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Thermo Review #2

Total questions: 67

Worksheet time: 1hrs 6mins

Name
Class
Date
1.

Do molecules generally move faster at 45oC or 106oC?

a)

45oC because molecules have more energy than in 106oC

b)

106oC because molecules have more energy than in 45oC

c)

106oC because molecules have less energy than in 45oC

d)

45oC because molecules have less energy than in 106oC

2.

Frying an egg on a skillet. Referring to the egg, would the enthalpy change be positive or negative?

a)

Skillet is absorbing heat energy from the egg. Absorbing energy is Endothermic. Endothermic has a positive Enthalpy

b)

Egg absorbing heat energy from the skillet. Absorbing energy is Endothermic. Endothermic has a positive Enthalpy

c)

Egg absorbing heat energy from the skillet. Releasing energy is Exothermic. Exothermic has a positive Enthalpy

d)

Egg absorbing heat energy from the skillet. Releasing energy is Exothermic. Exothermic has a negative Enthalpy

3.

Define ΔH

a)

Change in Specific Heat; Heat by one Degree Celsius

b)

Change in Temperature; the energy we calculate; Degree Celsius

c)

Change in Enthalpy; the energy/heat we calculate

d)

Change in Time; time travel

4.

Specific Heat is..

a)

the temperature initial minus temperature final

b)

the amount of heat/energy required to raise 1 gram of a substance by 1°C (or K) aka "C"

c)

the temperature final minus temperature initial

d)

the item in a system with given weight in grams

5.

How much energy is needed to raise the temperature of a 20.0-g piece of copper from 15.0oC to 25.0oC? The specific heat of copper is 0.385 J/goC. 

a)

-62.0 J

b)

77.0 J

c)

62.0 J

d)

-77.0 J

6.

Is the phase change representing an exothermic or endothermic reaction?

SOLID to LIQUID

a)

Endothermic

b)

Exothermic

7.

Is the reaction exothermic or endothermic?

H2 + S + O2 -> H2SO4 ΔH = -811.13kJ

a)

ΔH is negative so it is exothermic

b)

ΔH is positive so it is exothermic

c)

ΔH is positive so it is endothermic

d)

ΔH is negative so it is endothermic

8.
The diagram represents which type of reaction
a)
endothermic
b)
exothermic
9.
H2 + 2 C + N2 + 270.3 kJ --> 2 HCN
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
10.
What does temperature measure?
a)
Heat of Molecules
b)
ºC
c)
Average Kinetic Energy of Molecules
d)
Thermal Energy
11.
What is the symbol for Thermal Energy in the specific heat formula?
a)
Q
b)
t
c)
m
d)
C
12.
The specific heat of aluminum is 0.21 cal/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)
50 J
13.

The diagram shows a heating curve for ice. Which line represents the ice melting?

a)

A

b)

B

c)

C

d)

D

e)

E

14.

How many equations would need to be added together to move ice at -15.0oC to room-temperature water at 21.0oC?

a)

1

b)

2

c)

3

d)

4

15.

The diagram shows a heating curve for ice. Which line would require the use of the equation q=nΔHovap?

a)

A

b)

B

c)

C

d)

D

e)

E

16.

Water has a specific heat of 4184 J/kgºC.  Wood has a specific heat of 1760 J/kgºC.  What material needs more energy to raise the temperature 1ºC (a)  

Choose from the below words
Wood
Water
Both are the same
17.
A high specific heat means...
a)

it requires more energy to change temperature

b)

it requires less energy to change temperature

18.

Which will heat up the fastest? (a)  

Choose from the below words
copper
granite
iron
basalt
19.

Heat will always transfer from the ___________ object to the ________ object.

a)

The hottest object to the coolest object.

b)

The coolest object to the hottest object.

c)

The solid object to the liquid object.

d)

The liquid object to the solid object.

20.
The flow of thermal energy from warmer objects to cooler objects 
a)

Thermal energy

b)

Temperature

c)

Heat

d)

Convection 

21.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
22.
The temperature of a substance increases as___.
a)
the substance expands
b)
the average kinetic energy of its particles increases
c)
the substance's volume increases
d)
the substance's mass increases
23.

Which one has more thermal energy?

a)

an ice cube in a glass of lemonade

b)

a bathtub full of warm water

c)

a pot of soup boiling on the stove

d)

a cup of hot coffee

24.

What happens if I add ice cubes to a glass of soda

a)

The heat transfers from the coke to the ice

b)

The cold transfers from the ice to the coke

25.

The equation for cellular respiration is shown:

C6H12O6 + 6O2 --> 6CO2 + 6H2O + heat

What can be concluded about the heat energy in the reaction?

a)

The reaction absorbs heat and is, therefore, endothermic.

b)

The reaction absorbs heat and is, therefore, exothermic.

c)

The reaction releases heat and is, therefore, exothermic.

d)

The reaction releases heat and is, therefore, endothermic.

26.

The specific heat of platinum is 0.133 J/g°C. How much heat(Q) is absorbed when a 10 g piece of platinum warms from 100°C to 150°C?

a)

66.5 J

b)

0.0266 J

c)

665 J

d)

0.665 J

27.

Calculate ΔH for the process

Zn (s) + S (s) + 2O2 (g) → ZnSO4 (s)

from the following information:

Zn (s) + S (s) → ZnS (s)    ΔH = – 206.0 kJ

ZnS (s) + 2 O2 (g) → ZnSO4 (s)     ΔH= – 776.8 kJ

a)

570.8 kJ

b)

-570.8 kJ

c)

-982.8 kJ

d)

982.8 kJ

28.

Students are trying to calculate the heat of reaction for the following overall reaction.

4A + 5B → C + 3D 

They find the heat of reactions for the two reactions as shown. 

2A + 2B → C + 2D ΔH= -100 kJ  

2A +3B → D ΔH= 65 kJ 

a)

-35 kJ

b)

-165 kJ

c)

35 kJ

d)

165 kJ

29.

Ammonium nitrate and sodium chloride are each combined with water to make two solutions. The initial and final temperatures of the water are recorded in the table to the left. Based on the data, which is a true statement(s)?

a)

Dissolving ammonium nitrate is endothermic

b)

Dissolving sodium chloride is exothermic

c)

Dissolving ammonium nitrate is exothermic

d)

Dissolving sodium cloride is endothermic

30.

Select all which are endothermic...

a)

H2O(L)-->H2O(g)

b)

H2O(s)-->H2O(L)

c)

H2O(g)-->H2O(L)

d)

H2O(L)-->H2O(s)

31.

Use the graphs to help answer:

In an exothermic reaction, which has more potential energy?

a)

neither

b)

products

c)

reactants

d)

both are equal

32.

.


A hot piece of metal is placed into cooler water. Which statement describes how the second law of thermodynamics relates to this process?

a)

The temperature change of the metal is equal to the temperature change of the water.

b)

The amount of energy lost by the metal is equal to the amount of energy gained by the water.

c)

Energy flows from the metal to the water until they are at the same temperature.

d)

Energy flows from the water to the metal until they are at the same temperature.

33.

The diagram above represents the reaction X2 + Y2 --> 2XY. Which statement describes this reaction?

a)

It is endothermic and energy is absorbed.

b)

It is endothermic and energy is released.

c)

It is exothermic and energy is absorbed.

d)

It is exothermic and energy is released.

34.

Calculate the heat of reaction.

a)

0 KJ

b)

100 KJ

c)

130 KJ

d)

50 KJ

35.

Which letter represents the Activation Energy?

a)

a

b)

b

c)

c

d)

d

36.

Which letter represents the potential energy of the reactants?

a)

a

b)

b

c)

c

d)

d

37.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

38.

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

a)

Product

b)

Reactant

39.

Define the term Exothermic by picking the correct statements. (Choose 3)

a)

Products have less energy than the reactants

b)

ΔH is negative

c)

ΔH is positive

d)

Energy is given out to the surroundings (temperature goes up).

e)

products have more energy than the reactants

40.

Define Endothermic by picking the correct statements. (Choose 3)

a)

ΔH is positive

b)

Energy is taken in from the surroundings (temperature goes down).

c)

Energy is given out to the surroundings (temperature goes up).

d)

· Products have less energy than the reactants

e)

products have more energy than the reactants

41.

Based on the information in the table above, which of the following expressions gives the approximate ΔH° for the reaction represented by the following balanced chemical equation?

Fe2O3(s)+3 CO(g)→2 Fe(s)+3 CO2(g)

a)

ΔH°rxn=[(0kJ/mol)+(−394kJ/mol)]−[(−826kJ/mol)+(−111kJ/mol)]

b)

ΔH°rxn=[2(0kJ/mol)+ 3(−394kJ/mol)]−[(−826kJ/mol)+ 3(−111kJ/mol)]

c)

ΔH°rxn=[(−826kJ/mol)+ 3(−111kJ/mol)]−[2(0kJ/mol)+ 3(−394kJ/mol)]

d)

ΔH°rxn=[(−826kJ/mol)+(−111kJ/mol)]−[(0kJ/mol)+(−394kJ/mol)]

42.

Calculate the enthalpy of reaction (ΔH).

4CO2 (g) + 6H2O (g) → 2C2H6 (g) + 7O2 (g)


ΔHfo [CO2(g)] = -393.5 kJ

ΔHfo [H2O(g)] = -241.8 kJ

ΔHfo [C2H6(g)] = -84.7 kJ

a)

550.647 KJ/mol

b)

2855.584 KJ/mol

c)

-550.647 KJ/mol

d)

-2855.584 KJ/mol

43.

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

44.

4 NH3 (g) + 5 O2 (g) ⟶ 4 NO (g) + 6 H2O (g)

Using the following information, calculate ΔH for the reaction shown above:

N2 (g) + O2 (g) ⟶ 2 NO (g) ΔH = -180.5 kJ

N2 (g) + 3 H2 (g) ⟶ 2 NH3 (g) ΔH = -91.8 kJ

2 H2 (g) + O2 (g) ⟶ 2 H2O (g) ΔH = -483.6 kJ

a)

256.0 kJ

b)

-1628.2 kJ

c)

-6387 kJ

d)

None of these

45.

The enthalpy of reactions for the synthesis 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

46.
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
47.
What mass of P4 must be reacted to produce 5905 kJ of energy?
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
a)
25.43 g
b)
563.0 g
c)
2.421 g
d)
300.0 g
48.

NaCl was heated starting at an initial temperature of 0°C. The heating curve is shown in the picture. What is the melting point of this substance?

a)

0°C

b)

801°C

c)

1000°C

d)

1465°C

49.
Between which points is the temperature of the substance remaining constant?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
50.

Which section has the lowest energy?

A
B
C
51.

The graph shows the heating curves for benzene and water.

Which substance has a higher boiling point?

a)

benzene

b)

water

52.
Endothermic reactions feel
a)
warm
b)
cold
53.

A reaction that gives out energy to the surroundings causes the temperature of the surroundings to

a)

increase

b)

decrease

c)

remain constant

54.

What is the term for the amount of energy gained or released in a chemical reaction?

a)

enthalpy of vaporization

b)

enthalpy of condensation

c)

enthalpy of reaction

d)

enthalpy of sublimation

55.
Change from gas to liquid...
a)
condensation
b)
evaporation
c)
expansion
d)
movement
56.
Refer to 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
57.
Calculate ΔH when 4.72 g of carbon reacts with excess oxygen, according to the following equation?
C + O2 → CO2 
ΔH = -393.5 kJ
a)
-154.8 kJ
b)
-95.0 kJ
c)
-66.7 kJ
d)
-199.5 kJ
58.

When 26 g of a metal at 90 ◦C is added to 46 g of water at 22 ◦C, the temperature of the water rises to 26.5 ◦C. What is the specific heat capacity of the metal? Assume no heat was lost to the surroundings.

a)

0.525J/g◦C

b)

4.18J/g◦C

c)

0.148J/g◦C

d)

2.47J/g◦C

59.
Calculate the standard reaction enthalpy for the reaction shown provided the enthalpies of reaction for the subsequent reactions.
a)
+412.1kJ/mol
b)
+206.1kJ/mol
c)
+42.0kJ/mol
d)
+155.5kJ/mol
60.

What is the total energy required to raise the temperature of 135 g of water from 22.0°C to 133.0°C?

a)

358,100 J

b)

44,100 J

c)

53,450 J

d)

335,100 J

61.

When carbon disulfide (CS₂) is formed, heat is absorbed. How much heat is absorbed when 5.66 g of carbon disulfide is formed?

C(s) + 2S(s) → CS₂(l), ΔH=89.3 kJ

a)

89.3 kJ

b)

54.9 kJ

c)

37.5 kJ

d)

6.61 kJ

62.

How many equations need to be added together to determine how much heat must be absorbed to bring 50.0 g of water to a boil if it starts at 21.0oC?

a)

1

b)

2

c)

3

d)

4

63.

Which enthalpy change is equal and opposite to the heat of fusion?

a)

heat of combustion

b)

heat of reaction

c)

heat of solidification

d)

heat of vaporization

64.

The heat of combustion is the amount of heat required to burn _____ of a substance

a)

1 mole

b)

1 gram

c)

1 kilogram

d)

25 grams

65.

Which formula represents the calculation of specific heat capacity?

a)

c=mQΔTc = \frac{m}{Q \Delta T}

b)

c=Qm+ΔTc = \frac{Q}{m + \Delta T}

c)

c=QmΔTc = \frac{Q}{m \Delta T}

d)

c=mQΔTc = m Q \Delta T

66.

How is temperature related to heat?

a)

Temperature is a measure of the heat of an object.

b)

Heat causes a change in the temperature of an object.

c)

Raising the temperature causes the heat of an object to increase.

d)

Temperature and heat are two different ways to measure the same thing.

67.

In thermodynamics, what does the first law state?

a)

Energy cannot be created or destroyed, only transformed.

b)

Entropy of an isolated system always increases.

c)

Heat cannot spontaneously flow from a colder location to a hotter location.

d)

The total energy of a system and its surroundings is constant.

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