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Gas Chemistry



Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

1. 

The kinetic-molecular theory explains the behavior of
a.
gases only.
c.
liquids and gases.
b.
solids and liquids.
d.
solids, liquids, and gases.
 

2. 

According to the kinetic-molecular theory, what is the most significant difference between gases and liquids?
a.
the shapes of the particles
b.
the mass of each particle
c.
the distance between the particles
d.
the type of collision that occurs between particles
 

3. 

According to the kinetic-molecular theory, how does a gas expand?
a.
Its particles become larger.
b.
Collisions between particles become elastic.
c.
Its temperature rises.
d.
Its particles move greater distances.
 

4. 

Pressure is the force per unit
a.
volume.
c.
length.
b.
surface area.
d.
depth.
 

5. 

What does the constant bombardment of gas molecules against the inside walls of a container produce?
a.
temperature
c.
pressure
b.
density
d.
diffusion
 

6. 

Why does a can collapse when a vacuum pump removes air from the can?
a.
The inside and outside forces balance out and crush the can.
b.
The unbalanced outside force from atmospheric pressure crushes the can.
c.
The atmosphere exerts pressure on the inside of the can and crushes it.
d.
The vacuum pump creates a force that crushes the can.
 

7. 

Standard temperature is exactly
a.
100ºC.
c.
0ºC.
b.
273ºC.
d.
0 K.
 

8. 

If the pressure and temperature of a gas are held constant and some gas is added to the container or some is allowed to escape, a change in which of the following can be observed?
a.
kinetic energy
c.
elasticity
b.
volume
d.
fluidity
 

9. 

Suppose the temperature of the air in a balloon is increased. If the pressure remains constant, what quantity must change?
a.
volume
c.
compressibility
b.
number of molecules
d.
adhesion
 

10. 

If the temperature of a container of gas remains constant, how could the pressure of the gas increase?
a.
The mass of the gas molecules increases.
b.
The diffusion of the gas molecules increases.
c.
The size of the container increases.
d.
The number of gas molecules in the container increases.
 

11. 

Pressure and volume changes at a constant temperature can be calculated using
a.
Boyle's law.
c.
Kelvin's law.
b.
Charles's law.
d.
Dalton's law.
 

12. 

If V, P, and T represent the original volume, pressure, and temperature in the correct units, and V', P', and T' represent the new conditions, what is the combined gas law?
a.
gaswebtest_files/i0130000.jpg
c.
gaswebtest_files/i0130001.jpg
b.
gaswebtest_files/i0130002.jpg
d.
gaswebtest_files/i0130003.jpg
 
 
         Water Vapor Pressure
Temperature (ºC)
Pressure (mm Hg)
0
      4.6
5
      6.5
10
      9.2
15
      12.8
20
      17.5
25
      23.8
30
      31.8
35
      42.2
40
      55.3
50
      92.5
 

13. 

A sample of gas is collected by water displacement at 600.0 mm Hg and 30ºC. What is the partial pressure of the gas?
a.
568.2 mm Hg
c.
630 mm Hg
b.
600.0 mm Hg
d.
631.8 mm Hg
 

14. 

If gas A has a molar mass greater than that of gas B and samples of each gas at identical temperatures and pressures contain equal numbers of molecules, then
a.
the volumes of gas A and gas B are equal.
b.
the volume of gas A is greater than that of gas B.
c.
the volume of gas B is greater than that of gas A.
d.
their volumes are proportional to their molar masses.
 

15. 

The expression V = kn is a statement of
a.
the ideal gas law.
c.
Graham's law of effusion.
b.
the law of combining volumes.
d.
Avogadro's principle.
 

16. 

The standard molar volume of a gas is all of the following except
a.
the volume occupied by 1 mol of a gas at STP.
b.
equal for all gases under the same conditions.
c.
22.4 L at STP.
d.
dependent upon the size of the molecules.
 

17. 

All of the following equations are statements of the ideal gas law except
a.
P = nRTV
c.
gaswebtest_files/i0190000.jpg
b.
gaswebtest_files/i0190001.jpg
d.
gaswebtest_files/i0190002.jpg
 

18. 

A gas sample with a mass of 0.467 g is collected at 20.ºC and 732.5 mm Hg. The volume is 200. mL. What is the molar mass of the gas?
a.
58 g/mol
c.
290 g/mol
b.
180 g/mol
d.
730 g/mol
 

19. 

What is the number of moles of H2 produced when 23 g of sodium react with water according to the equation 2Na(s) + 2H2O(l) ® 2NaOH(aq) + H2(g)?
a.
0.50 mol
c.
2 mol
b.
1 mol
d.
4 mol
 

20. 

When carbon burns, carbon dioxide is produced by the reaction C + O2 ® CO2. If 14 L of CO2 are produced at STP, how many grams of carbon (atomic mass 12) were used?
a.
7.5 g
c.
17.5 g
b.
11.2 g
d.
75 g
 

21. 

According to the kinetic-molecular theory, particles of a gas
a.
attract each other but do not collide.
b.
repel each other and collide.
c.
neither attract nor repel each other but collide.
d.
neither attract nor repel each other and do not collide.
 

22. 

The volume of a gas collected when the temperature is 11.0ºC and the pressure is 710 mm Hg measures 14.8 mL. What is the calculated volume of the gas at 20.0ºC and 740 mm Hg?
a.
7.8 mL
c.
14.6 mL
b.
13.7 mL
d.
15 mL
 

23. 

To correct for the partial pressure of water vapor, the vapor pressure of H2O at the collecting temperature is
a.
divided by 22.4.
c.
subtracted from the total gas pressure.
b.
multiplied by 22.4.
d.
added to the total gas pressure.
 



 
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