Ch 10 Chemistry Test

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Multiple Choice - 2pts each

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

According to the kinetic-molecular theory, particles of matter

a.	are in constant motion.	c.	have different colors.
b.	have different shapes.	d.	are always fluid.

The kinetic-molecular theory explains the properties of solids, liquids, and gases in terms of the energy of the particles and

a.	gravitational forces.	c.	diffusion.
b.	the forces that act between the particles.	d.	the mass of the particles.

An ideal gas is an imaginary gas

a.	not made of particles.
b.	that conforms to all of the assumptions of the kinetic theory.
c.	whose particles have zero mass.
d.	made of motionless particles.

Unlike in an ideal gas, in a real gas

a.	all particles move in the same direction.
b.	all particles have the same kinetic energy.
c.	the particles cannot diffuse.
d.	the particles exert attractive forces on each other.

If two moving steel balls collide, their total energy after the collision is the same as before. This is an example of

a.	Boyle's law.	c.	an elastic collision.
b.	the law of gravity.	d.	both Boyle's law and Charles's law.

Which is an example of gas diffusion?

a.	inflating a flat tire
b.	the odor of perfume spreading throughout a room
c.	a cylinder of oxygen stored under high pressure
d.	All of the above

If a gas with an odor is released in a room, it quickly can be detected across the room because it

a.	diffuses.	c.	is compressed.
b.	is dense.	d.	condenses.

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.

Which is an example of effusion?

a.	air slowly escaping from a pinhole in a tire
b.	the aroma of a cooling pie spreading across a room
c.	helium dispersing into a room after a balloon pops
d.	oxygen and gasoline fumes mixing in an automobile carburetor

10.

What happens to the volume of a gas during compression?

a.	The volume increases.
b.	The volume decreases.
c.	The volume remains constant.
d.	It is impossible to tell because all gases are different.

11.

Which gases behave most like an ideal gas?

a.	gases composed of highly polar molecules
b.	gases composed of monatomic, nonpolar molecules
c.	gases composed of diatomic, polar molecules
d.	gases near their condensation temperatures

12.

Pressure is the force per unit

a.	volume.	c.	length.
b.	surface area.	d.	depth.

13.

What is the SI unit of force?

a.	torr	c.	pound
b.	pascal	d.	newton

14.

If force is held constant as surface area decreases, pressure

a.	remains constant.
b.	decreases.
c.	increases.
d.	increases or decreases, depending on the volume change.

15.

What does the constant bombardment of gas molecules against the inside walls of a container produce?

a.	temperature	c.	pressure
b.	density	d.	diffusion

16.

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.

17.

What instrument measures atmospheric pressure?

a.	barometer	c.	vacuum pump
b.	manometer	d.	torrometer

18.

A pressure of 745 mm Hg equals

a.	745 torr.	c.	1 pascal.
b.	1 torr.	d.	745 pascal.

19.

Convert the pressure 0.840 atm to mm Hg.

a.	365 mm Hg	c.	638 mm Hg
b.	437 mm Hg	d.	780 mm Hg

20.

Convert the pressure 2.50 atm to kPa.

a.	1 kPa	c.	760 kPa
b.	253 kPa	d.	1000 kPa

21.

Standard temperature is exactly

a.	100ºC.	c.	0ºC.
b.	273ºC.	d.	0 K.

22.

Standard pressure is the pressure exerted by a column of mercury exactly

a.	273 mm high.	c.	760 cm high.
b.	760 mm high.	d.	1.00 m high.

23.

If the height of mercury in a barometer at 0ºC is less than 760 mm Hg, then

a.	the atmospheric pressure is less than standard atmospheric pressure.
b.	the atmospheric pressure is greater than standard atmospheric pressure.
c.	the atmospheric pressure is equal to standard atmospheric pressure.
d.	the atmospheric pressure cannot be determined.

24.

To study the relationship between the temperature and volume of a gas, which factor must be held constant?

a.	elasticity	c.	kinetic energy
b.	fluidity	d.	pressure

25.

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

26.

The volume of a gas is 400.0 mL when the pressure is 1.00 atm. At the same temperature, what is the pressure at which the volume of the gas is 2.0 L?

a.	0.5 atm	c.	0.20 atm
b.	5.0 atm	d.	800 atm

27.

The pressure of a sample of helium is 2.0 atm in a 200-mL container. If the container is compressed to 10 mL without changing the temperature, what is the new pressure?

a.	200 atm	c.	100 atm
b.	0.10 atm	d.	40. atm

28.

A sample of gas collected at 750. mm Hg occupies 250. mL. At constant temperature, what pressure does the gas exert if the volume increases to 300. mL?

a.	50. mm Hg	c.	625. mm Hg
b.	550. mm Hg	d.	900. mm Hg

29.

A 180.0 mL volume of gas is measured at 87.0ºC. If the pressure remains unchanged, what is the volume of the gas at standard temperature?

a.	0.0 mL	c.	136 mL
b.	0.5 mL	d.	410 mL

30.

The volume of a gas is 93 mL when the temperature is 91ºC. If the temperature is reduced to 0ºC without changing the pressure, what is the new volume of the gas?

a.	70 mL	c.	120 mL
b.	100 mL	d.	273 mL

31.

If the temperature of 50.0 L of a gas at 40.0ºC falls by 10.0Cº, what is the new volume of the gas if the pressure is constant?

a.	45.0 L	c.	52.0 L
b.	48.4 L	d.	55.0 L

32.

The pressure of a sample of gas at a constant volume is 8.0 atm at 70.ºC. What is the pressure at 20.ºC?

a.	0.16 atm	c.	9.4 atm
b.	6.8 atm	d.	58 atm

33.

Suppose that the pressure of 1.00 L of gas is 380. mm Hg when the temperature is 200. K. At what temperature is the volume 2.00 L and the pressure 0.750 atm?

a.	1.00 K	c.	219ºC
b.	600. K	d.	67.0 K

34.

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

35.

A 70.0 L sample of gas at 20.0ºC and 600. mm Hg expands to 90.0 L at 15.0ºC. What is the new gas pressure?

a.	318 mm Hg	c.	583 mm Hg
b.	459 mm Hg	d.	710 mm Hg

36.

Who developed the concept that the total pressure of a mixture of gases is the sum of their partial pressures?

a.	Charles	c.	Kelvin
b.	Boyle	d.	Dalton

37.

Three samples of gas each exert 740. mm Hg in separate 2 L containers. What pressure do they exert if they are all placed in a single 2 L container?

a.	247 mm Hg	c.	1480 mm Hg
b.	740 mm Hg	d.	2220 mm Hg

38.

A mixture of four gases exerts a total pressure of 860 mm Hg. Gases A and B each exert 220 mm Hg. Gas C exerts 110 mm Hg. What pressure is exerted by gas D?

a.	165 mm Hg	c.	860 mm Hg
b.	310 mm Hg	d.	cannot be determined

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

39.

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

40.

A sample of nitrogen is collected by water displacement at 730.0 mm Hg and 20ºC. What is the partial pressure of the nitrogen?

a.	17.5 mm Hg	c.	717.2 mm Hg
b.	712.5 mm Hg	d.	747.5 mm Hg

Completion

Complete the chart below. Each box is worth 2pts (18 points total).

41.

Name 3 of the four gas laws that we have studied in this chapter.	Write the formula used when solving problems.	What remains constant? K is not an acceptable answer.
1)
2)
3)

Short Answer (2pts)

42.

Name 3 specific activities/ assignments that helped you the most in learning the material in chapter 10 (think about it, this will help me understand how you learn best).