Free Printable 11 Review Thermochemistry

1.

The specific heat of aluminum is 0.21 J/g°C. How much heat(Q) is released when a 10 g piece of aluminum foil is taken out of the oven and cools from 100° to 50°?

a)

105 J

b)

10.5 J

c)

1.05 J

d)

0.105 J

2.

20 g of water. specific heat of water is 4.18 J/g°C. temperature changes from 25° C to 20° C, how much heat energy (q) moves from the water to the surroundings?

a)

400 J

b)

210 J

c)

80 J

d)

4.18 J

3.

What does temperature measure?

a)

Heat

b)

ºC

c)

Kinetic Energy

d)

Thermal Energy

4.

In an endothermic reaction the system is releasing energy.

a)

True

b)

False

5.

For an endothermic reaction, the heat is on the ____ side.

a)

reactant

b)

product

c)

either side

6.

For an exothermic reaction, the heat is on the ____ side

a)

reactant

b)

product

c)

either side

7.

What type of reaction is shown in the picture?

a)

endothermic

b)

exothermic

8.

In an exothermic process, the surroundings are are gaining energy.

a)

True

b)

False

9.

If two objects have different temperatures, heat will flow from the warmer object to the cooler one UNTIL ____________

a)

one reaches a temperature of zero

b)

they both have an equal temperature

c)

one runs out of energy

10.

What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water. The water weighs 75. g and had an initial temperature of 20.00 °C? (Specific heat of water is 4.18 J/g°C) (show your work)

a)

0.111 J/g°C

b)

1.29 J/g°C

c)

0.129 J/g°C

d)

22225.85 J

11.

Calculate the amount of heat liberated from 366g of mercury when it cools from 77.0^oC to 12.0^oC. Specific heat of Hg = 0.140kJ/g*^oC

(a)

12.

A 12.1g piece of aluminum at 81.7^oC is placed in a calorimeter containing water at 23.4^oC. If the final temperature of the system is 24.9^oC, what is the mass of the water? specific heat of Al = 0.900 J/g*^oC; specific heat of water = 4.184 J/g*^oC

(a)

13.

Calculate the standard enthalpy change for the reaction :

2Al_(s)+Fe₂O_3(s) --> 2Fe_(s) + Al₂O_3(s)

given that:

2Al_(s)+3/2O_2(g) --> Al₂O_3(s) ΔH^o_rxn=-1669.8kJ/mol

2Fe_(s)+3/2O_2(g) --> Fe₂O_3(s) ΔH^o_rxn=-822.2kJ/mol

(a)

14.

Calculate the enthalpy change for the reaction:

2C_(graphite)+3H_2(g)--> C₂H_6(g)

given that:

C_(graphite)+O_2(g) --> CO_2(g) ΔH^o_rxn= -393.5kJ/mol

H_2(g)+1/2O_2(g) --> H₂O_(l) ΔH^o_rxn= -285.8kJ/mol

2C₂H_6(g)+7O_2(g) --> 4CO_2(g)+6H₂O_(l) ΔH^o_rxn= -3119.6kJ/mol

(a)

15.

Given the following data:

H_2(g) --> 2H_(g) ΔH^o_rxn= 436.4kJ/mol

Br_2(g) --> 2Br_(g) ΔH^o_rxn= 192.5kJ/mol

H_2(g)+ Br_2(g) --> 2HBr_(g) ΔH^o_rxn= -72.4kJ/mol

Calculate ΔH^o_{rxn for}

H_(g) + Br_(g) --> HBr_(g)

(a)

16.

Heat flows from _______ to ______ objects

a)

cooler to warmer

b)

warmer to warmer

c)

warmer to cooler

d)

cooler to cooler

17.

The transfer of thermal energy between objects of different temperatures is called...

a)

temperature

b)

heat

c)

internal energy

d)

none of these

18.

When thermal energy is added to a substance, the substance's particles move:

a)

More rapidly at an increased distance from each other.

b)

More rapidly with less distance between each other.

c)

More slowly with a greater distance between each other.

d)

More slowly with a reduced distance between each other.

19.

Heat transfer by conduction occurs when...

a)

particles bump into each other

b)

large numbers of atoms move from place to place

c)

atoms give off heat in the form of electromagnetic waves

d)

electromagnetic waves travel from place to place through a vacuum

20.

Heat transfer by convection occurs when...

a)

electrons bump into other electrons

b)

large numbers of atoms move from place to place

c)

atoms give off heat in the form of electromagnetic waves

d)

electromagnetic waves travel from place to place through a vacuum

21.

Thermal energy always moves:

a)

From a high temperature object to a lower temperature object.

b)

From a lower temperature object to a higher temperature object.

c)

From an object with lower kinetic energy to an object with higher kinetic energy.

d)

From an object of higher mass to an object of lower mass.

22.

A chemical reaction that absorbs heat from the surroundings is said to be __________ and has a __________ ΔH at constant pressure.

a)

endothermic; positive

b)

endothermic; negative

c)

exothermic; negative

d)

exothermic; positive

23.

Refer the the following question:
2N₂ + 3H₂ --> 2NH₃ + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?

a)

92 kJ

b)

0.143 kJ

c)

23 kJ

d)

15 kJ

24.

Do the reactants in an exothermic reaction have a higher or lower energy than the products?

a)

Higher

b)

Lower

25.

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

26.

Calculate $\Delta T$ when a substance goes from 10*C to 75*C

a)

-65*C

b)

75*C

c)

10*C

d)

65*C

27.

Calculate A 50g sample is heated with 500 joules of energy and has a 10*C temperature change. Calculate it’s specific heat.

a)

1 j/g*C

b)

250000 j/g*C

c)

500 j/g*C

d)

10 j/g*C

28.

4180 j of heat energy are added to change the temperature of water by 10*C. How many grams of water are being heated? c_water=4.18 j/g*C

a)

4.18 j/g*C

b)

10000g

c)

174724g

d)

100g

29.

What heat energy is required to raise the temperature of a 1g sample of mercury (c_Hg=.16 j/g*C) by 100*C?

a)

16j

b)

.0016j

c)

16000j

d)

625 j

30.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

31.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

32.

What does q stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

33.

What does c stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

34.

What does $\Delta T$ stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

35.

What does m stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

36.

When two samples of similar mass are subjected to the same heat energy, the sample with the SMALLER specific heat will have a _________ temperature change.

a)

SMALLER

b)

LARGER

c)

EQUAL

37.

___________________ is the capacity to do work or supply heat.

a)

energy

b)

heat changes

c)

specific heat

d)

thermochemistry

38.

Ice cream melting is an example of an __________ process.

a)

endothermic

b)

exothermic

39.

Sweating is an __________________ process because heat is released.

a)

endothermic

b)

exothermic

40.

what does c stand for?

a)

heat capacity

b)

specific heat

c)

mass

d)

temperature

41.

Mass must always be in ________ for energy calculations.

a)

kilograms

b)

grams

c)

joules

d)

calories

42.

What is the specific heat of water?

a)

4.184 J/gC

b)

1.00 cal/gC

c)

All of the above

d)

none of the above

43.

When heat flows from system to the surroundings that is an example of an ________________ process.

a)

exothermic

b)

endothermic

44.

What device is used to measure the amount of heat involved in a chemical reaction or physical process?

a)

barometer

b)

calorimeter

c)

thermometer

45.

Kinetic energy is energy gained _______________

a)

while at rest

b)

during motion

46.

What is calorimetry?

a)

process of measuring kinetic and potential energy

b)

process of measuring heat flow of chemical reactions

c)

process of measuring pressure and temperature of a substance

47.

Heat flows from _______ to _________.

a)

warm to cool

b)

cool to warm

48.

What area of study in chemistry is concerned with the heat transfers that occur during chemical reactions?

a)

stoichiometry

b)

thermochemistry

c)

inorganic chemistry

d)

physical chemistry

49.

The specific heat of a substance varies with the mass of a sample. True or False?

a)

True

b)

False

50.

1 food calorie = _______ chemistry calories

a)

1000

b)

1

c)

500

d)

4.184

51.

Samples of two different substances having the same mass always have the same heat capacity. True or False?

a)

True

b)

False

52.

What is the SI unit of heat and energy?

a)

calorie

b)

celsius

c)

joule

53.

The law of conservation of energy states that

a)

in any chemical or physical change, energy cannot be created or destroyed, only changed in form.

b)

heat changes occur during chemical and physical changes.

c)

energy is the capacity to do work or to supply heat

d)

there are two types of energy, kinetic and potential

54.

Any substance that does not conduct electricity when in solution is called a(n) ―

a)

nonelectrolyte

b)

electrolyte

c)

conductor

d)

semiconductor

55.

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

56.

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.

57.

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

58.

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.

59.

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)

60.

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

61.

A cast iron skillet is used to fry bacon. For optimal frying, the pan must be heated to about 178 ^oC from a room temperature of 22.0 ^oC. It is known that 1.58 x 10⁵ J of heat energy are absorbed by the pan to reach the desired temperature and the specific heat of iron is 0.450 J/g ^oC. What must the mass of the skillet be?

a)

12.7 kg

b)

2.25 kg

c)

110 kg

d)

1.97 kg

62.

Experimental Set-up for Calories in a Chocolate Chip Cookie Students designed an experiment to determine the amount of calories in a chocolate chip cookie. A ring stand was used with a clean aluminum soda can hung from the ring that was partially filled with a known mass of water. A thermometer was placed inside the can so that it measured the temperature of the water but did not touch any part of the metal can. Once set-up was complete, an initial water temperature was taken. The cookie was then lit on fire and allowed to completely burn. A final temperature of the water was measured.

Refer to the experimental set-up for calories in a chocolate chip cookie. How does this experiment allow students to measure the calories in a cookie?

a)

The difference in masses before and after the cookie is burned is calculated, then converted into heat energy.

b)

Heat energy from the burning cookie is transferred to the water. The change in water temperature is used to calculate the heat energy from the cookie.

c)

Data from the amount of time for the cookie to burn and the temperature change are used to calculate the heat energy from the cookie.

d)

The cookie is burned until the water reaches a boiling temperature, then masses are compared to calculate the heat energy from the cookie.

63.

When methane, CH4, and oxygen, O2, are mixed in a stove and ignited, a lovely blue flame results. The balanced equation is: CH₄(g) + 2O₂(g) 2H₂O(g) + CO₂(g) What can be said about the energy involved in this chemical reaction?

I. The average kinetic energy of the products is greater than that of the reactants.

II. The chemical energy stored in the reactants is greater than the chemical energy stored in the products.

III. Chemical energy in the reactants is changed into heat energy and light energy.

a)

I only

b)

II only

c)

III only

d)

I, II, and III

64.

Is the combustion of gasoline endothermic or exothermic?

a)

Endothermic

b)

Exothermic

65.

What is the symbol for heat?

a)

q

b)

H

c)

J

d)

∘C

66.

What are chemical reactions that absorb energy?

a)

endothermic

b)

fast

c)

slow

d)

exothermic

67.

What is the study of heat changes that accompany chemical reactions and phase changes?

a)

energy

b)

chemistry

c)

work

d)

thermochemistry

68.

What is the formula for calculating heat?

a)

q = mcΔT

b)

H = ΔH x moles

c)

H = ΔH x grams

d)

products - reactants

69.

Convert 42 kJ into joules

a)

0.042 J

b)

175.73 J

c)

42000 J

d)

10.04 J

70.

What are the two main types of energy?

a)

endothermic and exothermic

b)

spontaneous and nonspontaneous

c)

potential and kinetic

d)

entropy and enthalpy

71.

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

72.

The heat required to raise the temperature of a SUBSTANCE by 1∘C

a)

calorie

b)

joule

c)

specific heat

d)

4.184 J

73.

The heat required to raise the temperature of WATER 1∘C

a)

calorie

b)

joule

c)

specific heat

d)

energy

74.

Heat flows from _______ to ______ objects

a)

cooler to warmer

b)

warmer to warmer

c)

warmer to cooler

d)

cooler to cooler

75.

A 500g piece of aluminum has a temperature of 7°C. What is the heat energy produced? Specific heat of Aluminum is 0.900 J/gºC.

a)

3000 J

b)

3000 g

c)

3150 J

d)

3150 g

76.

What does temperature measure?

a)

heat

b)

average kinetic energy

c)

space

d)

time

77.

How much heat does an aluminum block absorb if 10.00 grams is heated from 25.0^oC to 50.0^oC? *Specific heat of aluminum is 0.900 J/g^oC

a)

450 J

b)

-450 J

c)

225 J

d)

-225 J

78.

Durning a phase change the temperature of a substance_________.

a)

always increases

b)

always decreases

c)

always stays the same

d)

varies

79.

A 24.0 gram sample of copper was heated from 25.0^oC to 500.0^oC, 4378 J of heat were absorbed, what is the specific heat of copper?

a)

0.384 J/g°C

b)

49909200 J/g°C

c)

2.60 J/g°C

d)

8.77 J/g°C

80.

The specific heat of platinum is 0.133 J/g°C. How much heat is released when a 10 g piece of platinum cools from 100°C to 50°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

81.

The temperature of an unknown piece of metal with a mass of 30.00 g changes from 25.0°C to 35.0°C when the metal absorbs 350.0 J of energy. What is the specific heat of the metal?

a)

1.17 J/g°C

b)

-1.17 J/g°C

c)

0.857 J/g°C

d)

-0.857 J/g°C

82.

Releasing heat into the surroundings occurs during an ___________________ reaction.

a)

Exothermic

b)

Endothermic

c)

Kinetic Energy

d)

Thermal Energy

83.

A sample of iron receives 50 J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?

a)

25g

b)

30g

c)

20g

d)

50g

84.

If 238 J of heat is absorbed by a sample of metal with a mass of 40.7 g, and it raises the temperature from 20.0°C to 32.4°C, what is the specific heat capacity of the metal?

a)

2.34 J/g°C

b)

0.472 J/g°C

c)

6.13 J/g°C

d)

0.163 J/g°C

85.

________ is a measure of the average kinetic energy of the random motion of molecules of a substance or material.

a)

Temperature

b)

Heat

c)

Potential energy

d)

Specific heat

86.

A(n) __________ reaction is one in which the energy of the products is higher than the energy of the reactants.

a)

exothermic

b)

endothermic

c)

combustion

d)

acid-base

87.

________ is a type of energy that flows from hotter to cooler regions.

a)

Kinetic energy

b)

Potential energy

c)

Chemical energy

d)

Heat

88.

A calorimeter is a device whose primary purpose is to measure ________ .

a)

temperature

b)

heat transfer

c)

kinetic energy

d)

potential energy

89.

__________ is the amount of energy required to raise the temperature of 1 gram of a substance by 1 °C.

a)

Specific heat capacity

b)

Heat

c)

Enthalpy

d)

Lattice energy

90.

50 grams of tin is heated and placed in 50 grams of cool water. The final temperature of the two will be ____________.

a)

half way between original temperatures of tin and water

b)

closer to the original temperature of the tin

c)

closer to the original temperature of the water

d)

cannot be determined without knowing the original temperatures

91.

If 50 grams of each substance absorb the same amount of heat, which will undergo the biggest change in temperature?

a)

silicone

b)

cement

c)

cotton

d)

styrofoam

92.

What is a calorie?

a)

the specific heat of water

b)

the fat content in food

c)

1000 Calories

d)

a device used to measure heat transfer

93.

What is the mass of 5 mL of water?

a)

.05 grams

b)

5 grams

c)

18.02 g/mol

d)

need more information

94.

The reaction below is ________.

$AB+CD\ \ \rightarrow\ \ AD+CB\ \ \ \ \ \ \ \ ΔΗ=2100\ kJ$

a)

endothermic

b)

exothermic

c)

neutral

d)

cannot be determined

95.

Solutions A and B are mixed together and a reaction occurs resulting in the temperature change shown. How do you calculate the enthalpy of reaction?

a)

$\Delta H=\left(900\right)\left(4.184\right)\left(5\right)$

b)

$\Delta H=\left(0.9\right)\left(1.0\right)\left(5\right)$

c)

$\Delta H=\left(18.02\right)\left(4.184\right)\left(5\right)$

d)

$\Delta H=\left(900\right)\left(4.184\right)\left(27\right)$

96.

A metal ball is heated and placed in cool water. As the ball cools, which of the following must be true?

a)

The extent of temperature change of the ball and the water are equal.

b)

The amount of heat loss of the ball equals the amount of heat absorption by the water.

c)

q_ball = q_water

d)

The ball is the system and the water is the surrounding.

97.

Let q represent the energy absorbed by 1 L of water as it goes from ice at -1 °C to water at 9 °C. The equation below shows the proper way to calculate q.

$q\ =\ 1000\cdot4.184\cdot10$

a)

True

b)

False

98.

The graph shows the temperature of a Substance X as it loses heat. The boiling point of Substance X is ________.

a)

120 °C

b)

100 °C

c)

0 °C

d)

160 °C

99.

The graph shows the temperature of a Substance X as it loses heat.

Substance X freezes at what temperature?

a)

0 °C

b)

70 °C

c)

120 °C

d)

20 °C

100.

To calculate the total energy loss depicted in the graph, you would need to use ____ mcΔT equations and ____ ΔH t-square conversions.

a)

1

2

b)

2

c)

3

d)

3

2

101.

A 1 gram metal filament is heated and then placed in a coffee cup calorimeter containing 100 mL of water. By the time it is done cooling, the temperature of the filament has dropped by 418.4 °C where the water has warmed by only 1 °C.

What is the specific heat capacity of the metal?

a)

0.1

b)

1.0

c)

10.0

d)

0.05

102.

Given the reactions and enthalpies below, the enthalpy of reaction for equation 1 is ________ according to Hess' Law.

$1.\ \ \ \ AB\ +G\ \ \rightarrow\ \ AG\ +\ B$

$2.\ \ \ \ AG+CB\ \ \rightarrow\ \ AB\ +C+G\ \ \ \ \ \ \ \ \Delta H\ =\ 300\ kJ$

$3.\ \ \ \ CB\ \ \rightarrow\ \ C+B\ \ \ \ \ \ \Delta H=100\ kJ$

a)

200

b)

-400

c)

400

d)

-200

103.

The heat of fusion (ΔH_fus) of iron is 11.7 kJ/mol. This means that...

a)

It takes 11.7 kilograms of iron to melt 1 kg of ice.

b)

If you were to turn 1 mole of iron from molten (liquid) to gas, it would take 11.7 kJ of energy.

c)

If you were to melt 1 mole of iron, it would take 11.7 kJ of energy.

d)

The temperature of 1 mole of iron will change by 11.7 °C as it goes from molten to solid form.

104.

The specific heat of ice is the amount of energy required to melt 1 mL (= 1 gram) of ice.

a)

True

b)

False

105.

Substance X is absorbing heat, therefore the temperature of Substance X is rising.

a)

Always

b)

Sometimes

c)

Never

106.

Exothermic reactions are reactions that

a)

release heat

b)

do not involve heat

c)

absorb heat

d)

take place instantaneously

107.

Which of the following is an endothermic process?

a)

solid to gas

b)

liquid to solid

c)

solid to liquid

d)

gas to liquid

108.

In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is the...

a)

free energy

b)

heat of reaction

c)

heat of fusion

d)

activation energy

109.

What kind of graph is this?

a)

endothermic

b)

exothermic

110.

Which of the letters (A-D) represents activation energy?

a)

A

b)

B

c)

C

d)

D

111.

Which of the letters (A-D) represents the potential energy of the reactants?

a)

A

b)

B

c)

C

d)

D

112.

Which of the letters (A-D) represents the potential energy of the products?

a)

A

b)

B

c)

C

d)

D

113.

What kind of reaction has a positive heat of reaction (ΔHr)?

a)

endothermic

b)

exothermic

114.

Compared to the potential energy of the products, the potential energy of the reactants above is?

a)

greater than

b)

less than

c)

the same

d)

impossible to determine

115.

What kind of reaction has a negative heat of reaction (ΔHr)?

a)

endothermic

b)

exothermic

116.

What kind of reaction is this?

a)

endothermic

b)

exothermic

117.

A process that absorbs heat is a(n) _______________ reaction?

a)

polythermic

b)

ergothermic

c)

exothermic

d)

endothermic

118.

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

a)

exothermic, releasing energy

b)

exothermic, absorbing energy

c)

endothermic, absorbing energy

d)

endothermic, releasing energy

119.

The minimum amount of energy needed to start a reaction is called the?

a)

surface energy

b)

activation energy

c)

concentration

d)

catalyst

120.

USE YOUR BURGER SHEET FOR CONVERSIONS!
If Karen eats a large curly fry and a bacon cheeseburger, how many calories from fat did she consume?

a)

279 calories

b)

495 calories

c)

55 calories

d)

216 calories

121.

USE YOUR BURGER SHEET FROM YESTERDAY!
Cady ate one small curly fries and two cheeseburgers, how many calories from carbohydrates?

a)

304 calories

b)

160 calories

c)

448 calories

d)

432 calories

122.

What kind of reaction moves from low PE to high PE?

a)

endothermic

b)

exothermic

123.

When activation energy is high, is the reaction slow or fast?

a)

slow

b)

fast

124.

What kind of reaction moves from high PE to low PE?

a)

endothermic

b)

exothermic

125.

What is the highest point in PE?

a)

activated complex

b)

activation energy

126.

Heat flows from _______ to ______ objects

a)

cooler to warmer

b)

warmer to warmer

c)

warmer to cooler

d)

cooler to cooler

127.

Energy can not be created or destroyed, it can only be transferred refers to the....

a)

law of conservation of energy

b)

law of conservation of mass

c)

life facts

d)

law of conservation of chemistry

128.

A slower particle has a lower energy than an identical, faster particle.

a)

True

b)

False

129.

When thermal energy is added to a substance, the substance's particles move:

a)

More rapidly at an increased diestance from each other.

b)

More rapidly with less distance between each other.

c)

More slowly with a greater distance between each other.

d)

More slowly with a reduced distance between each other.

130.

Heat travels from the sun to the earth by the process of...

a)

conduction

b)

convection

c)

radiation

d)

insulation

131.

Thermal energy always moves:

a)

From a high temperature object to a lower temperature object.

b)

From a lower temperature object to a higher temperature object.

c)

From an object with lower kinetic energy to an object with higher kinetic energy.

d)

From an object of higher mass to an object of lower mass.

132.

Which of the following is an example of an endothermic process or reaction?

a)

condensing

b)

freezing

c)

combustion

d)

melting

133.

Which of the following is an example of an exothermic process or reaction?

a)

melting

b)

boiling

c)

photosynthesis

d)

freezing

134.

energy in endothermic reactions are

a)

released

b)

ended

c)

absorbed

135.

.

How does an exothermic reaction compare with an endothermic reaction?

a)

Both changes absorb energy as reactants become products.

b)

Both changes release energy as reactants become products.

c)

An exothermic reaction absorbs energy, and an endothermic reaction releases energy.

d)

An endothermic reaction absorbs energy, and an exothermic reaction releases energy.

136.

Which of these processes is endothermic?

a)

freezing

b)

condensation

c)

deposition

d)

sublimation

137.

A chemical reaction in a beaker causes the beaker to feel cold to the touch. What type of reaction occurred?

a)

endothermic

b)

exothermic

138.

Which of these is the unit for specific heat?

a)

J

b)

J/g

c)

J/g^oC

d)

^oC

139.

Which of these phase changes requires energy to be released?

a)

boiling

b)

sublimation

c)

condensation

d)

melting

140.

Which of these would indicate that particles of a substance can be in three different phases on a phase diagram?

a)

critical point

b)

triple point

c)

phase section

d)

solid line

141.

Which of these statements is true?

a)

At the critical point on a phase diagram, a gas can no longer be changed to a liquid due to an increase in pressure.

b)

On a phase diagram you will find particles in three phases on a solid line segment.

c)

All substances have the same phase diagram.

d)

The normal boiling and melting points are found at 100 ^oC on a phase diagram.

142.

High temperatures and low pressures will usually result in which phase?

a)

solid

b)

liquid

c)

gas

d)

plasma

143.

Which type of energy is the energy stored in chemical bonds?

a)

kinetic energy

b)

potential energy

c)

chemical potential energy

d)

mechanical energy

144.

Which relationship is correct?

a)

1 calorie = 1 Calorie

b)

1 calorie = 1000 Calories

c)

1 Calorie = 4.184 Joules

d)

1 calorie = 4.184 Joules

145.

A piece of candy has 200 Calories per serving. How many calories of heat will be released when it is broken down?

a)

200 calories

b)

200,000 calories

c)

836,800 calories

d)

836.8 calories

146.

A snack item has 180 Calories per serving. How much heat energy (Joules) will be released when it is broken down?

a)

0.75312 Joules

b)

43,021 Joules

c)

43.02 Joules

d)

753,120 Joules

147.

What is the specific heat of water?

a)

2.02 J/g^oC

b)

2.05 J/g^oC

c)

4.184 J/g^oC

d)

41.84 J/g^oC

148.

Substance A heats more quickly than substance B. Which one has a higher specific heat?

a)

substance A

b)

substance B

c)

They have the same specific heat.

149.

A piece of aluminum with a mass of 20.0 grams is heated from 30 ^oC to 95 ^oC. If the specific heat of aluminum is 0.904 J/g^oC, how much heat is gained by the aluminum?

a)

1717.60 J

b)

1175.20 J

c)

963.68 J

d)

542.4 J

150.

A 300 gram sample of a metal is cooled from 120 ^oC to 60 ^oC, and releases 4230 J of energy. What is the specific heat of the metal?

a)

7.61 x 10⁷ J/g^oC

b)

4.26 J/g^oC

c)

0.47 J/g^oC

d)

0.235 J/g^oC

151.

A 95 gram volume of water has an initial temperature of 30 ^oC. A piece of metal with a mass of 120 grams and an initial temperature of 98 ^oC is placed in the water. The final temperature of the water and the metal is 35 ^oC. What is the specific heat of the metal?

a)

7560 J/g^oC

b)

3.80 J/g^oC

c)

0.263 J/g^oC

d)

1987.4 J/g^oC

152.

Which of these is a correctly balanced thermochemical equation for the combustion of C₂H₄?

a)

C₂H₄ (g) + 3O₂ (g) → 2CO₂ (g) + 2H₂O (g)

b)

2C₂H₄ (g) + 6O₂ (g) → 4CO₂ (g) + 4H₂O (g)

c)

C₂H₄ (g) + 3O₂ (g) → 2CO₂ (g) + 2H₂O (g) ΔH_comb= -1411 kJ/mol

d)

2C₂H₄ (g) + 6O₂ (g) → 4CO₂ (g) + 4H₂O (g) ΔH_comb= -1411 kJ/mol

153.

4Fe(s) + 3O₂(g) → 2Fe₂O₃(s) + 1625 kJ

Is this reaction endothermic or exothermic?

a)

endothermic

b)

exothermic

154.

Is the reaction represented in this graph endothermic or exothermic?

a)

endothermic

b)

exothermic

155.

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

H_fus= 334 J/g

H_vap = 2260 J/g

a)

7525 J

b)

135,600 J

c)

1112.1 J

d)

20,040 J

156.

If the temperature of a sample is decreased, the particles

a)

slow down

b)

have a lower kinetic energy

c)

speed up

d)

slow down and have a lower kinetic energy

157.

Which process releases the most heat when cooling down steam?

a)

freezing

b)

cooling it form 100 to 0 degrees

c)

condensing

158.

A piece of copper weighing 50 grams compared to a copper piece weighing 5 grams has

a)

has a higher specific heat

b)

has the same specific heat

c)

has a lower specific heat

159.

The heat of reaction is also called

a)

reactant energy

b)

enthalpy

c)

activation energy

d)

q, heat

160.

In an endothermic reaction, the energy stored in the bonds of the reactants is

a)

lower than the energy of the product bonds

b)

greater than the energy of the product bonds

c)

equal to the energy of the product bonds

d)

higher than the energy released

161.

What happens when a heated piece of metal is submerged in cool water?

a)

The temperature of the water will decrease

b)

The temperature of the water will increase

c)

The metal temperature will go up and water temperature will go down

d)

The water temperature will go up and the metal temperature will go down

162.

The calorie is a bigger unit than the Joule

a)

true

b)

false

163.

A potato chip has 10 Calories and is burned completely. How much heat does it give off.

a)

10 calories

b)

2390 Joules

c)

10,000 calories

d)

2.39 Joules

164.

Which of the following are specific heat units?

a)

cal

b)

Joule

c)

cal / *C

d)

joules / *C g

165.

A + B + heat ---> AB; Delta H, enthalpy is

a)

negative

b)

positive

c)

not enough information given

166.

A + B + heat ----- > AB; which statement is true?

a)

A and B have a greater energy

b)

AB has a geater energy

c)

The reaction is exothermic

d)

The reactants and products have the same energy

167.

A reaction that releases heat is

a)

endothermic

b)

exothermic

c)

exotic

d)

a combustion reaction

168.

3A + B + 350 J ------ > A3B; If the reaction absorbs 250 J, how many moles of A are needed?

a)

1.4 mol

b)

4.2 mol

c)

2.1 mol

d)

0.7 mol

169.

The heat required to change the temperature of 1 g of a substance by 1 degree C is

a)

one calorie

b)

one Joule

c)

specific heat capacity

d)

enthalpy

170.

What is the change of in enthalpy (kJ/mol) for the following reaction?

4 NH3 (g) + 5 O2 (g) ----> 4 NO (g) + 6 H2O (g)

Use Table 17.4 on page 530

a)

-904.6 kJ / mol

b)

-1274 kJ / mol

c)

-51.24 kJ / mol

d)

-794 kJ / mol

171.

What is the percent error when students find that a cheese puff has 2.8 Cal / gram and the manufacturer's value is 5.8 Cal / gram

a)

52 %

b)

48 %

c)

55 %

d)

45%

172.

How many calories are in 125 Joules? (1 cal = 4.18 J)

a)

523

b)

29.9

c)

0.0282

d)

65.7

173.

What is the specific heat of a 230 g metal that takes 3.1 kcal to heat from 25 *C to 83*C

a)

0.0023 cal /g *C

b)

0.23 cal /g *C

c)

3400 cal /g *C

d)

3.4 cal / g*C

174.

When 35 g of an alloy at 110 *C is dropped into 150 g of water at 23 *C, the final temperature is 35 *C. What is the specific heat of the alloy in calories?

a)

0.68

b)

1.5

c)

1.7

d)

1.9

175.

A piece of food has 4 Calories. If it was burned completely, how much heat would it give off?

a)

4 cal

b)

4000 cal

c)

17 joules

d)

not enough information is given

176.

A reaction is performed in a beaker with a temperature probe recording the temperature changes of the surroundings. If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius. If the reaction is our system, is the system endothermic or exothermic?

a)

Exothermic

b)

Endothermic

177.

Refer the the following question:
2N₂ + 3H₂ --> 2NH₃ + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?

a)

92 kJ

b)

0.143 kJ

c)

23 kJ

d)

15 kJ

178.

How much energy must be used to produce 4.75 mol of gaseous water?

H₂O (l) + 44.0 kJ --> H₂O (g)

a)

209 kJ

b)

9.26 kJ

c)

206 kJ

d)

9.36 kJ

179.

In a laboratory experiment a student was using Styrofoam cups and foil to reduce the energy lost during an exothermic reaction. The reaction constantly had a temperature probe in it. Towards the end of the reaction the student noticed the temperature in the cups was going down (opposite what they thought is should). The student concluded that the energy was destroyed within the system. This student's reasoning violates what law?

a)

Law of Conservation of Mass

b)

Law of Enthalpy

c)

First Law of Thermodynamics

d)

Law of Heat Transfer

180.

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.

181.

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.

182.

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)

183.

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

184.

A cast iron skillet is used to fry bacon. For optimal frying, the pan must be heated to about 178 ^oC from a room temperature of 22.0 ^oC. It is known that 1.58 x 10⁵ J of heat energy are absorbed by the pan to reach the desired temperature and the specific heat of iron is 0.450 J/g ^oC. What must the mass of the skillet be?

a)

12.7 kg

b)

2.25 kg

c)

110 kg

d)

1.97 kg

185.

When methane, CH4, and oxygen, O2, are mixed in a stove and ignited, a lovely blue flame results. The balanced equation is: CH₄(g) + 2O₂(g) 2H₂O(g) + CO₂(g) What can be said about the energy involved in this chemical reaction?

I. The average kinetic energy of the products is greater than that of the reactants.

II. The chemical energy stored in the reactants is greater than the chemical energy stored in the products.

III. Chemical energy in the reactants is changed into heat energy and light energy.

a)

I only

b)

II only

c)

III only

d)

I, II, and III

186.

The following is a thermochemical equation for the complete combustion of ethane:
2C₂H₆(g)+7O₂(g)→4CO₂(g)+6H₂O(g); ΔH=-3114 kJ/mol
If the activation energy of the reaction is 275 kJ per mol of ethane, the energy released, in kJ, during bond formation for the reaction as written above will be

a)

2564

b)

2839

c)

3389

d)

3664

187.

which of the following enthalpy changes represent the enthalpy change of formation?

a)

Mg(s) + Cl₂(g) → MgCl₂(s)

b)

Mg²⁺(g) + 2 Cl ^-(g) → MgCl₂(aq)

c)

O2(g) → 2 O(g)

d)

2Mg (s) + O₂(g) → 2MgO(S)

188.

If 100 g of aluminum at 145ºC gains 6,800 J of heat, what is the final temperature (T_final) of the aluminum? Aluminum has a specific heat of 0.897 J/gºC. (Q=mcΔT)

a)

-69°C

b)

0.52°C

c)

221°C

189.

Which statement is FALSE for an endothermic reaction?

a)

Products higher in energy and less stable

b)

Reactants lower in energy and more stable

c)

Products have stronger bonds than reactants

d)

Reactants have stronger bonds than products

190.

The diagram represents which type of reaction

a)

endothermic

b)

exothermic

191.

A reaction is performed in a beaker with a temperature probe recording the temperature changes of the surroundings. If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius. If the reaction is our system, is the system endothermic or exothermic?

a)

Exothermic

b)

Endothermic

192.

Refer the the following question:
2N₂ + 3H₂ --> 2NH₃ + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?

a)

92 kJ

b)

0.143 kJ

c)

23 kJ

d)

15 kJ

193.

How much energy must be used to produce 4.75 mol of gaseous water?

H₂O (l) + 44.0 kJ --> H₂O (g)

a)

209 kJ

b)

9.26 kJ

c)

206 kJ

d)

9.36 kJ

194.

In a laboratory experiment a student was using Styrofoam cups and foil to reduce the energy lost during an exothermic reaction. The reaction constantly had a temperature probe in it. Towards the end of the reaction the student noticed the temperature in the cups was going down (opposite what they thought is should). The student concluded that the energy was destroyed within the system. This student's reasoning violates what law?

a)

Law of Conservation of Mass

b)

Law of Enthalpy

c)

First Law of Thermodynamics

d)

Law of Heat Transfer

195.

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.

196.

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.

197.

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)

198.

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

199.

A cast iron skillet is used to fry bacon. For optimal frying, the pan must be heated to about 178 ^oC from a room temperature of 22.0 ^oC. It is known that 1.58 x 10⁵ J of heat energy are absorbed by the pan to reach the desired temperature and the specific heat of iron is 0.450 J/g ^oC. What must the mass of the skillet be?

a)

12.7 kg

b)

2.25 kg

c)

110 kg

d)

1.97 kg

200.

When methane, CH4, and oxygen, O2, are mixed in a stove and ignited, a lovely blue flame results. The balanced equation is: CH₄(g) + 2O₂(g) 2H₂O(g) + CO₂(g) What can be said about the energy involved in this chemical reaction?

I. The average kinetic energy of the products is greater than that of the reactants.

II. The chemical energy stored in the reactants is greater than the chemical energy stored in the products.

III. Chemical energy in the reactants is changed into heat energy and light energy.

a)

I only

b)

II only

c)

III only

d)

I, II, and III

201.

The following is a thermochemical equation for the complete combustion of ethane:
2C₂H₆(g)+7O₂(g)→4CO₂(g)+6H₂O(g); ΔH=-3114 kJ/mol
If the activation energy of the reaction is 275 kJ per mol of ethane, the energy released, in kJ, during bond formation for the reaction as written above will be

a)

2564

b)

2839

c)

3389

d)

3664

202.

which of the following enthalpy changes represent the enthalpy change of formation?

a)

Mg(s) + Cl₂(g) → MgCl₂(s)

b)

Mg²⁺(g) + 2 Cl ^-(g) → MgCl₂(aq)

c)

O2(g) → 2 O(g)

d)

2Mg (s) + O₂(g) → 2MgO(S)

203.

If 100 g of aluminum at 145ºC gains 6,800 J of heat, what is the final temperature (T_final) of the aluminum? Aluminum has a specific heat of 0.897 J/gºC. (Q=mcΔT)

a)

-69°C

b)

0.52°C

c)

221°C

204.

Which statement is FALSE for an endothermic reaction?

a)

Products higher in energy and less stable

b)

Reactants lower in energy and more stable

c)

Products have stronger bonds than reactants

d)

Reactants have stronger bonds than products

205.

The diagram represents which type of reaction

a)

endothermic

b)

exothermic

206.

On a heat curve, what is changing along the diagonal lines?

a)

temperature

b)

phase

c)

potential energy

d)

state

207.

How many Joules of energy are required to make 100 grams of ice at 0 ^οC completely melt? Ice has a heat of fusion of 334 J/g.

a)

200 J

b)

400 J

c)

33,400 J

d)

226,000 J

208.

Calculate the amount of energy required to boil 98.0 grams of liquid water. The heat of vaporization of water is 2260 J/g.

a)

221,480 J

b)

23 J

c)

32,732 J

d)

2260 J

209.

On the given heating curve, what is the substance's boiling point in °C?

a)

-60

b)

60

c)

-100

d)

100

210.

On this heat curve, which line segment represents only the solid state?

a)

AB

b)

BC

c)

CD

d)

DE

211.

The specific heat of Copper is 0.385 J/g °C. How much heat is required to raise the temperature of 23 g of copper from 20 °C to 50 °C?

a)

266 J

b)

620 J

c)

1792 J

d)

133 J

212.

How much heat is required to heat 5 g of mercury from 25 °C to 35 °C?

a)

7 J

b)

25 J

c)

18 J

d)

678 J

213.

You have 125 g of an unidentified substance. When you heat it from 25 °C to 60 °C it gives off 5478 J of heat. What is the specific heat of your substance?

a)

1.75 J/g °C

b)

0.89 J/g °C

c)

1.25 J/g °C

d)

0.50 J/g °C

214.

The heat absorbed or released during a chemical reaction is

a)

heat of fusion

b)

heat of vaporization

c)

enthalpy

d)

specific heat

215.

Energy is stored when chemical bonds are (1) and energy is released when chemical bonds are (2).

a)

1-formed, 2-broken

b)

1-broken, 2-formed

c)

1-heated, 2-cooled

d)

1-cooled, 2-heated

11 Review Thermochemistry

Total questions: 215

Worksheet time: 5hrs 47mins

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