77.2 L
D)   70.0 L
E)   33.1 LF) A) and E)
G) A) and D)

Question 7

Butane (C4H10)  is used as a fuel where natural gas is not available. How many grams of butane will fill a 45.0 liter container at 27°C and 3.05 atm?

Accepted Answer

A)   26.6 g
B)   3.60 × 103 g
C)   5.58 g
D)   10.4 g
E)   324 gF) B) and E)
G) B) and D)

Question 8

A sample of N2(g)  effuses through a tiny hole in 19.0 s. How long would it take for a sample of N2O2(g)  to effuse under the same conditions?

Accepted Answer

A)   27.8 s
B)   13.0 s
C)   8.87 s
D)   40.7 s
E)   19.0 sF) C) and E)
G) B) and D)

Question 9

What volume would be occupied by a mixture of 0.33 g of hydrogen gas and 0.67 g of nitrogen gas at 157°C and 4.4 atm?

Accepted Answer

A)   12 L
B)   4.2 L
C)   3.1 L
D)   1.5 L
E)   0.55 LF) C) and D)
G) B) and C)

Question 10

The energy of molecules of a gas:

Accepted Answer

A)   is dependent on concentration
B)   is distributed over a wide range at constant temperature
C)   is the same for all molecules at constant temperature
D)   increases with a decrease in temperature
E)   increases with an increase in pressureF) All of the above
G) A) and B)

Question 11

To increase the volume of a fixed amount of gas from 100 cm3 to 200 cm3:

Accepted Answer

A)   increase the temperature from 25.0 to 50.0°C at constant pressure
B)   increase the pressure from 1.00 to 2.00 atm at constant temperature
C)   reduce the temperature from 400 K to 200 K at constant pressure
D)   reduce the pressure from 608 mm Hg to 0.40 atm at constant temperature
E)   decrease the temperature from 600 K to 400 KF) None of the above
G) C) and D)

Question 12

If 250. L of nitrogen reacts with 582 L of hydrogen by the reaction: N2 (g)  + 3 H2 (g)  → 2 NH3 (g) ,
How much nitrogen is unreacted? All gases are at the same temperature and pressure.

Accepted Answer

A)   1.9 × 102 L
B)   3.3 × 102 L
C)   56 L
D)   3.0 × 102 L
E)   41 LF) B) and C)
G) D) and E)

Question 13

The fact that a balloon filled with helium will leak more slowly than one filled with hydrogen is explained by citing:

Accepted Answer

A)   Avogadro's Hypothesis
B)   Dalton's Law
C)   Graham's Law
D)   van der Waals Theory
E)   ideal gas lawF) A) and B)
G) A) and C)

Question 14

Consider the following reaction: N2(g)  + 3 H2(g)  → 2 NH3(g) 
What volume of NH3(g)  can be produced from 200.0 L of H2(g)  if the gases are measured at 350°C and 400 atm pressure?

Accepted Answer

A)   300.0 L
B)   66.7 L
C)   133.3 L
D)   400.0 L
E)   200.0 LF) None of the above
G) C) and D)

Question 15

Liquid mercury freezes at a temperature of -39°C. The freezing point of mercury on the Kelvin scale is 234 K

Accepted Answer

A) True 
 B)False

Question 16

Calculate urms, in m/s, for H2(g)  molecules at 30°C.

Accepted Answer

A)   6.09 × 102 m/s
B)   5.26 × 103 m/s
C)   6.12 × 101 m/s
D)   1.94 × 103 m/s
E)   2.74 × 103 m/sF) A) and B)
G) A) and C)

Question 17

Which of the following is a characteristic of an ideal gas?

Accepted Answer

A)   Gas cannot be compressed infinitely.
B)   Inter-particle forces are prominent.
C)   Collisions between gas particles are perfectly elastic
D)   Collisions between gas particles and container walls are not elastic
E)   Individual gas particles occupy fixed volume.F) All of the above
G) C) and D)

Question 18

Calculate the volume of H2(g)  expressed at STP, required to react with 3.00 L of CO(g)  at STP in the following reaction: 3 CO(g)  + 7 H2(g)  → C3H8(g)  + 3 H2O(l)

Accepted Answer

A)   3.00 L
B)   7.00 L
C)   10.0 L
D)   22.4 L
E)   1.00 LF) A) and D)
G) A) and C)

Question 19

The mutual attraction of gas molecules is an important aspect of:

Accepted Answer

A)   Avogadro's Hypothesis
B)   Dalton's Law
C)   Graham's Law
D)   van der Waals Theory
E)   ideal gas lawF) D) and E)
G) None of the above

Question 20

How many liters of gas is 10.8 grams of nitrogen at 780 mmHg and 38.0°C?

Accepted Answer

A)   10.1 L
B)   1.17 L
C)   9.59 L
D)   269 L
E)   0.353 LF) A) and B)
G) C) and D)

Exam 6: Gases

Calculate urms, in m/s, for H2(g) molecules at 30°C.

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Butane (C4H10) is used as a fuel where natural gas is not available. How many grams of butane will fill a 45.0 liter container at 27°C and 3.05 atm?

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How many liters of gas is 10.8 grams of nitrogen at 780 mmHg and 38.0°C?

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In the reaction 2 Na + 2 H2O → 2 NaOH + H2, how many liters of hydrogen at STP are produced from 50.0 grams of sodium (Na = 23.0, O = 16.0, H = 1.0 g/mol) ?

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What volume would be occupied by a mixture of 0.33 g of hydrogen gas and 0.67 g of nitrogen gas at 157°C and 4.4 atm?

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The volume in L H2(g) (measured at 22°C and 745 mmHg) required to react with 30.0 L CO(g) (measured at 0 °C and 760 mmHg) in the reaction 3 CO(g) + 7 H2(g) → C3H8(g) + 3 H2O(l) is:

Correct AnswerverifiedShow Answer

A sample of N2(g) effuses through a tiny hole in 19.0 s. How long would it take for a sample of N2O2(g) to effuse under the same conditions?

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The fact that a balloon filled with helium will leak more slowly than one filled with hydrogen is explained by citing:

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53.5 g of an ideal gas of molecular weight = 30.5 g/mol is confined at a pressure of 133 mmHg. The density of the gas is 0.228 g/L. Compute the temperature of the gas in degrees Celsius.

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A gas of twice the molecular weight as CO2 will pass through a small hole how much faster than CO2?

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Liquid mercury freezes at a temperature of -39°C. The freezing point of mercury on the Kelvin scale is 234 K

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If 250. L of nitrogen reacts with 582 L of hydrogen by the reaction: N2 (g) + 3 H2 (g) → 2 NH3 (g) , How much nitrogen is unreacted? All gases are at the same temperature and pressure.

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The mutual attraction of gas molecules is an important aspect of:

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Consider the following reaction: N2(g) + 3 H2(g) → 2 NH3(g) What volume of NH3(g) can be produced from 200.0 L of H2(g) if the gases are measured at 350°C and 400 atm pressure?

Correct AnswerverifiedShow Answer

To increase the volume of a fixed amount of gas from 100 cm3 to 200 cm3:

Correct AnswerverifiedShow Answer

The ideal gas equation connects three basic variables: volume, amount, and temperature of a gas.

Correct AnswerverifiedShow Answer

The energy of molecules of a gas:

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Which of the following is a characteristic of an ideal gas?

Correct AnswerverifiedShow Answer

Calculate the volume of H2(g) expressed at STP, required to react with 3.00 L of CO(g) at STP in the following reaction: 3 CO(g) + 7 H2(g) → C3H8(g) + 3 H2O(l)

Correct AnswerverifiedShow Answer

Calculate the height in meters of a column of liquid ethanol (density = 0.7893 g/cm3) required to exert the same pressure as 760 mmHg (d = 13.60 g/cm3) .

Correct AnswerverifiedShow Answer

Calculate urms, in m/s, for H₂(g) molecules at 30°C.

Correct Answer
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Butane (C₄H₁₀) is used as a fuel where natural gas is not available. How many grams of butane will fill a 45.0 liter container at 27°C and 3.05 atm?

Correct Answer
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Correct Answer
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In the reaction 2 Na + 2 H₂O → 2 NaOH + H₂, how many liters of hydrogen at STP are produced from 50.0 grams of sodium (Na = 23.0, O = 16.0, H = 1.0 g/mol) ?

Correct Answer
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Correct Answer
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The volume in L H₂(g) (measured at 22°C and 745 mmHg) required to react with 30.0 L CO(g) (measured at 0 °C and 760 mmHg) in the reaction 3 CO(g) + 7 H₂(g) → C₃H₈(g) + 3 H₂O(l) is:

Correct Answer
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A sample of N₂(g) effuses through a tiny hole in 19.0 s. How long would it take for a sample of N₂O₂(g) to effuse under the same conditions?

Correct Answer
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Correct Answer
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Correct Answer
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A gas of twice the molecular weight as CO₂ will pass through a small hole how much faster than CO₂?

Correct Answer
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Correct Answer
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If 250. L of nitrogen reacts with 582 L of hydrogen by the reaction: N₂ (g) + 3 H₂ (g) → 2 NH₃(g) , How much nitrogen is unreacted? All gases are at the same temperature and pressure.

Correct Answer
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Correct Answer
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Consider the following reaction: N₂(g) + 3 H₂(g) → 2 NH₃(g) What volume of NH₃(g) can be produced from 200.0 L of H₂(g) if the gases are measured at 350°C and 400 atm pressure?

Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Correct Answer
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Calculate the volume of H₂(g) expressed at STP, required to react with 3.00 L of CO(g) at STP in the following reaction: 3 CO(g) + 7 H₂(g) → C₃H₈(g) + 3 H₂O(l)

Correct Answer
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Calculate the height in meters of a column of liquid ethanol (density = 0.7893 g/cm3) required to exert the same pressure as 760 mmHg (d = 13.60 g/cm³) .

Correct Answer
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