Chemistry Chapter 13 & 14 Practice Test

Matching
Match each itme with the correct statement below.

Match each item with the correct statement below.
a.	melting point	d.	evaporation	
b.	boiling point	e.	vaporization	
c.	sublimation	f.	normal boiling point	

____	1.	vaporization at the surface of a liquid that is not boiling

____	2.	the conversion of a liquid to a gas below the boiling point

____	3.	the temperature at which the vapor pressure of a liquid is equal to the external pressure

____	4.	the temperature at which the vapor pressure of a liquid is equal to 1 atmosphere

____	5.	the temperature at which a solid changes into a liquid

____	6.	the change of a solid directly to a vapor

Match each item with the correct statement below.
a.	kinetic theory	d.	barometer	
b.	atmospheric pressure	e.	kinetic energy	
c.	vapor pressure	

____	7.	All matter consists of tiny particles that are in constant motion.

____	8.	the energy an object has due to its motion

____	9.	a device used to measure atmospheric pressure

____	10.	the pressure resulting from the collision of atoms and molecules with objects

____	11.	a measure of the force exerted by a gas above a liquid

Match each item with the correct statement below.
a.	Boyle's law	d.	Graham's law	
b.	Charles's law	e.	Gay-Lussac's law	
c.	Dalton's law	f.	ideal gas law	

____	12.	For a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure.

____	13.	The volume of a fixed mass of gas is directly proportional to its Kelvin temperature, if the pressure is kept constant.

____	14.	The pressure of a gas is directly proportional to its Kelvin temperature if the volume is kept constant.

____	15.	P ´ V = n ´ R ´ T

____	16.	At constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases.

____	17.	The rate at which a gas will effuse is inversely proportional to the square root of the gas’s molar mass.

Match each item with the correct statement below.
a.	effusion	c.	diffusion 	
b.	compressibility 	d.	partial pressure 	

____	18.	a measure of how much the volume of matter decreases under pressure

____	19.	the pressure exerted by a gas in a mixture

____	20.	the escape of gas through a small hole in a container

____	21.	tendency of molecules to move to regions of lower concentration

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

____	22.	According to the kinetic theory, collisions between molecules in a gas ____.
a.	are perfectly elastic	c.	never occur	
b.	are inelastic	d.	cause a loss of total kinetic energy	

____	23.	Which of the following statements is part of the kinetic theory?
a.	The particles of a gas move independently of each other.	
b.	The particles in a gas move rapidly.	
c.	The particles in a gas are relatively far apart.	
d.	all of the above	

____	24.	What instrument is normally used to measure atmospheric pressure?
a.	thermometer	c.	vacuum	
b.	barometer	d.	manometer	

____	25.	How does the atmospheric pressure at altitudes below sea level compare with atmospheric pressure at sea level?
a.	The atmospheric pressure below sea level is higher.	
b.	The atmospheric pressure below sea level is lower.	
c.	The pressures are the same.	
d.	Differences in pressures cannot be determined.	

____	26.	What causes gas pressure in a container such as a helium balloon?
a.	the walls of the container	
b.	the vacuum maintained in the container	
c.	the simultaneous collisions of fast-moving particles in the container	
d.	atmospheric pressure acting on the outside walls of the container	

____	27.	What happens to the range of energies of the particles in matter when the temperature is increased?
a.	The range of energies becomes narrower.	
b.	The range of energies becomes broader.	
c.	The range of energies does not change.	
d.	The range of energies cannot be determined.	

____	28.	The average kinetic energy of the particles of a substance ____.
a.	is not affected by the temperature of the substance	
b.	increases as the temperature of the substance is lowered	
c.	is directly proportional to the temperature of the substance	
d.	is equal to the total energy absorbed by the substance	

____	29.	When a gas is heated, ____.
a.	all of the absorbed energy is converted to kinetic energy	
b.	some of the absorbed energy is converted to potential energy, and some is converted to kinetic energy	
c.	all of the absorbed energy is converted to potential energy	
d.	none of the energy is converted to kinetic energy	

____	30.	Consider an iron cube and an aluminum cube. If the two cubes were at the same temperature, how would the average kinetic energy of the particles in iron compare with the average kinetic energy of the particles in aluminum?
a.	The average kinetic energy of the iron particles would be greater.	
b.	The average kinetic energy of the aluminum particles would be greater.	
c.	There would be no difference in the average kinetic energies.	
d.	No determination can be made based on the information given.	

____	31.	Which states of matter can flow?
a.	gases only	c.	gases and liquids only	
b.	liquids only	d.	gases, liquids, and solids	

____	32.	What happens to the rate of evaporation of a liquid as the liquid is cooled?
a.	It increases.	c.	It does not change.	
b.	It decreases.	d.	The change cannot be determined.	

____	33.	Why does a liquid's rate of evaporation increase when the liquid is heated?
a.	More molecules have enough energy to overcome the attractive forces holding them in the liquid.	
b.	The average kinetic energy of the liquid decreases.	
c.	The surface area of the liquid is reduced.	
d.	The potential energy of the liquid increases.	

____	34.	When the vapor pressure of a liquid is equal to the atmospheric pressure, the liquid ____.
a.	has no observable changes.	c.	evaporates.	
b.	boils vigorously.	d.	begins to boil.	

____	35.	What is the pressure when a liquid is boiling at its normal boiling point?
a.	0 kPa	c.	202 kPa	
b.	101.3 kPa	d.	505 kPa	

____	36.	Most solids ____.
a.	are dense and difficult to compress	c.	are amorphous	
b.	are able to flow	d.	have a disorderly structure	

____	37.	Crystals are characterized by particular patterns that repeat in how many dimensions?
a.	one dimension only	c.	three dimensions only	
b.	two dimensions only	d.	The patterns do not repeat.	

____	38.	The escape of molecules from the surface of a liquid is known as ____.
a.	condensation	c.	evaporation	
b.	boiling	d.	sublimation	

____	39.	Which of the following elements has the ability to undergo sublimation?
a.	oxygen	c.	sodium	
b.	carbon	d.	iodine	

____	40.	How are conditions of pressure and temperature, at which two phases coexist in equilibrium, shown on a phase diagram?
a.	by a line separating the phases	
b.	by the endpoints of the line segment separating the phases	
c.	by the planar regions between lines in the diagram	
d.	by a triple point on the diagram	

____	41.	Why does the pressure inside a container of gas increase if more gas is added to the container?
a.	There is an increase in the number of collisions between particles and the walls of the container.	
b.	There is an increase in the temperature of the gas.	
c.	There is a decrease in the volume of the gas.	
d.	There is an increase in the force of the collisions between the particles and the walls of the container.	

____	42.	How does the gas propellant move when an aerosol can is used?
a.	from a region of high pressure to a region of lower pressure	
b.	from a region of high pressure to a region of equally high pressure	
c.	from a region of low pressure to a region of higher pressure	
d.	from a region of low pressure to a region of equally low pressure	

____	43.	Which of these changes would NOT cause an increase in the pressure of a contained gas?
a.	The volume of the container is increased.	
b.	More of the gas is added to the container.	
c.	The temperature is increased.	
d.	The average kinetic energy of the gas in increased.	

____	44.	Boyle's law states that ____.
a.	the volume of a gas varies inversely with pressure	
b.	the volume of a gas varies directly with pressure	
c.	the temperature of a gas varies inversely with pressure	
d.	the temperature of a gas varies directly with pressure	

____	45.	When the volume and number of particles of a gas are constant, which of the following is also constant?
a.	the sum of the pressure and temperature in kelvins	
b.	the difference of the pressure and temperature in kelvins	
c.	the product of the pressure and temperature in kelvins	
d.	the ratio of the pressure and temperature in kelvins	

____	46.	The combined gas law relates which of the following?
a.	pressure and volume only	c.	volume and temperature only	
b.	temperature and pressure only	d.	temperature, pressure, and volume	

____	47.	An ideal gas CANNOT be ____.
a.	condensed	c.	heated	
b.	cooled	d.	compressed	

____	48.	If the atmospheric pressure on Mt. Everest is one-third the atmospheric pressure at sea level, the partial pressure of oxygen on Everest is ____.
a.	one-sixth its pressure at sea level	c.	one-half its pressure at sea level	
b.	one-third its pressure at sea level	d.	equal to its pressure at sea level	

____	49.	What happens to the partial pressure of oxygen in a sample of air if the temperature is increased?
a.	It increases.	c.	It decreases.	
b.	It stays the same.	d.	The change cannot be determined.	

____	50.	When a container is filled with 3.00 moles of H, 2.00 moles of O, and 1.00 mole of N, the pressure in the container is 768 kPa. What is the partial pressure of O?
a.	256 kPa	c.	128 kPa	
b.	128 kPa	d.	192 kPa	

____	51.	If the volume of a container of air is reduced by one-half, what happens to the partial pressure of oxygen within the container?
a.	It is reduced by one-half.	c.	It is doubled.	
b.	It does not change.	d.	It is reduced by one-fourth.	

____	52.	Which of the following atoms would have the greatest velocity if each atom had the same kinetic energy?
a.	bromine	c.	ammonia	
b.	chlorine	d.	hydrogen	

Short Answer

	53.	What is a pressure of 0.520 atm equal to in mm of Hg?

	54.	At what temperature do particles theoretically have no kinetic energy?

	55.	The vapor pressure of 10 mL of ethanol at 20C is 5.85 kPa. What is the vapor pressure of 20 mL of ethanol at the same temperature?

	56.	What is the pressure (in atm) at the normal boiling point of water?

	57.	The volume of a gas is 250 mL at 340.0 kPa pressure. What will the volume be when the pressure is reduced to 50.0 kPa, assuming the temperature remains constant?

	58.	A rigid container of O has a pressure of 340 kPa at a temperature of 713 K. What is the pressure at 273 K?

	59.	A gas storage tank has a volume of 3.5  10 m when the temperature is 27C and the pressure is 101 kPa. What is the new volume of the tank if the temperature drops to –10C and the pressure drops to 95 kPa?

	60.	A mixture of gases at a total pressure of 85 kPa contains N, CO, and O. The partial pressure of the CO is 24 kPa and the partial pressure of the N is 35 kPa. What is the partial pressure of the O?

	61.	Use Graham’s law to calculate how much faster chlorine gas, Cl , will effuse than oxygen gas, O, will. The molar mass of O = 48; the  molar mass of Cl = 70.9.

	62.	A gas occupies a volume of 140 mL at 35.0C and 97 kPa. What is the volume of the gas at STP?

	63.	The gaseous product of a reaction is collected in a 25.0-L container at 27C. The pressure in the container is 300.0 kPa and the gas has a mass of 96.0 g. How many moles of the gas are in the container?

Essay

	64.	Explain why it takes longer to hard boil an egg at high altitudes than at sea level.

	65.	How does the pressure of an enclosed gas in a rigid container change when the gas is heated? Explain why this change occurs.

Chemistry Chapter 13 & 14 Practice Test
Answer Section

MATCHING

	1.	ANS:	D	PTS:	1	DIF:	L1	REF:	p. 391
OBJ:	13.2.2  Define evaporation in terms of kinetic energy.

	2.	ANS:	E	PTS:	1	DIF:	L1	REF:	p. 391
OBJ:	13.2.2  Define evaporation in terms of kinetic energy.

	3.	ANS:	B	PTS:	1	DIF:	L1	REF:	p. 393
OBJ:	13.2.4  Identify the conditions under which boiling occurs.		

	4.	ANS:	F	PTS:	1	DIF:	L1	REF:	p. 395
OBJ:	13.2.4  Identify the conditions under which boiling occurs.		

	5.	ANS:	A	PTS:	1	DIF:	L1	REF:	p. 396
OBJ:	13.3.1  Evaluate how the way particles are organized explains the properties of solids.

	6.	ANS:	C	PTS:	1	DIF:	L1	REF:	p. 401
OBJ:	13.4.1  Identify the conditions necessary for sublimation.

	7.	ANS:	A	PTS:	1	DIF:	L1	REF:	p. 385
OBJ:	13.1.1  Describe the assumptions of the kinetic theory as it applies to gases.
STA:	Ch.4.a

	8.	ANS:	E	PTS:	1	DIF:	L1	REF:	p. 385
OBJ:	13.1.1  Describe the assumptions of the kinetic theory as it applies to gases.
STA:	Ch.4.a

	9.	ANS:	D	PTS:	1	DIF:	L1	REF:	p. 386
OBJ:	13.1.2  Interpret gas pressure in terms of kinetic theory.

	10.	ANS:	B	PTS:	1	DIF:	L1	REF:	p. 386
OBJ:	13.1.2  Interpret gas pressure in terms of kinetic theory.	STA:	Ch.4.a

	11.	ANS:	C	PTS:	1	DIF:	L1	REF:	p. 392
OBJ:	13.2.3  Describe the equilibrium between a liquid and its vapor.	
STA:	Ch.4.a

	12.	ANS:	A	PTS:	1	DIF:	L1	REF:	p. 418
OBJ:	14.2.1  Describe the relationships among the temperature, pressure, and volume of a gas.
STA:	Ch.4.c

	13.	ANS:	B	PTS:	1	DIF:	L1	REF:	p. 420
OBJ:	14.2.1  Describe the relationships among the temperature, pressure, and volume of a gas.
STA:	Ch.4.c

	14.	ANS:	E	PTS:	1	DIF:	L1	REF:	p. 422
OBJ:	14.2.1  Describe the relationships among the temperature, pressure, and volume of a gas.
STA:	Ch.4.c

	15.	ANS:	F	PTS:	1	DIF:	L1	REF:	p. 426
OBJ:	14.3.1  Compute the value of an unknown variable in the equation for the ideal gas law.
STA:	Ch.4.c

	16.	ANS:	C	PTS:	1	DIF:	L1	REF:	p. 432
OBJ:	14.4.1  Relate the total pressure of a mixture of gases to the partial pressures of the component gases.
STA:	Ch.4.i

	17.	ANS:	D	PTS:	1	DIF:	L1	REF:	p. 435
OBJ:	14.4.2  Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses.
STA:	Ch.4.i

	18.	ANS:	B	PTS:	1	DIF:	L1	REF:	p. 413
OBJ:	14.1.1  Explain why gases are easier to compress than solids or liquids are.
STA:	Ch.4.c

	19.	ANS:	D	PTS:	1	DIF:	L1	REF:	p. 432
OBJ:	14.4.1  Relate the total pressure of a mixture of gases to the partial pressures of the component gases.
STA:	Ch.4.i

	20.	ANS:	A	PTS:	1	DIF:	L1	REF:	p. 435
OBJ:	14.4.2  Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses.
STA:	Ch.4.c

	21.	ANS:	C	PTS:	1	DIF:	L1	REF:	p. 435
OBJ:	14.4.2  Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses.
STA:	Ch.4.b | Ch.4.i		

MULTIPLE CHOICE

	22.	ANS:	A	PTS:	1	DIF:	L1	REF:	p. 385
OBJ:	13.1.1  Describe the assumptions of the kinetic theory as it applies to gases.
STA:	Ch.4.a

	23.	ANS:	D	PTS:	1	DIF:	L1	REF:	p. 385
OBJ:	13.1.1  Describe the assumptions of the kinetic theory as it applies to gases.
STA:	Ch.4.b

	24.	ANS:	B	PTS:	1	DIF:	L1	REF:	p. 386
OBJ:	13.1.2  Interpret gas pressure in terms of kinetic theory.

	25.	ANS:	A	PTS:	1	DIF:	L2	REF:	p. 386
OBJ:	13.1.2  Interpret gas pressure in terms of kinetic theory.	STA:	Ch.4.a

	26.	ANS:	C	PTS:	1	DIF:	L2	REF:	p. 386
OBJ:	13.1.2  Interpret gas pressure in terms of kinetic theory.	STA:	Ch.4.a

	27.	ANS:	B	PTS:	1	DIF:	L2	REF:	p. 388
OBJ:	13.1.3  Define the relationship between the Kelvin temperature and the average kinetic energy.
STA:	Ch.7.a

	28.	ANS:	C	PTS:	1	DIF:	L2	REF:	p. 389
OBJ:	13.1.3  Define the relationship between the Kelvin temperature and the average kinetic energy.
STA:	Ch.7.a

	29.	ANS:	B	PTS:	1	DIF:	L3	REF:	p. 388
OBJ:	13.1.3  Define the relationship between the Kelvin temperature and the average kinetic energy.
STA:	Ch.4.g

	30.	ANS:	C	PTS:	1	DIF:	L3	REF:	p. 388
OBJ:	13.1.3  Define the relationship between the Kelvin temperature and the average kinetic energy.
STA:	Ch.7.a

	31.	ANS:	C	PTS:	1	DIF:	L2	REF:	p. 390
OBJ:	13.2.1  Identify the factors that determine physical properties of a liquid.

	32.	ANS:	B	PTS:	1	DIF:	L2	REF:	p. 391
OBJ:	13.2.2  Define evaporation in terms of kinetic energy.	STA:	Ch.7.a

	33.	ANS:	A	PTS:	1	DIF:	L2	REF:	p. 391
OBJ:	13.2.2  Define evaporation in terms of kinetic energy.	STA:	Ch.7.a

	34.	ANS:	D	PTS:	1	DIF:	L1	REF:	p. 393
OBJ:	13.2.4  Identify the conditions under which boiling occurs.		
STA:	Ch.4.a

	35.	ANS:	B	PTS:	1	DIF:	L2	REF:	p. 395
OBJ:	13.2.4  Identify the conditions under which boiling occurs.		
STA:	Ch.4.d

	36.	ANS:	A	PTS:	1	DIF:	L2	REF:	p. 396
OBJ:	13.3.1  Evaluate how the way particles are organized explains the properties of solids.

	37.	ANS:	C	PTS:	1	DIF:	L1	REF:	p. 396
OBJ:	13.3.2  Identify the factors that determine the shape of a crystal.	

	38.	ANS:	C	PTS:	1	DIF:	L1	REF:	p. 391 | p. 392 | p. 393 | p. 401
OBJ:	13.2.2  Define evaporation in terms of kinetic energy. | 13.2.4  Identify the conditions under which boiling occurs.	STA:	Ch.7.a

	39.	ANS:	D	PTS:	1	DIF:	L1	REF:	p. 401
OBJ:	13.4.1  Identify the conditions necessary for sublimation.

	40.	ANS:	A	PTS:	1	DIF:	L2	REF:	p. 402
OBJ:	13.4.2  Describe how equilibrium conditions are represented in a phase diagram.
STA:	Ch.7.d

	41.	ANS:	A	PTS:	1	DIF:	L1	REF:	p. 415
OBJ:	14.1.2  Describe the three factors that affect gas pressure.		
STA:	Ch.4.a

	42.	ANS:	A	PTS:	1	DIF:	L1	REF:	p. 416
OBJ:	14.1.2  Describe the three factors that affect gas pressure.		
STA:	Ch.4.c

	43.	ANS:	A	PTS:	1	DIF:	L2	REF:	p. 415 | p. 416 | p. 417
OBJ:	14.1.2  Describe the three factors that affect gas pressure.		
STA:	Ch.4.c

	44.	ANS:	A	PTS:	1	DIF:	L1	REF:	p. 418
OBJ:	14.2.1  Describe the relationships among the temperature, pressure, and volume of a gas.
STA:	Ch.4.c

	45.	ANS:	D	PTS:	1	DIF:	L1	REF:	p. 422
OBJ:	14.2.1  Describe the relationships among the temperature, pressure, and volume of a gas.
STA:	Ch.4.c

	46.	ANS:	D	PTS:	1	DIF:	L1	REF:	p. 424
OBJ:	14.2.2  Use the combined gas law to solve problems.	STA:	Ch.4.c

	47.	ANS:	A	PTS:	1	DIF:	L2	REF:	p. 428
OBJ:	14.3.2  Compare and contrast real and ideal gases.	STA:	Ch.4.c

	48.	ANS:	B	PTS:	1	DIF:	L1	REF:	p. 433
OBJ:	14.4.1  Relate the total pressure of a mixture of gases to the partial pressures of the component gases.
STA:	Ch.4.i

	49.	ANS:	A	PTS:	1	DIF:	L2	REF:	p. 422 | p. 432
OBJ:	14.2.1  Describe the relationships among the temperature, pressure, and volume of a gas. | 14.4.1  Relate the total pressure of a mixture of gases to the partial pressures of the component gases.
STA:	Ch.4.i

	50.	ANS:	A	PTS:	1	DIF:	L2	REF:	p. 434
OBJ:	14.4.1  Relate the total pressure of a mixture of gases to the partial pressures of the component gases.
STA:	Ch.3.d | Ch.4.h	

	51.	ANS:	C	PTS:	1	DIF:	L2	REF:	p. 426
OBJ:	14.4.1  Relate the total pressure of a mixture of gases to the partial pressures of the component gases.
STA:	Ch.4.i

	52.	ANS:	D	PTS:	1	DIF:	L2	REF:	p. 436
OBJ:	14.4.2  Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses.
STA:	Ch.4.c

SHORT ANSWER

	53.	ANS:	
0.520 atm  760 mm Hg / 1 atm = 395 mm Hg

PTS:	1	DIF:	L2	REF:	p. 387	
OBJ:	13.1.2  Interpret gas pressure in terms of kinetic theory.	STA:	Ch.4.d

	54.	ANS:	
0 K 
–273.15C

PTS:	1	DIF:	L1	REF:	p. 389	
OBJ:	13.1.3  Define the relationship between the Kelvin temperature and the average kinetic energy.
STA:	Ch.4.f

	55.	ANS:	
5.85 kPa

PTS:	1	DIF:	L3	REF:	p. 392	
OBJ:	13.2.3  Describe the equilibrium between a liquid and its vapor.	
STA:	Ch.4.d

	56.	ANS:	
101.3 kPa  1 atm/101.3 kPa = 1.00 atm

PTS:	1	DIF:	L2	REF:	p. 387 | p. 395		
OBJ:	13.2.4  Identify the conditions under which boiling occurs.		
STA:	Ch.4.d

	57.	ANS:	
V = V   = 250 mL   = 1700 mL

PTS:	1	DIF:	L2	REF:	p. 419	
OBJ:	14.2.1  Describe the relationships among the temperature, pressure, and volume of a gas.
STA:	Ch.4.h

	58.	ANS:	
P = P   = 340 kPa   = 140 kPa

PTS:	1	DIF:	L2	REF:	p. 421	
OBJ:	14.2.1  Describe the relationships among the temperature, pressure, and volume of a gas.
STA:	Ch.4.h

	59.	ANS:	
T = 27C + 273 = 300 K; P = 101 kPa
T = –10C + 273 = 263 K; P = 95 kPa
V = P  V   = (101 kP)  (3.5  10 m)  
V = 3.26  10 m

PTS:	1	DIF:	L3	REF:	p. 424	
OBJ:	14.2.2  Use the combined gas law to solve problems.	STA:	Ch.4.h

	60.	ANS:	
 =  – ( + ) = 85 kPa – (38 kPa + 24 kP) = 26 kPa

PTS:	1	DIF:	L2	REF:	p. 434	
OBJ:	14.4.1  Relate the total pressure of a mixture of gases to the partial pressures of the component gases.
STA:	Ch.4.h | Ch.4.i		

	61.	ANS:	
 = 1.4

New Answer is Rate of Cl / Rate of O  =  square root of 48/70.9 = 8.4

PTS:	1	DIF:	L2	REF:	p. 436	
OBJ:	14.4.2  Explain how the molar mass of a gas affects the rate at which the gas diffuses and effuses.
STA:	Ch.3.d | Ch.4.h | Ch.4.i

	62.	ANS:	
T = 35.0C + 273 = 308 K
T = 0.0C + 273 = 273 K
V = P  V  
V = 97 kPa  140 mL   = 120 mL

PTS:	1	DIF:	L3	REF:	p. 424	
OBJ:	14.2.2  Use the combined gas law to solve problems.	STA:	Ch.3.d | Ch.4.h

	63.	ANS:	
n =  =  = 3.0 mol

PTS:	1	DIF:	L2	REF:	p. 427	
OBJ:	14.3.1  Compute the value of an unknown variable in the equation for the ideal gas law.
STA:	Ch.3.d | Ch.4.h	

ESSAY

	64.	ANS:	
At high altitudes, atmospheric pressure is lower. Therefore, the boiling point of water is lower than at sea level. Because the highest temperature the water can reach while boiling is lower, the cooking time is increased.

PTS:	1	DIF:	L3	REF:	p. 394	
OBJ:	13.2.4  Identify the conditions under which boiling occurs.		
STA:	Ch.4.c

	65.	ANS:	
The pressure increases when the gas is heated because increasing the temperature of the gas increases the average kinetic energy of the particles in the gas. With an increase in average kinetic energy, there will be an increase in the number of collisions between the particles and the container walls. In addition, because the particles are moving faster, on average, the collisions will occur with greater force. Both factors, the increased frequency of collision and the increased force of the collisions, contribute to the increase in pressure.

PTS:	1	DIF:	L3	REF:	p. 417	
OBJ:	14.1.2  Describe the three factors that affect gas pressure.		
STA:	Ch.4.g