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kinetic energy

volume

pressure

temperature

2.Which one of the following assumptions of the kinetic molecular theory explains why gases are highly compressible?

Gas particles are in constant, random motion.

No kinetic energy is lost when gas particles collide with each other.

All gases have the same average kinetic energy at a given temperature.

Gas particles are negligibly small compared to the space between them.

3.Which of the following is NOT one of the five basic assumptions of the kinetic molecular theory?

There are attractive and repulsive forces that exist between gas particles.

All gases have the same average kinetic energy at a given temperature.

No kinetic energy is lost during collisions between gas particles.

Gas particles are negligibly small compared to the distances between them.

4.What is the total pressure exerted by a mixture containing hydrogen and nitrogen if the partial pressure of hydrogen is 30.0 kPa and the partial pressure of nitrogen is 40.0 kPa?

40.0 kPa

10.0 kPa

90.0 kPa

70.0 kPa

5.The pressure of 2.0 L of a gas at constant temperature is changed from 380 mmHg to 760 mmHg. The new volume of the gas is...

4.0 L

1.0 L

1.5 L

3.0 L

6.The size of a helium gas filled balloon decreases as the temperature around the balloon is reduced from 22C to 9C on a cold winter day. This is due to:

temperature of the gas particles increasing

reduced kinetic energy of the gas particles

particles of gas shrinking in size

flexibility and rigidity of the rubber balloon changes with changing temperature

7.Collisions with the walls of a container by moving particles of a gas are responsible for:

temperature

density

volume

pressure

8.Assume pressure and temperature are constant. As gas is added to a flexible container, the volume inside the container......

Stays the same

Decreases

Increases

Depends on the gas used

10.An 8.25 L sample of oxygen is collected at 25.0 C and 1.022 atm pressure. What volume will the gas occupy at 0.940 atm and -15.0 C?

9.27 L

-5.38 L

7.77 L

8.67 L

11.The diagram below shows a gas with an initial pressure of 3060 mm Hg in a cylinder at a constant temperature. The gas expands inside the cylinder and pushes the piston up. What will be the final pressure?

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11900 mm Hg

765 mm Hg

784 mm Hg

1530 mm Hg

12.0.0297 mole of PCl5 is placed in an evacuated 2.00 liter flask and is completely vaporized at 252C. Calculate the pressure (in atmospheres) in the flask if no chemical reaction were to occur.

0.640 atm

0.851 atm

1.33 atm

0.307 atm

13.Real gases behave most like ideal gases under which set of experimental conditions?

high temperature, low pressure

low temperature, low pressure

high temperature, high pressure

low temperature, high pressure

14.At which temperature would the molecules in a sample of an ideal gas have the highest kinetic energy?

173.15 K

100 K

278.15 K

5 K

15.Equal volumes of nitrogen and oxygen, at the same temperature and pressure, would:

contain the same number of particles

have the same mass

have different kinetic energies

contain different numbers of moles

16.What is the SI unit of temperature?

Fahrenheit

Pascal

Kelvin

Celsius

17.At what temperature will a fixed amount of gas with a volume of 175 L at 288 K and 760mm Hg occupy a volume of 198 L at a pressure 0f 650mm Hg.

547 K

487 K

278.7 K

387 K

18.The SI unit of pressure is the

ampere

newton

pascal

kilojoule

19.Standard conditions when working with gases are defined as ____.

0 K and 1 kPa

0 degree C and 101.3 kPa

0 degree C and 1 kPa

0 K and 101.3 kPa

20.A glass column is filled with mercury and inverted in a pool of mercury. The mercury column stabilizes at a height of 729 mm above the pool of mercury. What is the pressure of the atmosphere?

0.959 atm

2.04 atm

0.729 atm

456 atm

21.The gas pressure in an aerosol can is 1.8 atm at 298 K. If the gas is an ideal gas, what pressure would develop in the can if it were heated to 748 K?

0.717 atm

0.095 atm

4.52 atm

3.26 atm

22.Boyle's law states that:

The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.

Equal amounts of gases occupy the same volume at constant temperature and pressure.

The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.

23.Avogadro's law states that:

The total pressure of a mixture of gases is the simple sum of the partial pressure of all of the gaseous compounds.

The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.

Equal amounts of gases occupy the same volume at constant temperature and pressure.

The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

24.According to the kinetic theory, collisions between molecules in a gas ____.

cause a loss of total kinetic energy

are perfectly elastic

are inelastic

never occur

25.Calculate the mole of 2.74 L of CO gas measured at 306 K and 945 mmHg.

1.3 mole

0.14 mole

0.088 mole

0.010 mole

26.When the temperature and number of particles of a gas are constant, which of the following is also constant?

the ratio of the pressure and volume

the product of the pressure and volume

the sum of the pressure and volume

the difference of the pressure and volume

27.Which of these changes would NOT cause an increase in the pressure of a contained gas?

The volume of the container is increased.

More of the gas is added to the container

The average kinetic energy of the gas in increased.

The temperature is increased

28.When a container is filled with 3.00 moles of H2, 2.00 moles of O2, and 1.00 mole of N2, the pressure in the container is 768 kPa. What is the partial pressure of O2?

256 kPa

64 kPa

128 kPa

192 kPa

29.Which of the following gases will effuse the most rapidly?

SO2

CO

Cl2

O2

30.A 142-mL sample of gas is collected over water at 22C and 753 torr. What is the pressure of the dry gas? (The vapor pressure of water at 22C = 20. torr)

773 torr

733 torr

162 torr

136 torr

31.A gas occupies a volume of 2.4 L at 14.1 kPa. What volume will the gas occupy at 84.6 kPa?

2.5 L

0.40 L

497 L

14 L

32.Dalton's law of partial pressures states that:

The volume of a fixed amount of gas is directly proportional to its temperature in Kelvin at constant pressure.

The volume of a fixed amount of gas is inversely proportional to its pressure at constant temperature.

The total pressure of a mixture of gases is the sum of the partial pressure of all of the gaseous compounds.

Equal amounts of gases occupy the same volume at constant temperature and pressure.

33.Gaseous chlorine is held in two separate containers at identical temperature and pressure. The volume of container 1 is 1.30 L, and it contains 6.70 mol of the gas. The volume of container 2 is 2.33 L. How many moles of the gas are in container 2?

0.452 mol

3.74 mol

12.0 mol

20.3 mol

34.The tendency of molecules to move toward areas of lower concentration is called

diffusion

effusion

suffusion

suspension

36.The combined gas law expresses the relationship between the pressure, volume, and absolute temperature of a fixed amount of gas.

True

False

37.The volume of a sample of gas, initially at 25 C and 158 mL, increases to 450. mL. What is the final temperature of the sample of gas, if the pressure in the container is kept constant?

6 C

57 C

576 C

7 C

38.The temperature of a 500. mL sample of gas increases from 150. K to 350. K. What is the final volume of the sample of gas, if the pressure in the container is kept constant?

117 mL

1170 mL

11 mL

170 mL

The diagram below shows a gas with an initial pressure of 3060 mm Hg in a cylinder at a constant temperature. The gas expands inside the cylinder and pushes the piston up. What will be the final pressure? V = 2.03 L V = 0.520 L Initial Final 11900 mm Hg 765 mm Hg O 784 mm Hg 1530 mm Hg Next W tvWhich of the following is the best qualitative graph of P versus V of a gas at constant mole and temperature? OAll of the following equations are statements of the ideal gas law except O PV T - PR OP - MRTV OP RT V OR PV MT