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Thermochemistry Unit Review

Total questions: 74

Worksheet time: 3hrs 51mins

Name
Class
Date
1.
Describe the substance between letters A and B. 
a)
Solid
b)
Liquid
c)
Melting
d)
Evaporating
2.
Describe the substance between letters B and C. 
a)
Solid
b)
Liquid
c)
Melting
d)
Evaporating
3.
Describe the substance between letters C and D. 
a)
Gas
b)
Liquid
c)
Melting
d)
Evaporating
4.
Describe the substance between letters D and E. 
a)
Gas
b)
Liquid
c)
Melting
d)
Evaporating
5.
Describe the substance between letters E and F. 
a)
Gas
b)
Liquid
c)
Melting
d)
Evaporating
6.
Between which points is the temperature of the substance increasing?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
7.
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
8.
Between which points is heat not being added to the substance?
a)
Heat is always added
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
9.
Between which points is heat being added to the substance?
a)
Heat is always added
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
10.
Between which points is the substance changing its state of matter?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
11.
How many states of matter are present during line segment AB?
a)
One
b)
Two
c)
Three
d)
Depends on the temperature
12.
How many states of matter are present during line segment BC?
a)
One
b)
Two
c)
Three
d)
Depends on the temperature
13.
How many states of matter are present during line segment CD?
a)
One
b)
Two
c)
Three
d)
Depends on the temperature
14.
How many states of matter are present during line segment DE?
a)
One
b)
Two
c)
Three
d)
Depends on the temperature
15.
How many states of matter are present during line segment EF?
a)
One
b)
Two
c)
Three
d)
Depends on the temperature
16.
Which segment represents the heat of fusion?
a)
A-B
b)
B-C
c)
C-D
d)
D-E
17.
Which process takes the longest to occur?
a)
melting
b)
boiling
c)
freezing
d)
heating the solid
18.
What state(s) of matter are present at D-E?
a)
Solid-liquid
b)
Liquid
c)
Liquid-gas
d)
Gas-Solid
19.
True or false: melting and freezing occur at the same temperature.
a)
True
b)
False
20.
What state of matter is present at segment 5?
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
21.
What phase change occurs at D-E?
a)
melting
b)
condensing
c)
boiling
d)
freezing
22.
What state(s) of matter are present at D-E?
a)
Solid-liquid
b)
Liquid
c)
Liquid-gas
d)
Gas-Solid
23.
Which segment represents the heat of vaporization?
a)
E-F
b)
B-C
c)
C-D
d)
D-E
24.
Which of these conditions is always true for an exothermic process?
a)
They leave the surroundings feeling cold
b)
They release energy into the surroundings.
c)
They absorb energy from the surroundings
d)
The reactants gain energy as they form the products
25.
What type of process is happening as one moves along line segment B toward the right?
a)
An endothermic Process
b)
An exothermic Process
c)
The calorimetry process
d)
Nuclear fusion
26.
Looking at the heating curve above, What is occurring at letter B?
a)
Ice is melting to form liquid water.
b)
Liquid water is becoming warmer.
c)
Liquid water is boiling to form steam.
d)
Steam is becoming warmer
27.
What is occurring during the portion of the heating curve labeled C?
a)
Ice is melting to form liquid water
b)
Liquid water is becoming warmer.
c)
Liquid water is boiling to form steam.
d)
Steam is becoming warmer.
28.
Analyze this statement: Melting and freezing occurs at the same temperature.
a)
True
b)
False
c)
Depends on the material
d)
Depends on experimental conditions
29.
From 30 degrees to 55 degrees, what state(s) of matter is the substance?
a)
Solid
b)
Liquid
c)
Gas
d)
Plasma
30.
This type of graph is called a:
a)
Phase diagram
b)
Heating curve
c)
State of matter
d)
Temperature chart
31.
Chemical reactions that absorb energy are called
a)
endothermic
b)
fast
c)
slow
d)
exothermic
32.
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 .10 J/g°C, what is the mass of the iron sample?
a)
25g
b)
30g
c)
20g
d)
50g
33.
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? (show your work)
a)
2.34 J/g°C
b)
0.472 J/g°C
c)
6.13 J/g°C
d)
0.163 J/g°C
34.
H2 + 2 C + N2 + 270.3 kJ --> 2 HCN
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
35.
What letter represents boiling?
a)
B
b)
C
c)
D
d)
E
36.
What letter represents a liquid being heated?
a)
A
b)
B
c)
C
d)
D
37.
How much energy does it take to freeze 39.2 g of liquid benzene (C6H6)?  (ΔHfus = 9.08 kJ/mol, ΔHvap = 28.4 kJ/mol)  (Show your work)
a)
4.940 kJ
b)
-4.940 kJ
c)
258 kJ
d)
-258 kJ
38.
Will H be positive or negative in this reaction?
a)
positive
b)
negative
39.
If ΔH is positive, heat would be shown on the _____ side of the thermochemical equation.
a)
Reactant
b)
Product
40.
Water exists as a _____________ at 700 mmHg and 50 °C.
a)
solid
b)
liquid
c)
gas
d)
supercritical fluid
41.
What change occurs from C to D?
a)
condensation
b)
vaporization
c)
melting
d)
sublimation
42.
What is the normal boiling point of this substance?
a)
150 °C
b)
100 °C
c)
-50 °C
d)
0 °C
43.
At 10 atm, dry ice is heated from -100 °C to 30 °C.  What changes occur?
a)
freezing, then condensation
b)
melting only
c)
sublimation only
d)
melting, then boiling
44.

The branch of chemistry that studies the heat transfers that accompany chemical or physical changes is ________________.

a)

thermochemistry

b)

organic

c)

inorganic

d)

physical

45.

Also called the law of ________ of energy, the first law of thermodynamics states that the total amount of energy in a thermodynamic system remains constant.

a)

entropy

b)

conservation

c)

creation

d)

generation

46.

The total amount of energy in a thermodynamic system is called ___________.

a)

conservation

b)

entropy

c)

generation

d)

enthalpy

47.

The measurement of enthalpy changes caused by chemical reactions, changes of state, or the formation of a solution is called ___________.

a)

calorimetry

b)

thermochemistry

c)

thermodynamics

d)

analytics

48.

What is the symbol for Specific Heat

a)

q

b)

t

c)

m

d)

c

49.

What is the equation to measure change in Heat Energy?

a)

q=mc∆t

b)

q=mc

c)

q= ∆mct

d)

m=qCc

50.
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
51.
How does heat flow?
a)
Always from cold to warm
b)
Always from warm to cold
c)
Both warm to cold & cold to warm
d)
It depends on the temperature
52.

The specific heat of platinum is 0.133 J/g°C. How much heat(q) 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

53.
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
54.
In an exothermic reaction, heat is ...
a)
taken in or absorbed
b)
given out or released
55.

2H2 + O2 --> 2H2O + 570 kJ is an example of a(n)

a)

Electrical equation

b)

Heat equation

c)

Thermochemical equation

56.

C+ O2 --> CO2 + 60kJ, what is the value for ΔH for the reaction?

a)

+60 kJ

b)

-60 kJ

c)

there is no way to know

57.

A reaction that causes the temperature of the surrounding to drop is

a)

endothermic

b)

exothermic

c)

displacement

d)

oxidation

58.

4NO + 6H2O + 1170 kJ --> 4NH3 + 5 O2


What is the ΔH of this reaction if 13.1 grams of NO reacts with water?

a)

100 kJ

b)

1.27 kJ

c)

128 kJ

d)

0.32 kJ

59.

When a reaction requires energy in order to be completed, this energy can be written on the ___ side of the equation

a)

Left

b)

Right

60.

The heat content of a substance

a)

Enthalpy

b)

Energy

c)

Specific Heat

d)

Calorimeter

61.

Describes the additive nature of chemical equations and heat changes

a)

Hess's Law

b)

Law of Conservation of Energy

c)

Specific Heat

d)

Thermochemistry

62.

The heat absorbed by 1 mole of a substance in boiling from a liquid to a gas at constant temperature

a)

deltaHvap

b)

deltaHfus

c)

specific heat

d)

enthalpy

63.

The fact that equal masses of both water and copper, when supplied with identical energy amounts of energy heat up at different rates is due to their ___.

a)

specific heat

b)

enthalpy

c)

deltaHvap

d)

deltaHfus

64.

Convert 475 J to cal

a)

114 cal

b)

1990 cal

c)

0.475 cal

d)

475,000 cal

65.

Convert 1420 J to kJ

a)

1.42 kJ

b)

1,420,000 kJ

c)

339 kJ

d)

5940 kJ

66.

Convert 10.1 kcal to J

a)

42,300 J

b)

0.0423 J

c)

42.3 J

d)

2410 J

67.

What is the specific heat of liquid water?

a)

4.184 J/gC

b)

1.84 J/gC

c)

2.01 J/gC

d)

2.02 J/gC

68.

How much heat (in joules) is needed to raise the temperature of 355 g of ethanol (c = 2.4 J/goC) by 63oC?

a)

54,000 J

b)

94,000 J

c)

22,000 J

d)

852 J

69.

What mass of iron (c = 0.11 cal/goC) would need 875 cal of energy in order to raise its temperature by 3.5oC?

a)

2300 g

b)

340 g

c)

28 g

d)

28,000 g

70.

What is the final temperature of a sample of magnesium (c = 0.24 cal/goC), if 1835 cal is added to 612 g of magnesium at an initial temperature of 19.3oC?

a)

31 C

b)

5200 C

c)

12 C

d)

19.3 C

71.

How many moles of water are produced from the following reaction, when 275 kJ of energy is given off?

4 NH3 + 3 O2 --> 2 N2 + 6 H2O ΔH = -1530 kJ

a)

1.08 mol H2O

b)

1300 mol H2O

c)

1700 mol H2O

d)

70,000 mol H2O

72.

How much energy is produced when 93.5 grams of oxygen reacts with 13.2 g hydrogen in the following reaction?

2 H2 + O2 --> 2 H2O ΔH = -572 kJ

a)

-1670 kJ produced

b)

-1870 kJ produced

c)

-419 kJ produced

d)

-835 kJ produced

73.

Calculate the ΔH for the following reaction:

a)

-333.3 kJ

b)

-298.9 kJ

c)

- 482.8 kJ

d)

-149.3 kJ

74.

Calculate the ΔH for the following reaction:

a)

+ 5.1 kJ

b)

-512 kJ

c)

-1638 kJ

d)

-2,201 kJ

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