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Thermodynamics

Total questions: 165

Worksheet time: 4hrs 2mins

Name
Class
Date
1.

True or False? Temperature is a measure of the total kinetic energy in a substance.

a)

True

b)

False

2.

Select the correct SI unit for Heat

a)

calorie

b)

joule

c)

kelvin

d)

celsius

3.

Select the correct SI unit for temperature

a)

calorie

b)

joule

c)

kelvin

d)

celsius

4.

Select the correct symbol for Heat

a)

H

b)

t

c)

Q

d)

E

5.

If system A and system B have no heat flow between them and system B and system C have no heat flow between them, what do systems A and C have in common?

a)

They must have no heat flow between them

b)

A is hotter than C

c)

C is hotter than A

d)

Heat is flowing back and forth between the two systems rapidly.

6.

The transfer of heat through a fluid (liquid or gas) is...

a)

Conduction

b)

Convection

c)

Radiation

d)

Ablation

7.

What method of heat transfer is causing heat to flow from the tip of the spoon to the handle of the spoon?

a)

Conduction

b)

Convection

c)

Radiation

d)

Erosion

8.

What method of heat transfer do solar panels rely on?

a)

Conduction

b)

Convection

c)

Radiation

d)

Nucleation

9.

A wool blanket is an example of a good ___________.

a)

Radiator

b)

Conductor

c)

Insulator

d)

Equilizer

10.

What is the branch of physics concerned with heat and temperature?

a)

Kinematics

b)

Mechanics

c)

Optics

d)

Thermodynamics

11.

A measure of the amount of disorder or randomness in a system.

a)

Entropy

b)

Exothermic

c)

First Law of Thermodynamics

d)

Heat engine

12.

The law stating that energy is neither created nor destroyed; it only changes form. It is also known as the law of conservation of energy.

a)

First Law of Thermodynamics

b)

Second Law of Thermodynamics

c)

Third Law of Thermodynamics

d)

Fourth Law of Thermodynamics

13.

A law stating that all spontaneous processes result in an increase in the total entropy of the system and its surroundings.

a)

First Law of Thermodynamics

b)

Second Law of Thermodynamics

c)

Third Law of Thermodynamics

d)

Fourth Law of Thermodynamics

14.

Consider 2 blocks of Aluminium (one of 1kg and one of 10 kg) and being supplied with thermal energy.

Which one heats up the fastest?

a)

1 kg

b)

10 kg

c)

They both heat up at the same rate

d)

They don't heat up.

15.

The specific heat(c) of copper is 0.39 Jg-1K-1. What is the temperature change(∆T) when 100 Joules of heat(Q) is added to 20 grams?

a)

12.82 °C

b)

24.12°C

c)

351 °C

16.
Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using the same thermal energy.  What material would be the coolest after being heated?
a)
Copper
b)
Carbon Steel
c)
Zinc
d)
Stainless Steel
17.
Heat energy moves from __________ things to _________ things.
a)
warm / cold
b)
cold / warm
c)
liquid / solid
18.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
19.

Specific heat of water is 4.18 J/g°C. Specific heat of wood is 1.760 J/g°C What material needs more heat energy to raise the temperature?

a)

Water

b)

Wood

c)

Both are same

20.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
21.
A(n) _____________ is a device for measuring temperature.
a)
thermometer
b)
barometer
c)
anemometer
d)
psychrometer 
22.
Temperature is a measure of the...
a)
total energy in a substance
b)
total kinetic energy in a substance
c)
average potential energy in a substance
d)
average kinetic energy of molecules in a substance
23.
A slower particle has a lower energy than an identical, faster particle.
a)
True
b)
False
24.
The transfer of thermal energy between objects of different temperatures is called...
a)
temperature
b)
heat
c)
internal energy
d)
none of these
25.
It is possible to reach absolute zero
a)
true
b)
false
26.
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.
27.
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
28.
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
29.
Heat travels from the sun to the earth by the process of...
a)
conduction
b)
convection
c)
radiation
d)
insulation
30.
A substance with a high specific heat:
a)
Is always extremely hot.
b)
Requires a lot of energy to become hot.
c)
Is not heavy.
d)
Does not requires a lot of energy to become hot.
31.
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.
32.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
33.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
34.
What type of reaction is shown in the reaction pathway?
a)
endothermic reaction
b)
exothermic reaction
35.

How do you calculate Enthalpy of a reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔT = q / mC

c)

ΔG = ΔH -TΔS

d)

E = mc2

36.
Which statement is true regarding endothermic reactions?
a)
a) Temperature change is positive and enthalpy change is positive
b)
b) Temperature change is positive and enthalpy change is negative
c)
c) Temperature change is negative and enthalpy change is positive
d)
d) Temperature change is negative and enthalpy change is negative
37.
Endothermic reactions feel
a)
warm
b)
cold
38.
Define 'Enthalpy'
a)
a) Energy stored in the movement of molecules in a substance
b)
b) The opposite of temperature
c)
c) The temperature of a molecule
d)
d) Energy stored in the chemical bonds in a substance
39.

A reaction that gives out energy to the surroundings causes the surroundings ....

a)

temperature to drop

b)

temperature to rise

c)

temperature to remain constant

d)

temperature to vary

40.

The enthalpy change is a negative (-) value, what side of the equation will the energy value be on.

a)

Reactants

b)

Products

41.

In the reaction picture, the energy will be on product or reactant

a)

Product

b)

Reactant

42.
 _?_  is the amount of energy required to raise the temperature of 1 gram of any substance 1oC.
a)
Specific heat
b)
A calorie
c)
Thermal energy
d)
Conduction
43.
What type of reaction is shown in the reaction pathway?
a)

endothermic reaction

b)

exothermic reaction

44.

In the Image, will the heat (+177.8 KJ) be a product or a reactant?

a)

Product

b)

Reactant

45.

In the Image, will the heat (+177.8 KJ) be a product or a reactant?

a)

Product

b)

Reactant

46.
If the enthalpy ter (ΔH) is negative the reaction is ____.
a)
Endothermic
b)
Exothermic
c)
Neutral
47.

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.

48.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
49.

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

a)

-200 KJ

b)

200 KJ

c)

400 KJ

d)

-300 KJ

50.

What type of reaction is this?

a)

Exothermic

b)

Endothermic

c)

Energy Producing

d)

No way to tell

51.
Endothermic reactions feel
a)
warm
b)
cold
52.

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

53.

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

54.
(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 
55.

How do you calculate the Enthalpy of Reaction?

a)

ΔH = ΔHproducts - ΔHreactants

b)

ΔG = ΔH -TΔS

c)

ΔT = q / mC

d)

E = mc2

56.

Systemsincludes _______.

a)

reactants

b)

products

c)

both reactants and products

d)

None of the above

57.

Change in enthalpy is also called as _______.

a)

Systematic Reaction

b)

Balanced Reaction

c)

Energy of Reaction

d)

Heat of Reaction

58.

Endothermic:_________:__________

Exothermic:_________:__________

a)

positive:warm

negative:cold

b)

positive:warm

negative:warm

c)

positive:cold

negative:cold

d)

positive:cold

negative:warm

59.

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

60.

Which of the following represents an exothermic reaction?

a)
b)
61.

Find the enthalpy of formation for the following chemical equation.

CH4 (g) + 2 O2 (g) --> CO2 (g) + 2 H2O (g)

a)

-802.3 kJ

b)

802.3 kJ

c)

951.9 kJ

d)

-951.9 kJ

62.

Find the enthalpy of formation for the following chemical reaction.

2Al (s) + Fe2O3 (s) --> Al2O3 (s) + 2Fe (s)

a)

-847.6 kJ

b)

847.6 kJ

c)

2492 kJ

d)

-2492 kJ

63.

Find the enthalpy change that occurs over the following two-step equations.

2 H2 (g) + O2 (g) --> 2 H2O (l) ΔH = -572 kJ

2 H2O2 (l) --> 2 H2 (g) + 2 O2 (g) ΔH = 376 kJ

a)

-196 kJ

b)

-948 kJ

c)

196 kJ

d)

948 kJ

64.

Find the change in enthalpy over the following two-step equations.

N2 (g) + O2 (g) --> 2 NO (g) ΔH = 180kJ

2 NO (g) + O2 (g) --> 2 NO2 ΔH = -112kJ

a)

-292 kJ

b)

-68 kJ

c)

292 kJ

d)

68 kJ

65.

How much energy would it take to condense 4.9 moles of C2H5OH?

a)

189.14 kJ

b)

-189.14 kJ

c)

24.206 kJ

d)

-24.206 kJ

66.

How much energy is required to turn 7.3 moles of NH3 from a solid to a liquid?

a)

-170.09 kJ

b)

-41.32 kJ

c)

41.32 kJ

d)

170.09 kJ

67.

Which of these processes represents a decrease in entropy?

a)

sublimation of CO2

b)

boiling water

c)

condensation of steam on cold glass

d)

NaCl dissolving in water

68.

Which of these reactions shows a DECREASE in entropy?

a)

CaCO3(s) → CaO(s) + CO2(g)

b)

3O2(g) → 2O3(g)

c)

2NH3(g) → 3H2(g) + N2(g)

d)

C6H6(l) → C6H6(g)

69.

Which reaction has a +ΔS ?

a)

AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

b)

H2O(g) + CO2(g) → H2CO3(aq)

c)

H2(g) + I2(g) → 2Hl(g)

d)

C2H2O2(g) → 2CO(g) + H2(g)

70.

Systems in nature tend to undergo changes toward

a)

lower energy and less disorder

b)

lower energy and more disorder

c)

higher energy and less disorder

d)

higher energy and more disorder

71.

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

72.

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.

73.

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.

74.
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.
75.

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

a)

0

b)

4

c)

8

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.

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

78.

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

a)

1

b)

3

c)

5

79.

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

a)

452 K

b)

-2210 K

c)

382 K

d)

-363 K

80.
True/False: The rate of a chemical reaction is unrelated to the spontaneity of the reaction.
a)
True
b)
False
81.

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

82.

What is the symbol for entropy?

a)

H

b)

G

c)

S

d)

E

83.

Entropy is a measure of

a)

accuracy

b)

precision

c)

the disorder of a system

d)

the attraction of a nucleus for an electron

84.

Which of these processes represents a decrease in entropy?

a)

sublimation of CO2

b)

boiling water

c)

condensation of steam on cold glass

d)

NaCl dissolving in water

85.

Which of these reactions shows a DECREASE in entropy?

a)

CaCO3(s) → CaO(s) + CO2(g)

b)

3O2(g) → 2O3(g)

c)

2NH3(g) → 3H2(g) + N2(g)

d)

C6H6(l) → C6H6(g)

86.

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

87.

Which reaction has a +ΔS ?

a)

AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)

b)

H2O(g) + CO2(g) → H2CO3(aq)

c)

H2(g) + I2(g) → 2Hl(g)

d)

C2H2O2(g) → 2CO(g) + H2(g)

88.

Systems in nature tend to undergo changes toward

a)

lower energy and less disorder

b)

lower energy and more disorder

c)

higher energy and less disorder

d)

higher energy and more disorder

89.

Which sample has the lowest entropy?

a)

1 mole of KNO3(l)

b)

1 mole of KNO3(s)

c)

1 mole of H2O(l)

d)

1 mole of H2O(g)

90.

Entropy increases from solid, liquid to gas. Why?

a)

Molecular disorder increases

b)

Molecules increase in number from solid to gas

c)

Molecules are heavier in solid

d)

Molecules are more reactive

91.

Which sample has the lowest entropy?

a)

1 mole of HNO3(aq)

b)

1 mole of KNO3(s)

c)

1 mole of H2O(l)

d)

1 mole of N2O(g)

92.

Which state of matter has the greatest motion and least orderly arrangement?

a)

solid

b)

liquid

c)

gas

d)

aqueous

93.

Which phase change represents a decrease in entropy?

a)

solid to liquid

b)

gas to liquid

c)

liquid to gas

d)

solid to gas

94.
Entropy always increases when
a)
enthalpy decreases.
b)
temperature decreases.
c)
temperature increases.
d)
volume increases.
95.

Given the change of phase:  CO2(g) →\rightarrow  CO2(s)

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

a)

decreases

b)

increases

c)

remains the same

96.

What phase of matter has the most entropy?

a)

solid

b)

liquid

c)

gas

97.

Entropy of a system increases when a reaction increases the number of particles.

a)

True

b)

False

98.

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

99.

Predict the entropy change for this reaction 

  N2O4(g)N_2O_4\left(g\right)   →  2NO2(g)2NO_2\left(g\right)   

a)

ΔS = +ve and non spontaneous

b)

ΔS = -ve and spontaneous

c)

ΔS = -ve and non spontaneous

d)

ΔS = +ve and spontaneous

100.

Which of the reactions below has a negative ∆S?

a)

CuCO3 (s) + 2HCl (aq) → CuCl2 (aq) + CO2 (g) + H2O (l)

b)

C (s) + O2 (g) → CO2 (g)

c)

CuO (s) + H2SO4 (aq) → CuSO4 (aq) + H2O (l)

d)

BaCl2 (aq) + Na2SO4 (aq) → BaSO4 (s) + 2NaCl (aq)

101.

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

102.

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.

103.

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.

104.

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.

105.

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.

106.

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

107.

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

108.

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

a)

0

b)

4

c)

8

109.

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

a)

1

b)

3

c)

5

110.

Which of the following situations demonstrates high entropy?

a)

water freezing

b)

water vaporizing

c)

steam condensing to water

111.

A spontaneous reaction is more profitable to a company.

a)

True

b)

False

112.
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
113.

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

114.

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

115.

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)

116.
Which phase of matter has the greatest motion and least orderly arrangement?
a)
solid
b)
liquid
c)
gas
117.

Which phase change represents a decrease in entropy?

a)

solid to liquid

b)

gas to liquid

c)

liquid to gas

d)

solid to gas

118.
Entropy always increases when
a)
enthalpy decreases.
b)
temperature decreases.
c)
temperature increases.
d)
volume increases.
119.

Entropy is a measure of

a)

accuracy

b)

precision

c)

the disorder of a system

d)

the attraction of a nucleus for an electron

120.

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

121.

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

122.

Entropy is a measure of

a)

heat energy

b)

temperature

c)

the disorder/randomness of a system

123.

A small S value indicates the system has _______

a)

more order

b)

more randomness

124.
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
125.
Which phase of matter has the greatest motion and least orderly arrangement?
a)
solid
b)
liquid
c)
gas
126.

Which process is accompanied by a decrease in entropy?

a)

boiling of water

b)

condensing of water vapor

c)

subliming of iodine

d)

melting of ice

127.

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

128.

Identify whether the following result in an increase or decrease in entropy:


3 moles of gas (on reactant side) --> 6 moles of gas (product)

a)

increase

b)

decrease

129.

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

130.

The average bond enthalpies for O-O and O=O are 146 and 496 kJ/mol respectively. What is the enthalpy change, in kJ, for the reaction below?

H-O-O-H(g) → H-O-H(g) + ½O=O(g)

a)

-102

b)

+102

c)

+350

d)

+394

131.

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

132.
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
133.

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

134.

The average bond enthalpies for O-O and O=O are 146 and 496 kJ/mol respectively. What is the enthalpy change, in kJ, for the reaction below?

H2O2(g) → H2O(g) + ½O2(g)

a)

-102

b)

+102

c)

+350

d)

+394

135.

Using the equations below:

C(s) + O2(g) → CO2(g) ∆H = –390 kJ

Mn(s) + O2(g) → MnO2(s) ∆H = –520 kJ

what is ∆H (in kJ) for the following reaction?

MnO2(s) + C(s) → Mn(s) + CO2(g)

a)

910

b)

130

c)

-130

d)

-910

136.

Using the equations below

Cu(s) + 1/2O2(g) → CuO(s) ∆H = –156 kJ

2Cu(s) + O2(g) → Cu2O(s) ∆H = –170 kJ

what is the value of ∆H (in kJ) for the following reaction?

2CuO(s) → Cu2O(s) + 1/2O2(g)

a)

142

b)

15

c)

-15

d)

-142

137.

Consider the following equations.

Mg(s) + O2(g) → MgO(s) ∆H = –602 kJ

H2(g) + O2(g) → H2O(g) ∆H = –242 kJ

What is the ∆H value (in kJ) for the following reaction?

MgO(s) + H2(g) → Mg(s) + H2O(g)

a)

-844

b)

-360

c)

+360

d)

+844

138.

The standard enthalpy change of formation values of two oxides of phosphorus are:

P4(s) + 3O2(g) → P4O6(s) ΔHf = –1600 kJ mol–1

P4(s) + 5O2(g) → P4O10(s) ΔHf = –3000 kJ mol–1

What is the enthalpy change, in kJ mol–1, for the reaction below?

P4O6(s) + 2O2(g) → P4O10(s)

a)

+4600

b)

+1400

c)

–1400

d)

–4600

139.

If N2 (g) + 2O2 (g) ⟶\longrightarrow   2NO2(g) has a ΔHrxn \Delta H_{rxn\ }  = 68, then what is the ΔHrxn\Delta H_{rxn}  if you reverse the reaction?

a)

86 kJ

b)

- 86 kJ

c)

68 kJ

d)

-68 kJ

140.
a)
-804.6
b)
-202.3
c)
-296.1
d)
-233.0
141.
What does the heat capacity of an object measure?
a)
the amount of energy required to change the temperature of an object
b)
the total amount of energy an object can store
c)
the thermal potential energy of the object
d)
the amount of work done by the object
e)
the amount of energy required to melt a solid object
142.
When applying the first law of thermodynamics to a system, when is heat a positive quantity?
a)
when the system does work
b)
when the system has work done on it
c)
when the system absorbs heat
d)
when the system loses heat
e)
when no work is done either on the system or by the system
143.
The product of the pressure and volume of a system  has the same SI units as which one of the following choices?
a)
force
b)
work
c)
acceleration
d)
momentum
e)
impulse
144.

25 °C in kelvins

a)

298.45 K

b)

248.15 K

c)

298.15 K

145.

Calculate the volumetric flow of a system feed by water with a mass flow of 3 kg/s.

a)

3000 kg/s

b)

0.003 kg/s

c)

3003 kg/s

146.

Calculate the heat transfer to the environment if the system produce a work of 45 kJ and receive 9 kJ in the way of heat. The enthalpy difference of the system is equal to 55 kJ.

a)

1

b)

91

c)

19

147.

A 7.50 liter sealed jar at 18 °C contains 0.125 moles of oxygen and 0.125 moles of nitrogen gas. What is the pressure in the container?

a)

7.38 atm

b)

0.796 atm

c)

0.684 atm

d)

0.398 atm

148.
What is 50 °C in Kelvin?
a)
223
b)
323
c)
100
d)
50
149.

What does R stand for

a)

Ideal gas constant

b)

Real gas constant

c)

Temperature constant

d)

Ideal gas law

150.

Which of the following equations represents the Ideal Gas Law?

a)
b)
c)
d)
151.
An ice cube is placed on a table and begins to melt.  The following conclusion can be made.
a)
Energy is being absorbed by the table which causes the cube to melt.
b)
Energy is being transferred from the table to the ice cube.
c)
Energy is being created by the air and table and making the cube heat up.
d)
Energy  is being created by the ice cube and is being released to the air
152.
A hot cup of tea absorbs thermal energy from a cold room.
a)
True
b)
False
153.
The _____ Law of Thermodynamics says that heat always flows from an object with a higher temperature to an object of lower temperature naturally
a)
Zeroth
b)
First
c)
Second
d)
Third
154.
Which law of thermodynamics states that absolute zero cannot be reached?
a)
1st
b)
2nd
c)
3rd
d)
Zeroth
155.
It is possible to reach absolute zero
a)
true
b)
false
156.
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
157.
Two cups of water, one at 100oC and the other at 50oC are poured into a larger container. What would be the final temperature of the water?
a)
Less than 50oC.
b)
Greater than 100oC.
c)
Between  50oC and 100oC.
d)
The water temperature will rise and fall continually.
158.
As water in a freezer turns into ice,
a)
the water absorbs energy from the air in the freezer.
b)
the water absorbs the coldness from the air in the freezer.
c)
the freezer air absorbs heat from the water.
d)
the water neither absorbs nor releases energy.
159.
What causes water to freeze solid when placed in a freezer? The freezer–
a)
adds heat to the water
b)
puts electricity in the water
c)
takes heat away from the water
d)
does not let light shine on the water
160.
As time progresses, Energy will naturally become more spread out.  It can only come together if you make it.
a)
Zeroth Law of Thermodynamics
b)
First Law of Thermodynamics
c)
Second Law of Thermodynamics
d)
Third Law of Thermodynamics
161.
What is thermodynamics?
a)
movement of heat
b)
it's magic
c)
measurement of heat
d)
none of them
162.
How many laws of thermodynamics are there?
a)
a lot
b)
3
c)
4
d)
1
163.
Energy is created by....
a)
running
b)
boiling ice
c)
touching slime
d)
none of them
164.
What is absolute zero?
a)
0 K
b)
273 K
c)
0oC
165.
Energy can be less than zero
a)
true
b)
false

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