1. Chapter 12 Practice Test Assignment #2

2. Chapter 12 Understanding Concepts
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1. A sample of oxygen gas has a volume of 150 milliliters when its pressure is atmosphere. If the pressure is increased to atmosphere and the temperature remains constant, what will the new volume be?
A. 140 mL
B. 160 mL
C. 200 mL
D. 240 mL

3. Chapter 12 Understanding Concepts
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Understanding Concepts
1. A sample of oxygen gas has a volume of 150 milliliters when its pressure is atmosphere. If the pressure is increased to atmosphere and the temperature remains constant, what will the new volume be?
A. 140 mL
B. 160 mL
C. 200 mL
D. 240 mL

4. Chapter 12 Understanding Concepts
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Understanding Concepts
2. What does the kinetic-molecular theory state about ideal gas molecules?
F. They have weight and take up space.
G. They are in constant, rapid, random motion.
H. They have high densities compared to liquids and solids.
I. They exert forces of attraction and repulsion on one another.

5. Chapter 12 Understanding Concepts
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2. What does the kinetic-molecular theory state about ideal gas molecules?
F. They have weight and take up space.
G. They are in constant, rapid, random motion.
H. They have high densities compared to liquids and solids.
I. They exert forces of attraction and repulsion on one another.

6. Chapter 12 Understanding Concepts
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3. Gases that have properties like those stated in the kinetic molecular theory are said to be ideal. Which of the following gases is most nearly ideal?
A. helium
B. hydrogen
C. oxygen
D. xenon

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3. Gases that have properties like those stated in the kinetic molecular theory are said to be ideal. Which of the following gases is most nearly ideal?
A. helium
B. hydrogen
C. oxygen
D. xenon

8. Chapter 12 Understanding Concepts 4. The SI unit of pressure is
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4. The SI unit of pressure is
pascals.
newtons.
atms.
liters.

9. Chapter 12 Understanding Concepts 4. The SI unit of pressure is
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4. The SI unit of pressure is
pascals.
newtons.
atms.
liters.

10. Chapter 12 Understanding Concepts
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5. According to the kinetic-molecular theory, gases are highly compressible because the particles of which they consist
lose energy when they collide with each other.
are very apart from each other.
experience a strong force of attraction.
experience a strong force of repulsion.

11. Chapter 12 Understanding Concepts
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5. According to the kinetic-molecular theory, gases are highly compressible because the particles of which they consist
lose energy when they collide with each other.
are very apart from each other.
experience a strong force of attraction.
experience a strong force of repulsion.

12. Chapter 12 Understanding Concepts
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Understanding Concepts
Gases tend to deviate from the ideal gas law at
high pressures.
low temperatures.
high temperatures.
high pressures and low temperatures.

13. Chapter 12 Understanding Concepts
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Understanding Concepts
Gases tend to deviate from the ideal gas law at
high pressures.
low temperatures.
high temperatures.
high pressures and low temperatures.

14. Chapter 12 Understanding Concepts
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7. Which is an example of gas diffusion?
inflating a flat tire
the odor of perfume spreading throughout a room
a cylinder of oxygen stored under high pressure
All of the above

15. Chapter 12 Understanding Concepts
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7. Which is an example of gas diffusion?
inflating a flat tire
the odor of perfume spreading throughout a room
a cylinder of oxygen stored under high pressure
All of the above

16. Chapter 12 Understanding Concepts
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8. The ratios of the volumes of the gaseous reactants and products in a chemical reaction at constant temperature and pressure can be determined from the
formulas.
coefficients in the balanced equation.
subscripts in the balanced equation.
gas constant.

17. Chapter 12 Understanding Concepts
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Understanding Concepts
8. The ratios of the volumes of the gaseous reactants and products in a chemical reaction at constant temperature and pressure can be determined from the
formulas.
coefficients in the balanced equation.
subscripts in the balanced equation.
gas constant.

18. Chapter 12 Understanding Concepts
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9. According to Avogadro’s law, 1 L of H2 (g) and 1 L of O2 (g) at the same temperature and pressure
have the same mass.
have unequal volumes.
contain 1 mol of gas each.
contain equal number of molecules.

19. Chapter 12 Understanding Concepts
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9. According to Avogadro’s law, 1 L of H2 (g) and 1 L of O2 (g) at the same temperature and pressure
have the same mass.
have unequal volumes.
contain 1 mol of gas each.
contain equal number of molecules.

20. Chapter 12 Understanding Concepts
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10. Standard temperature and pressure for a gas is
0 K and 1 Pa
0°C and 1 Pa
0 K and 1 atm
0° C and 1 atm

21. Chapter 12 Understanding Concepts
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10. Standard temperature and pressure for a gas is
0 K and 1 Pa
0°C and 1 Pa
0 K and 1 atm
0° C and 1 atm

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11. If a gas is found to have a volume of 24.5 L under a pressure of kPa at 298 K, what is the number of moles of the gas?

23. Chapter 12 Understanding Concepts
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11. If a gas is found to have a volume of 24.5 L under a pressure of kPa at 298 K, what is the number of moles of the gas?
=0.501 mol

25. Chapter 12 Understanding Concepts
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12. Given 20.0 L of ammonia at 278 K and kPa, determine its volume at 303 K and 1.05 atm.

26. Chapter 12 Understanding Concepts
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12. Given 20.0 L of ammonia at 278 K and kPa, determine its volume at 303 K and 1.05 atm.
=20.8 L

28. Chapter 12 Understanding Concepts
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13. A sample of oxygen occupies 10.0 L under a pressure of 105 kPa. At what pressure will it occupy 13.4 L if the temperature does not change?

29. Chapter 12 Understanding Concepts
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13. A sample of oxygen occupies 10.0 L under a pressure of 105 kPa. At what pressure will it occupy 13.4 L if the temperature does not change?
=78.4 kPa

31. Chapter 12 Understanding Concepts
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14. If mL of HCl gas at K and kPa dissolved in pure water requires NaOH solution to neutralize in a titration experiment, what is the mass of the NaOH needed?
HCl + NaOH  NaCl + H2O

32. Chapter 12 Understanding Concepts
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14. If mL of HCl gas at K and kPa dissolved in pure water requires NaOH solution to neutralize in a titration experiment, what is the mass of the NaOH needed?
HCl + NaOH  NaCl + H2O
= g NaOH

34. Chapter 12 Understanding Concepts
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15. How many liters of water can be made from 55 grams of oxygen gas and an excess of hydrogen at a pressure of 12.4 atm and a temperature of 85° C?
2 H2(g) + O2(g)  2 H2O(g)

35. Chapter 12 Understanding Concepts
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15. How many liters of water can be made from 55 grams of oxygen gas and an excess of hydrogen at a pressure of 12.4 atm and a temperature of 85° C?
2 H2(g) + O2(g)  2 H2O(g)
=8.1 L of H2O