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Worksheets

Final Review HChem

Total questions: 160

Worksheet time: 4hrs 39mins

Name
Class
Date
1.
A balloon will pop in the atmosphere because..
a)
Pressure goes down volume goes up
b)
Pressure goes up volume goes down
c)
temperature goes down volume goes up
d)
volume goes down temperature goes down
2.
Convert: 253 C to K:
a)
526 K
b)
625 K
c)
0 K
d)
186 K
3.

If a gas is at 0.95 atm, how many kPa is this?

a)

0.35 kPa

b)

1.07 kPa

c)

96 kPa

d)

400,025 kPa

4.

_________ is a measure of the average kinetic energy of the particles in an object. When temperature increases, the motion of these particles also increases.

a)

Measurement

b)

Pressure

c)

Temperature

5.
Gas pressure is caused by
a)
gas molecules colliding with surfaces
b)
gas molecules condensing to a liquid
c)
gas molecules hitting other gas molecule
d)
barometers
6.
If you increase the pressure, what will happen to the temperature, if volume is constant?
a)
Increase
b)
Decrease
c)
Stay the same
d)
It will Blow Up
7.
Which of the following would increase the (gas) pressure of a system?
a)
Increase the Temperature
b)
Pump in more gas
c)
Decrease the volume
d)
All of these
8.
Dalton's Law states...
a)
that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure.
b)
that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases
c)
how gases tend to expand when heated
d)
that the density of an ideal gas at constant pressure varies inversely with the absolute temperature of the gas.
9.
At STP, what is pressure in atmospheres?
a)
1 atm
b)
10 atm
c)
0 atm
d)
100 atm
10.

At STP what is the temperature?

a)

0 K

b)

100 C

c)

273 K

d)

30 F

11.

At STP, how many liters are in 2 moles of oxygen gas?

a)

22.4 L

b)

44.8 L

c)

11.2 L

d)

24.2 L

12.

What happens at absolute zero?

a)

All Motions cease

b)

everything turns to a solid

c)

everything dies

d)

who knows?

13.
How do gas molecules move? 
a)
in an orderly fashion 
b)
constantly and randomly
c)
in straight line paths
d)
in a circular motion
14.
Which container will have a lower pressure?
a)
left
b)
right
c)
they both have the same pressure
d)
I don't know
15.
What is the device that measures atmospheric pressure?
a)
Aerometer
b)
Annemeter
c)
Barometer
d)
Humidity Detector
16.

A student inflates a balloon with helium then places it in the freezer. The student should expect

a)

the balloon's volume to increase

b)

the balloon's volume to decrease

c)

the balloon's moles to increase

d)

the balloon's moles to decrease

17.

If a hairspray can is heated, what can be expected of the pressure of the gas inside the can?

a)

The pressure will increase

b)

The pressure will decrease

c)

The pressure will remain constant

d)

The pressure will equalize

18.
In order to convert to Kelvin, you add ______ to the Celsius measurement.
a)
372
b)
273
c)
237
d)
732
19.
In the ideal gas law, what does the variable n represent? 
a)
gas constant 
b)
moles 
c)
Temperature 
d)
Volume 
20.
Boyle's PV law : When _______ is held constant, the pressure and volume of a gas are ________  proportional
a)
temperature,  equally
b)
mass, inversely
c)
temperature, inversely
d)
mass, equally
21.
When a cold tire is inflated to a certain pressure and then is warmed up due to friction with the road, the pressure increases. This happens because the
a)
air molecules hit the walls of the tire less frequently
b)
rubber in the tires reacts with oxygen in the atmosphere
c)
air molecules speed up and collide with the tire walls more often
d)
air molecules diffuse rapidly through the walls of the tire.
22.

Three gases are mixed together in a container with a total pressure of 4.8 atm. If two of the gases have pressures of 1.2 atm and 1.5 atm, what is the pressure of the third gas?

a)

2.5 atm

b)

1.8 atm

c)

2.1 atm

d)

1.3 atm

23.

If pressure is constant, temperature and volume have a(n) ________ relationship with each other.

a)

Direct

b)

Inverse

24.

If temperature is constant, pressure and volume have a(n) ________ relationship with each other.

a)

direct

b)

indirect

25.

What is the name of this instrument, which is used to measure atmospheric pressure?

a)

barometer

b)

thermometer

c)

anemometer

d)

voltmeter

26.
Lighter gases have a ________________ rate of effusion.
a)
faster 
b)
slower
c)
rate of effusion does not depend on mass.
27.
Effusion is
a)
used to describe the combustibility of a gas.
b)
ability of a gas to escape through a tiny opening
c)
what occurs after diffusion.
d)
the ability of a gas to mix with other gases.
28.
Which gas diffuses slower?
a)

ammonia (NH3)

b)
oxygen
29.
Why does ice float?
a)
As water freezes, it expands and its density decreases.
b)
As water freezes, it takes up more hydrogen from the atmosphere, causing it to have a greater buoyancy.
c)
As water freezes, air becomes trapped between the hydrogen bonds of water molecules.
d)
As water freezes, it takes up more oxygen from the atmosphere, causing it to have a greater buoyancy.
30.
The substance that gets dissolved is called solvent.
True or False?
a)
True.
b)
False.
31.
Type of mixture in which all substances are evenly distributed is a?
a)
Solution
b)
Solute
c)
Solvent
32.
What is a solvent?
a)
The substance that does the dissolving in a solution.
b)
The substance that is being dissolved in a solution.
c)
The mixing of different substances.
d)
The process in which neutral molecules lose or gain electrons
33.
This is the part of a solution that dissolves
a)
Solute
b)
Solvent
c)
Solution
d)
Mixture 
34.
What is the reason why oil and water don't mix?
a)
Oil is too heavy to mix with water
b)
Water can only mix with polar molecules 
c)
Water can only mix with non-polar molecules
d)
Oil is too light to mix with water 
35.
Which end of the water molecule has a slightly positive charge?
a)
the oxygen end
b)
the hydrogen end
c)
both ends are slightly positive
d)
neither end is positive
36.

Surface tension is the property of water in which...

a)

water molecules at the surface tend to stick together.

b)

water spills easily.

c)

water tends to be see-through.

d)

water tends to push up into a dome over a container before it finally spills.

37.

What is a surfactant?

a)

A molecule that does not adsorb at surfaces

b)

A substance that prevent bubble formation

c)

A molecule that reduces surface tension of a liquid

d)

A substance that is always water soluble

38.

A substance that conducts an electrical current when dissolved in water is called

a)

catalyst

b)

metalloid

c)

electrolyte

d)

nonelectrolyte

39.
Solutions in which electric currents cannot run through are said to be
a)
noncolloidal
b)
electrolytes
c)
nonelectrolytes
d)
conductors
40.

Which of the following containers most likely contains sugar?


A B

a)

Container A because it forms ions.

b)

Container B because it forms ions.

c)

Container A because it does not form ions.

d)

Container B because it does not form ions.

41.
Which technique could increase or speed up the rate of dissolving?
a)
Allowing the mixture to settle
b)
Stirring the mixture
c)
Adding more powder
d)
Adding more water
42.

A teacher performs a demonstration in which she places a conductivity tester into a series of solutions. Which substance listed below would have made the bulb light up the most brightly?

a)

Acetic acid (HC2H3O2)

b)

Sucrose (C12H22O11)

c)

Methanol (CH3OH)

d)

Sodium hydroxide (NaOH)

43.

Water is held together by _____________ which lead to its ______ surface tension and _______ boiling point.

a)

Dipole-dipole forces, high, high

b)

Hydrogen bonds, high, high

c)

LDF forces, high, low

d)

Hydrogen bonds, low, high

44.

During the process of ______________, a __________ dissolves in a _____________.

a)

Solute, solvation, solvent

b)

Solute, solvent, solvation

c)

Solvent, solvation, solute

d)

Solvation, solute, solvent

45.

How does the solubility of a gas in a liquid change as the temperature is increased?

a)

remains the same

b)

decreases

c)

Increases

46.

Which of the following operations usually make a substance dissolve faster in a solvent?

a)

Agitation

b)

Raising the temperature

c)

crushing the substance into a powder

d)

all of the above

47.

How does this factor affect the solubility of a SOLID?


Increasing temperature

a)

More soluble

b)

Less soluble

c)

No effect

48.
How many grams of K2Cr2O7, are soluble in 100 g of water at 95 ºC?
a)
83 grams
b)
75 grams
c)
40 grams
d)
12 grams
49.
Which solute does not increase in solubility as temperature rises?
a)
NH3
b)
NaNO3
c)
KNO3
d)
NaCl
50.
What is the minimum temperature needed to dissolve at least 10 g of KClO3?
a)
25 ⁰C
b)
10 ⁰C
c)
5 ⁰C
d)
100 ⁰C
51.

The amount of solute that can be dissolved in a specific volume of solvent at a specific temperature.

a)

Solution

b)

Solubility

c)

Solvent

52.

Determine the type of solution present when 110 grams of Potassium Nitrate are dissolved at 60°C.

a)

Saturated

b)

Supersaturated

c)

Unsaturated

53.

Determine the type of solution present when 60 grams of Ammonia are dissolved at 10°C

a)

Supersaturated

b)

Saturated

c)

Unsaturated

54.

Which of these pH values represent an acid?

a)

4

b)

8

c)

10

d)

12

55.

Which of the following are properties of acids?

a)

They conduct electricity when dissolved in water

b)

They taste sour

c)

They react with metals to produce hydrogen gas

d)

All of the answer choices are correct

56.

If the substance is neutral, what would the pH be?11

a)

3

b)

5

c)

7

d)

9

e)

11

57.

A substance is found to have the following characteristics:


Very bitter taste

Feels slippery to the touch

Produces OH- ions when dissolved in water


In what category would the substance be classified?

a)

acid

b)

base

c)

enzyme

d)

fatty acid

58.
Which of the following statements is correct?
a)
Blue litmus paper turns red when placed in a base.
b)
Red litmus paper turns blue when placed in a base.
c)
Blue litmus paper stays blue when placed in an acid.
d)
Red litmus paper stays red when placed in a base.
59.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
60.

Phenolophalein turns from clear to pink when the pH turns

a)

acidic

b)

basic

c)

saline

d)

ionic

61.

What completely ionizes in solution?

a)

Weak acids

b)

Strong acids

c)

Strong Salts

d)

Neutral salts

62.
Holly has an unknown substance in a beaker. She wants to determine the relative pH of the unknown substance. She places a piece of blue litmus paper into the substance, and the litmus paper stays blue.
The substance in the beaker
a)
is a base.
b)
has a neutral pH.
c)
is an acid.
d)
does not have a pH.
63.

For a solution, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

64.
If a solution is basic which ion will be more present?
a)
H+
b)
K+
c)
OH-
d)
H-
65.

Which of the following is a strong acid?

a)

oxalic acid

b)

nitric acid

c)

carbonic acid

d)

acetic acid

66.

What is the pH of a solution that has a [H+] of 2.5 x 10-5?

a)

4.6

b)

5.0

c)

2.5

d)

7.0

67.

What is the [OH-] if the pH is 4.9?

a)

7.94 x 10-10 M

b)

1.0 x 10-4 M

c)

7.94 x 10-14 M

d)

4.9 x 10-10 M

68.

An aqueous solution of HNO3 has a pH of 2.34. What is the concentration of the acid?

a)

218.78 M

b)

4.57 x 10-3 M

c)

1 M

d)

6.04 x 10-3 M

69.

Human blood has a pH of between 7.38 and 7.42. This means that the blood is ________.

a)

very acidic

b)

slightly acidic

c)

very basic

d)

slightly basic

70.

An increase in the amount of hydroxide ions in a solution ____ the pH.

a)

raises

b)

lowers

c)

does not effect

d)

doubles

71.
Ca(OH)2 is an example of a(n)
a)
Acid
b)
Base
c)
Neutral
72.

According the Bronsted Lowry acid-base theory a base is an

a)

H+ acceptor

b)

H+ donator

c)

OH- acceptor

d)

OH- donator

73.
sulfuric acid
a)
HSO3
b)
H2SO3
c)
H2SO4
d)
H3SO4
74.

Name the following compound.

H NO3

a)

Nitric acid

b)

Hydrogen nitride acid

c)

Hydronitric acid

75.
HBr
a)
hydrogen bromine acid
b)
hydrobromide acid
c)
hydrobromic acid
76.

Name the following compound.

KOH

a)

Potassium monohydroxide

b)

Potassium hydroxide

c)

Monopotassium monohydroxide

77.

What is the formula for hydrochloric acid?

a)

HCl

b)

HClO

c)

H3ClO3

d)

HClO3

78.
Strong acids and bases...
a)
do not break apart into ions (non-electrolyte)
b)
partially break apart into ions (weak electrolyte)
c)
completely break apart into ions (non-electrolyte)
d)
completely break apart into ions (strong electrolyte)
79.

Which of the following compounds is a base?

a)

CH3COOH

b)

HCl

c)

NaOH

d)

HNO3

80.

What color does red litmus paper turn in a basic solution?

a)

Red

b)

Blue

c)

Green

d)

Yellow

81.

Which of the following substances will turn red litmus paper blue?

a)

Orange juice

b)

Vinegar

c)

Ammonia solution

d)

Lemon juice

82.

What is the pH of a solution with a hydrogen ion concentration of 1.0 x 10-7 M?

a)

14

b)

10

c)

7

d)

1

83.

Which of the following is a property of acids?

a)

They react with metals to produce hydrogen gas

b)

They taste bitter

c)

They turn blue litmus paper blue

d)

They feel slippery

84.

What is this piece of apparatus called

a)

Pipette

b)

Burette

c)

Janette

d)

Cuvette

85.

What allows us to know when the end point has been reached?

a)

Bubbles

b)

Feels warm

c)

indicator changing color

d)

Turns to a solid

86.

How much liquid is in this buret? (Burets are read from the top down)

a)

8.61 mL

b)

7.34 mL

c)

7.4 mL

d)

7.43 mL

87.
what is the reading on this burette?
a)
4.40mL
b)
3.50mL
c)
3.60mL
d)
4.50mL
88.

How is the H+ concentration related to the OH- concentration in a solution?

a)
The H+ concentration is always greater than the OH- concentration
b)
The H+ concentration is always less than the OH- concentration
c)

In a solution, the product of the H+ concentration and the OH- concentration is always equal to 1 x 10-14.

d)
The H+ concentration is always equal to the OH- concentration
89.

Which of the solutions in are acids? Which are bases?

a)

Solution A and D are acids, solution C and B are bases

b)

Only Solution B is an acid, and Solution A is a base

c)

Solution A and B are acids, solution C and D are bases

d)

Both Solution A and Solution B are bases

90.

How does H⁺ concentration relate to pH?

a)
The higher the pH, the lower the H⁺ concentration.
b)
There is no relationship between pH and H⁺ concentration.
c)
H⁺ concentration is directly proportional to pH.
d)
The lower the pH, the higher the H⁺ concentration.
91.

If the hydroxide ion (OH-) concentration is greater than the hydronium ion (H3O+) concentration, then what is the solution?

a)

acidic

b)

basic

c)

neutral

d)

salty

92.

Is this a strong acid or a weak acid?

a)

strong

b)

weak

93.

Which of the following is a weak base?

a)

NH3

b)

KOH

c)

NaOH

d)

Ba(OH)2

94.

What letter represents the energy of the products?

a)

A

b)

B

c)

C

d)

D

95.

If a catalyst for this reaction was present, which arrows would be affected?

a)

Arrow A

b)

Arrow B

c)

Arrow C

d)

Arrow D

e)

Arrows B and C

96.

What letter represents the activation energy for the forward reaction?

a)

A

b)

B

c)

C

d)

D

e)

E

97.

Is the forward reaction endothermic or exothermic?

a)

endothermic

b)

exothermic

98.

What is the ΔH of the forward reaction?

a)

40 kJ

b)

20 kJ

c)

80 kJ

d)

-60 kJ

e)

-20 kJ

99.

What is the energy of the activated complex?

a)

75 kJ

b)

225 kJ

c)

300 kJ

d)

225 kJ

100.

Which letter represents the activation energy for the reverse reaction?

a)

A

b)

B

c)

C

d)

D

e)

E

101.

Which of the following increase the reaction rate?

a)

less surface area

b)

lower temperature

c)

increasing pressure

d)

increased concentration

102.

A catalyst works by

a)

changing the order of the reaction

b)

increasing the temperature

c)

lowering the amount of energy needed

d)

making the activated complex

103.

If the concentration of a reactant is increased, the reaction rate will ___________.

a)

increase

b)

decrease

c)

stay the same

104.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
105.
What two factors govern whether a collision between reacting particles will be effective?
a)
orientation and potential energy 
b)
kinetic energy and temperature 
c)
kinetic energy and orientation 
d)
potential energy and kinetic energy 
106.

If the temperature is reduced, a reaction rate will ______

a)

increase

b)

decrease

c)

stay the same

107.

The ____________ states that atoms, ions, or molecules must collide in order to react.

a)

transition state

b)

activation energy

c)

rate law

d)

collision theory

108.
N2O4(g) ↔ 2 NO2(g)
What is the concentration equilibrium constant expression?
a)
Kc = [NO2]2/[N2O4]
b)
Kc = [N2O4]/[NO2]2
c)
Kc = [N2O4]2/[NO2]
d)
Kc = [NO2]/[N2O4]2
109.
If the equilibrium constant is much greater than one (K >> 1) then
a)
Equilibrium is not established.
b)
Equilibrium lies to the right (products are favored)
c)
Equilibrium lies to the left (reactants are favored)
d)
Neither products or reactants are favored.
110.
If the equilibrium constant is much less than one (K << 1) then
a)
Equilibrium is not established.
b)
Equilibrium lies to the right (products are favored)
c)
Equilibrium lies to the left (reactants are favored)
d)
Neither products or reactants are favored.
111.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
112.

Which is the correct equilibrium constant expression for the following reaction?

Fe2O3(s) + H2(g) —> Fe(s) + H2O(g)

a)

K = [H2O]3 / [H2]3

b)

K = [Fe2O3] [H2]3 / [Fe]2[H2O]3

c)

K = [Fe]2[H2O]3 / [Fe2O3] [H2]3

d)

K= [Fe] [H2O] / [Fe2O3] [H2]

e)

K = [H2] / [H2O]

113.

Around what time does the reaction reach equilibrium?

a)

25 min

b)

70 min

c)

45 min

d)

80 min

114.

What states of matter are omitted when writing Keq expressions?

a)

solids and liquids

b)

aqueous solutions and gas

c)

solids, liquids, aqueous solutions and gases

d)

aqueous solutions & liquids

115.

Which changes occur when O2(g) is added to this

system?

a)

The equilibrium shifts to the right and the

concentration of PCl3(g) increases.

b)

The equilibrium shifts to the right and the

concentration of PCl3(g) decreases.

c)

The equilibrium shifts to the left and the

concentration of PCl3(g) increases.

d)

The equilibrium shifts to the left and the

concentration of PCl3(g) decreases.

116.

Which change will cause the equilibrium to shift to

the right?

a)

adding a catalyst

b)

adding more PCl3(g)

c)

increasing the pressure

d)

increasing the temperature

117.

The formation of ammonia is favored by

a)

an increase in pressure

b)

a decrease in pressure

c)

removal of N2(g)

d)

removal of H2(g)

118.

Increasing the temperature of the system causes the

concentration of

a)

HI to increase

b)

H2 to increase

c)

HI to remain constant

d)

H2 to remain constant

119.

Which change will not shift the point of

equilibrium?

a)

changing the pressure

b)

changing the temperature

c)

changing the concentration of H2(g)

d)

changing the concentration of HF(g)

120.
Le Chaltelier's Principle states that if a chemical system at equilibrium is stressed,
a)
the system will adjust to increase the stress
b)
the system will adjust to reduce the stress
c)
the system will not adjust
121.
A +  B <--> C + D   ΔH= 151kJ
Rewrite the above equation with energy as a reactant or product:
a)
A +  B <--> C + D + energy
b)
A +  B + energy <--> C + D 
122.
For the reaction...
heat  +  N2(g)  +  O2(g)  <−>  2NO(g)
If the heat is removed to the chemical system, the equilibrium will _______.
a)
shift to the left
b)
shift to the right
c)
not shift
123.

Which of the following statements is FALSE for a system that has established equilibrium?

a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
124.

A melting ice cube is an example of

a)

exothermic

b)

endothermic

c)

none

d)

both

125.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
126.

If 20 g of water undergoes a temperature change from 25° C to 30° C, how much heat energy (Q) moves from the water to the surroundings?

a)

418 J

b)

209 J

c)

83 J

d)

4.18 J

127.

Which substance would heat up the fastest?

a)

aluminum

b)

water

c)

copper

d)

gold

128.

What is chemical potential energy?

a)

Energy from chemicals

b)

Energy to make chemicals

c)

Energy stored in chemical bonds

d)

Energy from the sky

129.
For the reaction...
SO2(g) + O2(g) <−>  SO3(g)
If the concentration of SO2(g)  is increased, the equilibrium of the reaction will ___________.
a)
shift to the left
b)
shift to the right
c)
not shift
130.
An exothermic reaction is allowed to reach equilibrium. If heat energy is then removed, the equilibrium will shift
a)
toward the middle
b)
toward the reactant side
c)
toward the product side
131.
When writing an endothermic reaction, heat energy is stated as
a)
product
b)
catalyst
c)
reactant
132.

Which change will cause the equilibrium to shift to

the right?

a)

adding a catalyst

b)

adding more PCl3(g)

c)

increasing the pressure

d)

increasing the temperature

133.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is decreased,  which substance will increase in concentration?
a)
N2
b)
H2
c)
N2 and H2
d)
NH3
134.
The following factors affect the position of equilibrium EXCEPT
a)

Concentration

b)

Pressure

c)

Temperature

d)

Catalysts

135.

The diagram shows what happens when zinc reacts with hydrochloric acid. Which of these best describes the energy transformation that occurs during this reaction?

a)

Thermal energy - kinetic energy

b)

Kinetic energy -potential energy

c)

Chemical energy - thermal energy

d)

Potential energy - chemical energy

136.

The potential energy diagram of a reaction is shown. Which statement below is correct relating to this reaction?

a)

#1 represents the enthalpy change for this exothermic reaction.

b)

#2 represents the enthalpy change for this endothermic reaction.

c)

#3 represents the enthalpy change for this endothermic reaction.

d)

#4 represents the enthalpy change for this exothermic reaction.

137.

During an exothermic reaction, heat content in the surroundings increases because

a)

heat energy is destroyed during reactions

b)

the reaction absorbs heat energy

c)

the energy contained in the reactants is lower then the products

d)

the energy contained in the products is lower than the reactants

138.

The diagram represents two solids and the temperature of each. What occurs when the two solids are placed in contact with each other?

a)

Heat energy flows from solid A to solid B. Solid A decreases in temperature

b)

Heat energy flows from solid A to solid B. Solid A increases in temperature

c)

Heat energy flows from solid B to solid A. Solid B decreases in temperature.

d)

Heat energy flows from solid B to solid A. Solid B increases in temperature.

139.

The amount of heat energy required to change the temperature of 12 g of gold from 45°C to 15°C is -47 J. What is the specific heat capacity of gold?

a)

0.13 J/(g°C)

b)

17,000 J/(g°C)

c)

1600 J/(g°C)

d)

0.065 J/(g°C)

140.

The graph represents the uniform heating of a substance, starting with the substance as a solid below its melting point. Which line segment listed below represents an increase in potential energy and no change in average kinetic energy?

a)

Line segment AB

b)

Line segment BC

c)

Line segment CD

d)

Line segment EF

141.

What is energy?

a)

Something you get from sleeping

b)

The ability to do work or supply heat

c)

A stadium in Houston

d)

A magical power

142.

What is thermochemistry?

a)

study of heat changes that occur during a chemical reaction & physical changes of state

b)

the study of heat and chemistry

c)

the study of heat

d)

the study of chemistry

143.

How does heat move?

a)

From cold to hot

b)

From hot to cold

144.

What is chemical potential energy?

a)

Energy from chemicals

b)

Energy to make chemicals

c)

Energy stored in chemical bonds

d)

Energy from the sky

145.

When a hot object and a cold object come together, heat will move from the warmer one to the colder one until they are the same temperature. What is this called?

a)

Equal

b)

Equilibrium

c)

Equality

146.

Match the following

a)

Q

1.

heat

b)

M

2.

mass

c)

C

3.

specific heat

d)

ΔT\Delta T

4.

change in temperature

147.

Match the following

a)

Jg ∘C or calg ∘C\frac{J}{g\ \circ C}\ or\ \frac{cal}{g\ \circ C}

1.

c

b)

g or kg

2.

m

c)

ΔT\Delta T

3.

C or K

d)

c

4.

J or cal, kJ or Kcal

148.

How much heat, in calories, is needed to raise the temperature of 125.0 g of lead (c lead= 0.130 J/g°C) from 17.5°C to 41.1°C?

a)

91.7 cal

b)

9.17 cal

c)

917 cal

d)

917.0 cal

149.

A sample of H2O with a mass of 60 grams boils until it has completely changed to steam. How much heat was absorbed?

Hfus = 334 J/g

Hvap = 2260 J/g

a)

7525 J

b)

135,600 J

c)

1112.1 J

d)

20,040 J

150.
In which region(s) does temperature remain constant?
a)
Region 1, 3, & 5
b)
Region 2 & 4
c)
Region 1 only
d)
Region 1 & 2
151.
In which region(s) does temperature increase?
a)
Region 1, 3, & 5
b)
Region 2 & 4
c)
Region 1 only
d)
Region 1 & 2
152.

Convert 42 kJ into joules

a)

0.042 J

b)

175.73 J

c)

42000 J

d)

10.04 J

153.

Consider the reaction: 2 H2O + energy --> 2H2 + O2

a)

exothermic because releasing energy

b)

exothermic because absorbing energy

c)

endothermic because absorbing energy

d)

endothermic because releasing energy

154.

In which region(s) does temperature increase?

a)

Region C only

b)

Regions B and D

c)

Regions A, C, and E

d)

Regions A and B

155.

During which phase change is energy (heat) added?

a)

Melting

b)

Freezing

c)

Condensation

d)

Deposition

156.

During which phase change is energy (heat) removed

a)

Melting

b)

Vaporization

c)

Sublimation

d)

Freezing

157.

Is graph B showing an endothermic reaction or an exothermic reaction?

a)

Endothermic

b)

Exothermic

c)

Both

d)

No way to tell

158.
Enthalpy is energy absorbed or relased during a chemical reaction as
a)
light.
b)
heat.
c)
sound.
d)
pressure.
159.
How would this reaction be classified?
2Na + Cl2 → 2NaCl + 25kJ energy
a)
Exothermic
b)
Endothermic
c)
Isothermic
d)
None of the above
160.

What is Standard Temperature and Pressure (STP)?

a)

1 Degrees Celsius and 0 atm

b)

0 Degrees Celsius and 1 atm

c)

0 Kevin and 10 atm

d)

273 Celsius and 273 atm

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