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AP Chemistry Thermodynamics Test

Total questions: 143

Worksheet time: 7hrs 2mins

Name
Class
Date
1.
A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  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
2.
Enthalpy is energy absorbed or relased during a chemical reaction as
a)
light.
b)
heat.
c)
sound.
d)
pressure.
3.
In an endothermic reaction, the sum of the heats of formation of the products are____than the sum of the heats of formation of the reactants. Hint: is ΔH + or -? This about how you calculate ΔH
a)
less than
b)
greater than
c)
equal to
4.

Calculate the change in enthalpy  ΔH\Delta H  for the following reaction:
2CO + O2 ⟶ 2CO22CO\ +\ O_{2_{\ _{ }}^{ }}\longrightarrow\ 2CO_{2_{ }}  
Use your heats of formation table from your worksheet

a)

-393.5 kJ/mol

b)

-566.0 kJ/mol

c)

566.0 kJ/mol

d)

-369 kJ/mol

5.

Which one of the following expressions is the correct way to calculate standard enthalpy change for the combustion of propane?

C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(l)

Use your heats of formation table for reference.

a)

[103.85 + (5 × 286)] – [-393.5 + -285.8]

b)

[-103.85 + 0] + [(3 x -393.5) + (4 x -285.8)]

c)

[-103.85 + 0] – [(3 x -393.5) + (4 x -285.8)]

d)

[(3 x -393.5) + (4 x -285.8)] + [-103.85 + 0]

6.

What is the heat of formation for 6 moles of ethanol? Use your heats of formation table for reference.

a)

-1666.2 kJ/mol

b)

-277.7 kJ/mol

c)

52.3 kJ/mol

d)

Only able to calculate in a reaction

7.

Calculate ΔH\Delta H  using heats of formation for the combustion of methane:
CH4(g) + 2O2(g) → CO2(g) +2H2O(l)CH_4\left(g\right)\ +\ 2O_2\left(g\right)\ \rightarrow\ CO_2\left(g\right)\ +2H_2O\left(l\right)  
Use your heats of formation table for reference.

a)

-890.25 kJ/mol

b)

-604.45 kJ/mol

c)

-754.15 kJ/mol

d)

No way to tell

8.

What is the difference between calculating ΔH\Delta H   with bond energies versus with heats of formation?

a)

Bond energies are averages based on multiple scenarios of breaking bonds, heats of formation is the energy required to form a specific molecule from its elemental forms.

b)

Heats of formation are averages based on multiple scenarios of breaking bonds, bond energies is the energy required to form a specific molecule from its elemental forms.

c)

Bond energies are calculated using only lewis dot structures, but heats of formation requires a reference table

d)

Heats of formation helps calculate enthalpy, while bond energies helps calculate entropy

9.

What is the heat of formation for 8 moles of ammonia? Use your heats of formation table for reference.

a)

-369.52 kJ/mol

b)

-46.19 kJ/mol

c)

-92.38 kJ/mol

d)

-102.4 kJ/mol

10.
In an endothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released 
11.
If the enthalpy ter (ΔH) is negative the reaction is ____.
a)
Endothermic
b)
Exothermic
c)
Neutral
12.

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.

13.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
14.

What is the Heat of Reaction ΔH\Delta H  for this reaction?

a)

-200 KJ

b)

200 KJ

c)

400 KJ

d)

-300 KJ

15.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

16.
Endothermic reactions feel
a)
warm
b)
cold
17.

The enthalpy change for the reaction

C(s, graphite) + 1⁄2O2(g) --> CO(g) cannot be measured directly since some carbon dioxide is always formed in the reaction.

It can be calculated using Hess’s Law and the enthalpy changes of combustion of graphite and of carbon monoxide.

C(s, graphite) + O2(g) --> CO2 ΔH=-394 kJmol–1

CO(g) + 1⁄2O2(g) --> CO2 ΔH=-283 kJmol–1

The enthalpy change for the reaction of graphite with oxygen to give carbon monoxide is

a)

-677 kJmol–1

b)

-111 kJmol–1

c)

+111 kJmol–1

d)

+677 kJmol–1

18.

The enthalpies of formation of C(s), H2(g) and C4H9OH(l) (in kJmol-1) are as follows

C(s) ∆H=a

H2(g) ∆H=b

C4H9OH(l) ∆H=c

What is the enthalpy change for the reaction shown below?

4C(g) + 5H2(l) + ½O2(g) -> C4H9OH(l)

a)

c – 4a + 5b

b)

4a + 5b - c

c)

2a + 10b - c

d)

2a + 5b + c

19.
(Hess's Law)Calculate the ∆H for the following reaction: 2H2O2 →  2H2O  + 1 O2 
You are given these two equations:
2H2  +  O2 → 2H2O            ∆H  =  -572 kJ
 H2  +  O2  →  H2O2            ∆H  =  -188 kJ 
a)
∆H  =  -948 kJ 
b)
∆H  =  -196 kJ 
c)
∆H  =  -384 kJ 
d)
∆H  =  -188 kJ 
20.

How do you calculate the Enthalpy of Reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔG = ΔH -TΔS

c)

ΔT = q / mC

d)

E = mc2

21.

Systemsincludes _______.

a)

reactants

b)

products

c)

both reactants and products

d)

None of the above

22.

Change in enthalpy is also called as _______.

a)

Systematic Reaction

b)

Balanced Reaction

c)

Energy of Reaction

d)

Heat of Reaction

23.

Endothermic:_________:__________

Exothermic:_________:__________

a)

positive:warm

negative:cold

b)

positive:warm

negative:warm

c)

positive:cold

negative:cold

d)

positive:cold

negative:warm

24.

When the solids Ba(OH)2 and NH4SCN are mixed, a solution is produced and the temperature drops. Which statement about the energetics of this reaction is correct?

a)

The reaction is endothermic and ΔH is negative

b)

The reaction is endothermic and ΔH is positive

c)

The reaction is exothermic and ΔH is negative

d)

The reaction is exothermic and ΔH is positive

25.

Which of the following represents an exothermic reaction?

a)
b)
26.
What is the second law of thermodynamics state
a)
Cold air always rises
b)
Hot air always rises
c)
thermal energy can be lost
d)
Thermal energy always transfers to cooler objects
27.
What is "Entropy"?
a)
The tendency of objects to warm up
b)
The tendency of energy to spread out
c)
The tendency of energy to make heat
d)
The tendency of objects to do work
28.
In order for energy to be less concentrated what must be done?
a)
Heat released
b)
Reduce thermal energy
c)
Work
d)
Increase Radiation
29.
What heating system is most common in newer homes?
a)
Forced air
b)
A Radiator
c)
Electrical
d)
Convection
30.
What do we call the relationship between thermal energy, heat and work?
a)
Closed System
b)
Entropy
c)
Conductors
d)
Thermodynamics
31.
Why can't a heat engine be 100% efficient?
a)
Heat is always created
b)
No work can be done
c)
Entropy is lost
d)
Thermal energy decreases
32.
Which would have more entropy?
a)
Frozen ice cream
b)
Liquid Ice cream
33.
In which of the following systems is entropy increasing?
a)
Putting together a puzzle
b)
Putting books on a shelf
c)
Breaking a plate
d)
Filling a jar of salt
34.
Which of the following describes the first law of thermodynamics?
a)
The increase in thermal energy equals the work done
b)
Energy becomes less concentrated over time
35.
How can energy be transferred from a cool object to a warm object?
a)
Work must be done
b)
Increase thermal energy
c)
Use convection
d)
Q=mTC
36.
What is the name of a device that converts thermal energy into work?
a)
Heating system
b)
Heat engine
c)
Entropy
d)
Power
37.
“When thermal energy is converted into work, some thermal energy is always transferred to the surroundings.”
a)
True
b)
False
38.
How does a refrigerator work?
a)
Moves heat from inside the fridge to the room
b)
Blows cold air into the fridge
c)
Uses convection cells
d)
It generates cold air
39.
You blow up a balloon and do not tie the end.  When you let go the air flows out of the balloon. Why?
a)
The balloon is doing work
b)
Energy is being concentrated
c)
Entropy is decreasing
d)
Entropy is increasing
40.
A closed system is when energy flows across the boundary.
a)
True 
b)
False
41.

Which has higher entropy?

A. A small pool of water sits in an enclosed glass chamber.

B. An enclosed glass chamber is filled with water vapor.

a)

A

b)

B

42.

Which has higher entropy?

A. A fried egg rests on a plate.

B. A fresh, uncooked egg rests on a plate.

a)

A

b)

B

43.

Which has higher entropy?

A. A car is at rest in a driveway with a full tank of gas.

B. A car drives down the highway with half a tank of gas left.

a)

A

b)

B

44.

Which has higher entropy?

A. A box contains 1 million gas particles, all within the left half of the box.

B. 1 million gas particles are more or less evenly distributed throughout both halves of a box.

a)

A

b)

B

45.

Which has higher entropy?

A. Broken pieces of glass lie on a wet floor.

B. A glass of water sits on top of a table.

a)

A

b)

B

46.

Which has higher entropy?

A. An enclosed space is filled with ash and smoke particles.

B. A pile of logs sits on the floor of an enclosed space.

a)

A

b)

B

47.
Entropy increases from solid, liquid to gas. Why?
a)
Molecular disorder increases
b)
Molecular randomness decreases
c)
Molecules are more energetic
d)
Molecules are more reactive
48.

Which of the following is the best example of The Second Law of Thermodynamics?

a)

A bike parked at the top of a hill has stored potential energy

b)

A bike rolling down a hill has kinetic energy

c)

Water flowing over a dam is used to generate electricity

d)

Some of the potential energy stored in gasoline is lost as heat when burned in a car's engine

49.

Which of the following correctly describes the entropy changes of the water molecules and the universe when a sample of water freezes?

a)

A

b)

B

c)

C

d)

D

50.
Which statement is true about the ENTROPY?
a)
Entropy refers to DISORDER, the unusable energy that escapes a system.
b)
Entropy refers to the balance of temperature among two or more systems.
c)
Entropy refers to the average kinetic energy of the molecules.
d)
Entropy refers to the inability to destroy or create energy. 
51.
Which state of H2O  has the greatest entropy?
a)
Ice
b)
Water
c)
Vapor
52.
As a system becomes more disordered, entropy
a)
remains the same
b)
increases
c)
decreases
d)
cannot be determined
53.
Entropy increases from solid, liquid to gas. Why?
a)
Molecular disorder increases
b)
Molecular randomness decreases
c)
Molecules are more energetic
d)
Molecules are more reactive
54.

What information do we need to perform a calculation of Gibbs Free Energy?

a)

Enthalpy of the reaction.

b)

Entropy of the reaction.

c)

The temperature of the reaction in Kelvin.

d)

All of the above are needed.

55.
A reaction has a positive ΔH and a positive ΔS. Which of the following is true?
a)
It will be spontaneous at all temperatures.
b)
It will be nonspontaneous at all temperatures.
c)
It will be spontaneous at low temperatures.
d)
It will be spontaneous at high temperatures.
56.

Your enthalpy is +20 and your entropy is +5. Which temperature will give a spontaneous reaction?

a)

0

b)

4

c)

8

57.

Your enthalpy is high and negative but your entropy is also negative. What type of temperature would you want to get a spontaneous reaction?

a)

low

b)

high

58.

Which combination of ΔH and ΔS NEVER has a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

59.

At what temperature would a given reaction become spontaneous if ΔH =+119kJ and ΔS=+263J/K.mol

a)

455 K

b)

-2210 K

c)

382 K

d)

-363 K

60.
True/False: The rate of a chemical reaction is unrelated to the spontaneity of the reaction.
a)
True
b)
False
61.

6. The formation ½ A2 + 2 B2 + C --> CAB4 has an enthalpy of formation of -104 kJ and a change in entropy of -60.8 J/K at 30 °C. What is the free energy and spontaneity of the reaction?

a)

-85.6 kJ, spontaneous

b)

-18.3 kJ, not spontaneous

c)

+18.3 kJ, spontaneous

d)

+85.6 kJ, not spontaneous

62.

enthalpy is driving force when

a)

exothermic

b)

endothermic

c)

increase in entropy

d)

decrease in entropy

63.

If a reaction occurs, then delta G is

a)

negative

b)

positive

c)

can't tell

d)

0

64.

What are the signs on G, H, and S if a solid is combined with another solid, a gas forms and the temperature drops?

a)

+, +, +

b)

- , - , -

c)

- ,+, +

d)

+ , +, -

65.

Which statement is true regarding the desublimation of gaseous CO2?

a)

ΔH is negative, ΔS is positive, and ΔG is negative at all temperatures.

b)

ΔH is positive, ΔS is negative, and ΔG is positive at all temperatures.

c)

ΔH is positive, ΔS is positive, and ΔG is positive at low temperature and negative at high temperature.

d)

ΔH is negative, ΔS is negative, and ΔG is negative at low temperature and positive at high temperature.

66.

What is the significance of the change in Gibbs free energy (ΔG) for a reaction?

The change in Gibbs free energy for a process is ​ (a)   to the ​​ (b)   of ΔSuniv. Since ΔSuniv is a criterion for ​ (c)   , ΔG is also a criterion for ​ (d)   (although opposite in sign).

Choose from the below words
proportional
negative
spontaneity
inversely proportional
slow reactions
fast reactions
positive
high reaction yield
67.

Calculate the change in Gibbs free energy for each set of ΔH°rxn, ΔS°rxn, and T. (Assume that all reactants and products are in their standard states.)

ΔH°rxn = +119 kJ ; ΔS°rxn = −242 J/K ; T = 308K

Express your answer in kilojoules to three significant figures.

ΔG°rxn = (a)   KJ

68.

Calculate the change in Gibbs free energy for each set of ΔH°rxn, ΔS°rxn, and T. (Assume that all reactants and products are in their standard states.)

ΔH°rxn = −119 kJ ; ΔS°rxn = +242 J/K ; T = 308 K
Express your answer in kilojoules to three significant figures.

ΔG°rxn = (a)   kJ

69.

Calculate the change in Gibbs free energy for each set of ΔH°rxn, ΔS°rxn, and T. (Assume that all reactants and products are in their standard states.)

ΔH°rxn = −119 kJ ; ΔS°rxn = −242 J/K ; T = 308 K

Express your answer in kilojoules to three significant figures.

ΔG°rxn = (a)   kJ

70.

Calculate the change in Gibbs free energy for each set of ΔH°rxn, ΔS°rxn, and T. (Assume that all reactants and products are in their standard states.)

ΔH°rxn = −119 kJ ; ΔS°rxn = −242 J/K ; T = 711 K

Express your answer in kilojoules to three significant figures.

ΔG°rxn = (a)   kJ

71.

Predict whether each reaction is spontaneous at the temperature indicated.

Drag the appropriate items to their respective bins.

Categorize the following

Reaction in part C ΔG = -44.5 kJ

Reaction In part B ΔG = -194 kJ

Reaction in part D ΔG = 53.1 kJ

Reaction in part A ΔG = 194 kJ

Spontaneous
Nonspontaneous
72.

What does Gibbs Free Energy tell us?

a)

How much energy is given off by a reaction.

b)

The tendency of a reaction to become "random"

c)

How spontaneous a reaction is.

73.

What information do we need to perform a calculation of Gibbs Free Energy?

a)

Enthalpy of the reaction.

b)

Entropy of the reaction.

c)

The temperature of the reaction in Kelvin.

d)

All of the above are needed.

74.

Which of the following would most likely lead to a spontaneous reaction.

a)

A high negative enthalpy.

b)

A low negative enthalpy.

c)

A high positive enthalpy.

d)

A low positive enthalpy.

75.

What are the best conditions to lead towards a spontaneous reaction?

a)

high negative enthalpy, high temp, high negative entropy

b)

high positive enthalpy, high temp, high negative entropy

c)

high negative enthalpy, low temp, high positive entropy

d)

high negative enthalpy, high temp, high positive entropy.

76.

Your enthalpy is high and negative but your entropy is also negative. What type of temperature would you want to get a spontaneous reaction?

a)

low

b)

high

77.

Your enthalpy is positive and your entropy is positive. What type of temperature would you want to ensure a spontaneous reaction.

a)

very high

b)

very low

78.

Your enthalpy is +20 and your entropy is +5. Which temperature will give a spontaneous reaction?

a)

0

b)

4

c)

8

79.

Your enthalpy is -20 and your entropy is -8. Which temperature will give you a spontaneous reaction?

a)

1

b)

3

c)

5

80.

Which of the following situations demonstrates high entropy?

a)

water freezing

b)

water vaporizing

c)

steam condensing to water

81.

A spontaneous reaction is more profitable to a company.

a)

True

b)

False

82.
Entropy increases from solid, liquid to gas. Why?
a)
Molecular disorder increases
b)
Molecular randomness decreases
c)
Molecules are more energetic
d)
Molecules are more reactive
83.

Which represents a decrease in entropy?

a)

sublimation of CO2

b)

boiling water

c)

condensation of steam on cold glass

d)

NaCl dissolving in water

84.

The entropy will usually increase when

a)

a molecule is broken into two or more smaller molecules

b)

a reaction occurs that results in an increase in the number of moles of gas

c)

a solid changes to a liquid

d)

all of these

85.

Which sample has the lowest entropy?

HINT - Look at the phase of each chemical....

a)

1 mole of KNO3(l)

b)

1 mole of KNO3(s)

c)

1 mole of H2O(l)

d)

1 mole of H2O(g)

86.
Which phase of matter has the greatest motion and least orderly arrangement?
a)
solid
b)
liquid
c)
gas
87.

Which phase change represents a decrease in entropy?

a)

solid to liquid

b)

gas to liquid

c)

liquid to gas

d)

solid to gas

88.
Entropy always increases when
a)
enthalpy decreases.
b)
temperature decreases.
c)
temperature increases.
d)
volume increases.
89.

Entropy is a measure of

a)

accuracy

b)

precision

c)

the disorder of a system

d)

the attraction of a nucleus for an electron

90.

Given the change of phase:

CO2(g) —> CO2(s)

As CO2(g) changes to CO2(s), the entropy of the system

a)

decreases

b)

increases

c)

remains the same

91.

What is a spontaneous process ?

a)

slow process

b)

fast process

c)

process that needs an external intervention to occur

d)

process that does not need external intervention to occur / keep happening

92.

Given the change of phase:

CO2(g) —> CO2(s)

As CO2(g) changes to CO2(s), the entropy of the system

a)

decreases

b)

increases

c)

remains the same

93.

What information do we need to perform a calculation of Gibbs Free Energy?

a)

Enthalpy of the reaction.

b)

Entropy of the reaction.

c)

The temperature of the reaction in Kelvin.

d)

All of the above are needed.

94.

What does Gibbs Free Energy tell us?

a)

How much energy is given off by a reaction.

b)

The tendency of a reaction to become "random"

c)

How spontaneous a reaction is.

95.

When a reaction is exothermic and the products have more entropy than the reactants, the reaction is;

a)

Spontaneous with a positive ΔG

b)

Spontaneous with a negative ΔG

c)

Non-Spontaneous with a positive ΔG

d)

Non-Spontaneous with a negative ΔG

96.

Which of the following would most likely lead to a spontaneous reaction.

a)

A high negative enthalpy.

b)

A low negative enthalpy.

c)

A high positive enthalpy.

d)

A low positive enthalpy.

97.
A reaction has a positive ΔH and a positive ΔS. Which of the following is true?
a)
It will be spontaneous at all temperatures.
b)
It will be nonspontaneous at all temperatures.
c)
It will be spontaneous at low temperatures.
d)
It will be spontaneous at high temperatures.
98.

Your enthalpy is +20 and your entropy is +5. Which temperature will give a spontaneous reaction?

a)

0

b)

4

c)

8

99.

Your enthalpy is positive and your entropy is positive. What type of temperature would you want to ensure a spontaneous reaction.

a)

very high

b)

very low

100.

Which combination of ΔH and ΔS NEVER has a spontaneous reaction?

a)

+ΔH and +ΔS

b)

+ΔH and -ΔS

c)

-ΔH and -ΔS

d)

-ΔH and +ΔS

101.

Predict the signs of ΔH , ΔS and ΔG for the reaction:

Mg(s) --> Mg(g)

a)

Δ H = - , Δ S = + and Δ G = - (all temperature)

b)

Δ H = + , Δ S = + and Δ G = - (At all temperature)

c)

Δ H = + , Δ S = + and Δ G = - (At low temperature)

d)

Δ H = + , Δ S = + and Δ G = - (At high temperature)

102.

Your enthalpy is high and negative but your entropy is also negative. What type of temperature would you want to get a spontaneous reaction?

a)

low

b)

high

103.

A reactionthat is spontaneous at any temperature has a

-------------- entropy and a ---------------- enthalpy.

a)

positive, positive

b)

positive, negative

c)

negative, negative

d)

negative, positive

104.

Which is correct for the reaction H2O (g) → H2O (l) ?


A. Enthalpy increases and entropy increases.

B. Enthalpy decreases and entropy increases.

C. Enthalpy increases and entropy decreases.

D. Enthalpy decreases and entropy decreases.

a)

A

b)

B

c)

C

d)

D

105.

When the solids Ba(OH)2 and NH4SCN are mixed, a solution is produced and the temperature drops. Which statement about the energetics of this reaction is correct?

a)

The reaction is endothermic and ΔH is negative

b)

The reaction is endothermic and ΔH is positive

c)

The reaction is exothermic and ΔH is negative

d)

The reaction is exothermic and ΔH is positive

106.

The following equation shows the formation of magnesium oxide from magnesium metal. Which statement is correct for this reaction?

2Mg(s) + O2(g) → 2MgO(s) ΔH = -1204 kJ

a)

1204 kJ of energy are released for every mole of magnesium reacted

b)

602 kJ of energy are absorbed for every mole of magnesium oxide formed

c)

602 kJ of energy are released for every mole of oxygen reacted

d)

1204 kJ of energy are released for every two moles of magnesium oxide formed

107.

For the reaction 2H2(g) + O2(g) → 2H2O(g) the bond enthalpies (in kJ/mol) are

H-H = x, O=O = y, O-H = z

Which calculation will give the value, in kJ/mol, of ΔH for the reaction?

a)

2x + y - 2z

b)

4z - 2x - y

c)

2x + y - 4z

d)

2z - 2x - y

108.
Which is an example of an endothermic physical reaction? 
a)
a) Ice melting 
b)
b) Combustion 
c)
c) Steam condensing 
d)
d) Photosynthesis
109.

Using the table of average bond energies below the image, the ΔH for the reaction in kJ is.....

a)

+ 160 kJ

b)

-63 kJ

c)

- 160 kJ

d)

-217 kJ

110.

Does breaking bonds require energy, release energy, or not involve energy at all?

a)

requires energy to break

b)

releases energy when broken

c)

No energy involved

111.

What kind of energy change happens in the photosynthesis reaction in plant leaves?

a)

Endothermic

b)

Exothermic

c)

No change

112.

Is this equation endo- or exo-thermic?

PCl3 (s) + Cl2 (g) --> PCl5 (s) + energy

a)

endothermic

b)

exothermic

113.

Is this equation endo- or exo-thermic?

2KNO3 (s) + energy --> 2KNO2 (s) + O2

a)

endothermic

b)

exothermic

114.

How can we figure out if an overall reaction is endo- or exo-thermic? It is the difference between _______ and __________.

a)

hot and cold temperatures

b)

energy to break and energy to form bonds.

c)

time to form a bond versus time to break a bond

115.
For the formula:
 Q= m c ∆T
The  units for specific heat are:
a)
g /J C
b)
°C/g J
c)
kJ/g
d)
J/g°C
116.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
117.

If two objects have different temperatures when they come in contact, 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

118.
The total energy of all the particles in a substance is called: 
a)
temperature
b)
thermal energy
c)
degrees
d)
mass
119.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? (show your work)

a)

-80,256 J

b)

80.256 J

c)

80,256 J

d)

-80.256 J

120.
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
121.

For a skillet, used for cooking, do you want a high or low specific heat

a)

High, so that it will need more energy to heat up

b)

Low, so that it will change temperature quickly

122.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
123.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?  (show your work)
a)
25g
b)
30g
c)
20g
d)
50g
124.
A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius. Is the reaction endothermic or exothermic?
a)
Exothermic
b)
Endothermic
125.
Calorimetry Question:
A piece of metal with a mass of 32.8 g is heated to 100.5°C and dropped into 138.2 g of water at 20.0°C.  The final temperature of the system is 30.2°C.  What is the specific heat capacity of the metal? (show your work)
a)
2.56 J/g°C
b)
0.391 J/g°C
c)
5.29 J/g°C
d)
3.50 J/g°C
126.
In an exothermic process, the surroundings are gaining energy.
a)
True
b)
False
127.

What does "q" mean?

a)

A measure of heat energy

b)

A change in heat energy

c)

A measure of kinetic energy

d)

A change in temperature

128.
What is a tool that measures the heat of chemical reactions?
a)
calorimeter
b)
 calorie
c)
Styrofoam™ cup
d)
none of these
129.
Calorimeters use insulating materials to:
a)
encourage affordable materials in science experiments in schools.
b)
preserve the heat of the environment outside the Styrofoam cup.
c)
prevent heat from escaping to the environment.
d)
keep the liquid inside the Styrofoam cup from overheating.
130.
A metal cube at temperature of 10°C immersed in a liquid at temperature of 70°C.
What is the temperature of the metal cube when thermal equilibrium is achieved between the cube and the liquid?
a)
Between 10°C and 70°C
b)
More than 70°C
c)
Less than 10°C
d)
Same as the room temperature
131.

The specific heat of water is 4.18 J/g°C.

If 980. J of energy is added to 6.20 g of water at 18.0 °C, what is the final temperature of the water?

a)

37.8 °C

b)

-19.8 °C

c)

19.8 °C

d)

55.8 °C

132.

What does "ΔT" mean?

a)

A change in health

b)

A change in heat

c)

A change in height

d)

A change in temperature

133.

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

a)

-65*C

b)

75*C

c)

10*C

d)

65*C

134.

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

135.

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

a)

4.18 j/g*C

b)

10000g

c)

174724g

d)

100g

136.

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

a)

16j

b)

.0016j

c)

16000j

d)

625 j

137.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

138.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

139.

What does q stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

140.

What does c stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

141.

What does ΔT\Delta T   stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

142.

What does m stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

143.

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

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