Question 1

If 0.24 mol of He were added to a balloon, how large would the balloon grow? Atmospheric pressure is 0.9871 bar and the ambient temperature is 23.2 °C.

Accepted Answer

A) 5.99 L 
B) 6.54 L 
C) 3.73 L 
D) 6.49 L 
E) 7.28 L 
A) 5.99 L 
B) 6.54 L 
C) 3.73 L 
D) 6.49 L 
E) 7.28 L

Question 2

Convert 717.28 mmHg to bar.

Accepted Answer

A) 1.046 bar 
B) 0.9438 bar 
C) 1.060 bar 
D) 0.9563 bar 
E) 0.8971 bar 
A) 1.046 bar 
B) 0.9438 bar 
C) 1.060 bar 
D) 0.9563 bar 
E) 0.8971 bar

Question 3

What is the definition of diffusion?

Accepted Answer

A) gas molecules mix equally 
B) gas molecules spread out in a concentration gradient 
C) gas molecules escape from a container into a vacuum through a small hole 
D) average distance between collisions 
E) gas molecules mix unequally 
A) gas molecules mix equally 
B) gas molecules spread out in a concentration gradient 
C) gas molecules escape from a container into a vacuum through a small hole 
D) average distance between collisions 
E) gas molecules mix unequally

Question 4

Determine the density of CO2 gas at 278 K and 1.00 bar.

Accepted Answer

A) 1.14 g L-1 
B) 2.37 g L-1 
C) 1.90 g L-1 
D) 3.08 g L-1 
E) 2.11 g L-1 
A) 1.14 g L-1 
B) 2.37 g L-1 
C) 1.90 g L-1 
D) 3.08 g L-1 
E) 2.11 g L-1

Question 5

What pressure will 14.0 g of CO exert in a 3.5 L container at 75 °C?

Accepted Answer

A) 4.1 bar 
B) 5.0 bar 
C) 6.4 bar 
D) 1.1 bar 
E) 2.3 bar 
A) 4.1 bar 
B) 5.0 bar 
C) 6.4 bar 
D) 1.1 bar 
E) 2.3 bar

Question 6

Match the following.

-Boyle's law

Accepted Answer

A) measures blood pressure 
B) measures pressure of a gas 
C) V1/n1 = V2/n2 
D) PV = nRT 
E) P1V1 = P2V2
F)measures atmospheric pressure
G)V1/T1 = V2/T2
H)PT = PA + PB + PC ... 
A) measures blood pressure 
B) measures pressure of a gas 
C) V1/n1 = V2/n2 
D) PV = nRT 
E) P1V1 = P2V2
F)measures atmospheric pressure
G)V1/T1 = V2/T2
H)PT = PA + PB + PC ...

Question 7

Convert 3.1473 atm to bar.

Accepted Answer

A) 4.976 bar 
B) 3.189 bar 
C) 2.577 bar 
D) 4.112 bar 
E) 3.875 bar 
A) 4.976 bar 
B) 3.189 bar 
C) 2.577 bar 
D) 4.112 bar 
E) 3.875 bar

Question 8

Determine the density of O3 gas at 341 K and 2.14 bar.

Accepted Answer

A) 3.62 g L-1 
B) 2.91 g L-1 
C) 0.321 g L-1 
D) 4.82 g L-1 
E) 3.17 g L-1 
A) 3.62 g L-1 
B) 2.91 g L-1 
C) 0.321 g L-1 
D) 4.82 g L-1 
E) 3.17 g L-1

Question 9

A 2.75 L container filled with CO2 gas at 25 °C and 2.25 bar springs a leak. When the container is resealed, the pressure is 1.85 bar and the temperature is 10 °C. How many moles of gas were lost?

Accepted Answer

A) 0.0335 mol 
B) 0.728 mol 
C) 0.882 mol 
D) 3.39 mol 
A) 0.0335 mol 
B) 0.728 mol 
C) 0.882 mol 
D) 3.39 mol

Question 10

What is the temperature of NO2 gas if the average speed (actually the root mean square speed)of the molecules is 750 m s-1?

Accepted Answer

A) 1.38 K 
B) 1.04 × 103 K 
C) 1.38 × 103 K 
D) 1.04 × 106 K 
A) 1.38 K 
B) 1.04 × 103 K 
C) 1.38 × 103 K 
D) 1.04 × 106 K

Question 11

Convert 29.592 inches Hg to bar.

Accepted Answer

A) 0.9889 bar 
B) 1.011 bar 
C) 1.002 bar 
D) 1.023 bar 
E) 0.9980 bar 
A) 0.9889 bar 
B) 1.011 bar 
C) 1.002 bar 
D) 1.023 bar 
E) 0.9980 bar

Question 12

How many molecules of XeF6 are formed from 12.9 L of F2 (at 298 K and 2.635 bar)according to the following reaction? Assume that there is excess Xe. Xe(g)+ 3F2(g)→ XeF6(g)

Accepted Answer

A) 1.21 × 1023 molecules XeF6 
B) 8.25 × 1023 molecules XeF6 
C) 2.75 × 1023 molecules XeF6 
D) 7.29 × 1023 molecules XeF6 
E) 1.37 × 1023 molecules XeF6 
A) 1.21 × 1023 molecules XeF6 
B) 8.25 × 1023 molecules XeF6 
C) 2.75 × 1023 molecules XeF6 
D) 7.29 × 1023 molecules XeF6 
E) 1.37 × 1023 molecules XeF6

Question 13

Using the graph below, determine the gas that has the lowest density at STP.

Accepted Answer

A) A 
B) B 
C) C 
D) D 
E) All of the gases have the same density at STP. 
A) A 
B) B 
C) C 
D) D 
E) All of the gases have the same density at STP.

Question 14

Give the temperature and pressure at STP.

Accepted Answer

A) 0° C and 1.00 bar 
B) 0 K and 1.00 bar 
C) 25° C and 30.00 in Hg 
D) 300 K and 1 Torr Hg 
E) 0° C and 1 mmHg 
A) 0° C and 1.00 bar 
B) 0 K and 1.00 bar 
C) 25° C and 30.00 in Hg 
D) 300 K and 1 Torr Hg 
E) 0° C and 1 mmHg

Question 15

Which of the following samples will have the greatest average speed at 355 K?

Accepted Answer

A) Ne 
B) C2H4 
C) Cl2 
D) CH4 
E) All of these samples will have the same average speed at the same temperature. 
A) Ne 
B) C2H4 
C) Cl2 
D) CH4 
E) All of these samples will have the same average speed at the same temperature.

Question 16

A fixed amount of gas at 25.0 °C occupies a volume of 10.0 L when the pressure is 0.8386 bar. Use Charles's law to calculate the volume (L)the gas will occupy when the temperature is increased to   while maintaining the pressure at 0.8386 bar.

Accepted Answer

A) 10.9 L 
B) 13.2 L 
C) 2.07 L 
D) 7.56 L 
E) 48.4 L 
A) 10.9 L 
B) 13.2 L 
C) 2.07 L 
D) 7.56 L 
E) 48.4 L

Question 17

Convert 1.25 atm to bar.

Accepted Answer

A) 1.23 bar 
B) 0.975 bar 
C) 1.27 bar 
D) 0.7874 bar 
E) 1.25 bar 
A) 1.23 bar 
B) 0.975 bar 
C) 1.27 bar 
D) 0.7874 bar 
E) 1.25 bar

Question 18

A gas bottle contains 0.250 mol of gas at 0.973 bar pressure. If the final pressure is 1.165 bar, how many moles of gas were added to the bottle?

Accepted Answer

A) 0.0262 mol 
B) 0.0493 mol 
C) 0.276 mol 
D) 0.299 mol 
A) 0.0262 mol 
B) 0.0493 mol 
C) 0.276 mol 
D) 0.299 mol

Question 19

Which of the following samples will have the greatest volume at STP?

Accepted Answer

A) 22 g CO 
B) 22 g He 
C) 22 g O2 
D) 22 g Cl2 
E) All of these samples would have the same volume at STP. 
A) 22 g CO 
B) 22 g He 
C) 22 g O2 
D) 22 g Cl2 
E) All of these samples would have the same volume at STP.

Question 20

The volume of a gas is inversely proportional to the pressure of a gas. What is this known as?

Accepted Answer

A) Avogadro's law 
B) Ideal gas law 
C) Charles's law 
D) Boyle's law 
E) Dalton's law 
A) Avogadro's law 
B) Ideal gas law 
C) Charles's law 
D) Boyle's law 
E) Dalton's law

Exam 5: Gases

If 0.24 mol of He were added to a balloon, how large would the balloon grow? Atmospheric pressure is 0.9871 bar and the ambient temperature is 23.2 °C.

Convert 717.28 mmHg to bar.

What is the definition of diffusion?

Determine the density of CO2 gas at 278 K and 1.00 bar.

What pressure will 14.0 g of CO exert in a 3.5 L container at 75 °C?

Match the following. -Boyle's law

Convert 3.1473 atm to bar.

Determine the density of O3 gas at 341 K and 2.14 bar.

A 2.75 L container filled with CO2 gas at 25 °C and 2.25 bar springs a leak. When the container is resealed, the pressure is 1.85 bar and the temperature is 10 °C. How many moles of gas were lost?

What is the temperature of NO2 gas if the average speed (actually the root mean square speed)of the molecules is 750 m s-1?

Convert 29.592 inches Hg to bar.

How many molecules of XeF6 are formed from 12.9 L of F2 (at 298 K and 2.635 bar)according to the following reaction? Assume that there is excess Xe. Xe(g)+ 3F2(g)→ XeF6(g)

Using the graph below, determine the gas that has the lowest density at STP.

Give the temperature and pressure at STP.

Which of the following samples will have the greatest average speed at 355 K?

A fixed amount of gas at 25.0 °C occupies a volume of 10.0 L when the pressure is 0.8386 bar. Use Charles's law to calculate the volume (L)the gas will occupy when the temperature is increased to while maintaining the pressure at 0.8386 bar.

Convert 1.25 atm to bar.

A gas bottle contains 0.250 mol of gas at 0.973 bar pressure. If the final pressure is 1.165 bar, how many moles of gas were added to the bottle?

Which of the following samples will have the greatest volume at STP?

The volume of a gas is inversely proportional to the pressure of a gas. What is this known as?

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Filters

Determine the density of CO₂ gas at 278 K and 1.00 bar.

Determine the density of O₃ gas at 341 K and 2.14 bar.

A 2.75 L container filled with CO₂ gas at 25 °C and 2.25 bar springs a leak. When the container is resealed, the pressure is 1.85 bar and the temperature is 10 °C. How many moles of gas were lost?

What is the temperature of NO₂ gas if the average speed (actually the root mean square speed)of the molecules is 750 m s^-1?

How many molecules of XeF₆are formed from 12.9 L of F₂ (at 298 K and 2.635 bar)according to the following reaction? Assume that there is excess Xe. Xe(g)+ 3F₂(g)→ XeF₆(g)