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WorksheetsThermochemistry Review Game
Total questions: 55
Worksheet time: 1hrs 23mins
Name
Class
Date
1.
Device that accurately measures energy changes during a chemical process.
a)
thermometer
b)
calorimeter
c)
barometer
d)
anemometer
2.
Energy stored in a substance because of its composition
a)
kinetic energy
b)
potential energy
c)
thermal energy
d)
chemical energy
3.
Phase change from gas to liquid
a)
sublimation
b)
condensation
c)
vaporization
d)
freezing
4.
Heat transfer through direct contact
a)
conduction
b)
convection
c)
radiation
d)
thermal
5.
Heat transfer through liquids or gases
a)
conduction
b)
convection
c)
radiation
d)
thermal
6.
Phase change from solid to gas
a)
endothermic
b)
exothermic
7.
Amount of energy required to increase the temperature of 1 g of a substance by 1'C
a)
joules
b)
specific heat
c)
Calorie
d)
calorie
8.
What type of heat transfer is shown in this picture?
a)
radiation
b)
convection
c)
conduction
d)
solar
9.
What type of heat transfer is shown in the picture?
a)
radiation
b)
conduction
c)
convection
10.
Phase change from solid to liquid
a)
melting
b)
condensation
c)
vaporization
d)
sublimation
11.
A process that releases heat to its surroundings
a)
endothermic
b)
exothermic
c)
radiation
d)
heat transfer
12.
What type of reaction is shown in the picture?
a)
endothermic
b)
exothermic
c)
potential energy
d)
kinetic energy
13.
If there is an increase in H, why would this reaction feel cold to your hand?
a)
energy is absorbed from surroundings
b)
energy is released into surroundings
c)
heat moves from colder to warmer objects
d)
it would not feel colder
14.
Will H be positive or negative in this reaction?
a)
positive
b)
negative
15.
124 joules of heat are added to a piece of lead (specific heat = 0.128 J/goC). It is heated to 100.0oC, and then lowered into a calorimeter filled with water. The lead’s temperature decreases to 28.8oC. What is the mass?
a)
150 g
b)
13.6 g
c)
4 g
d)
1130 g
16.
What is the specific heat capacity of silver metal if 55 grams of the metal absorbs 47.3 joules of heat and the temperature rises 15 degrees Celcius?
a)
0.033 J/gC
b)
0.057 J/gC
c)
39000 J/gC
d)
.0455 J/gC
17.
Amount of energy required to increase the temperatureof 1 g of water by 1"C
a)
calorie
b)
joule
c)
Calorie
d)
kcal
18.
Which of the letters (A-D) represents the potential energy of the reactants?
a)
A
b)
B
c)
C
d)
D
19.
Which of the letters (A-D) represents the potential energy of the products?
a)
A
b)
B
c)
C
d)
D
20.
What kind of reaction has a negative heat of reaction (ΔHr)?
a)
endothermic
b)
exothermic
21.
What kind of reaction is this?
a)
endothermic
b)
exothermic
22.
A process that absorbs heat is a(n) _______________ reaction?
a)
polythermic
b)
ergothermic
c)
exothermic
d)
endothermic
23.
Consider the reaction: 2 H2O + energy --> 2H2 + O2
a)
exothermic, releasing energy
b)
exothermic, absorbing energy
c)
endothermic, absorbing energy
d)
endothermic, releasing energy
24.
The minimum amount of energy needed to start a reaction is called the?
a)
surface energy
b)
activation energy
c)
concentration
d)
catalyst
25.
Exothermic reactions are reactions that
a)
release heat
b)
do not involve heat
c)
absorb heat
d)
take place instantaneously
26.
Which of the following is an endothermic process?
a)
solid to gas
b)
liquid to solid
c)
solid to liquid
d)
gas to liquid
27.
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
28.
What kind of reaction has a positive heat of reaction (ΔHr)?
a)
endothermic
b)
exothermic
29.
The movement of thermal energy from one thing to another.
a)
Heat transfer
b)
Potential energy
c)
Law of conservation
d)
Specific heat
30.
Energy can neither be created nor destroyed; only transformed from one form to another.
a)
First Law of Thermodynamics
b)
Second Law of Thermodynamics
c)
Third Law of Thermodynamics
d)
Law of Conservation of Matter
31.
In this type of system heat or energy flows out:
a)
Specific Heat
b)
Heat
c)
Endothermic
d)
Exothermic
32.
Calculate delta T if a system's temperature decreases from 50 degrees Celsius to 18 degrees Celsius.
a)
50
b)
68
c)
-32
d)
32
33.
Determine the energy (in kJ) required to raise the temperature of 100.0 g of water from 20.0 C to 85.0 C? The specific heat of water is 4.184 J/(gxC)
a)
5kJ
b)
4,182 J
c)
27,196 J
d)
27.20kJ
34.
How much energy would be needed to heat 450 grams of copper metal from a temperature of 25.0ºC to a temperature of 75.0ºC? (The specific heat of copper at 25.0ºC is 0.385 J/g ºC.)
a)
4,000 J
b)
8,700 J
c)
5,000 J
d)
3,578 J
35.
For the formula:
Q= m c ∆T
The units for specific heat are:
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
36.
What is the specific heat, c, (J/g·oC) of a substance if 51 J of heat are required to raise the temperature of 1.7 grams of this substance from 20.5 ºC to 25.5 ºC?
a)
- 433.5 J/g·oC
b)
6 J/g·oC
c)
-6 J/g·oC
d)
433.5 J/g·oC
37.
A 16.0 g sample of
iron was heated from 0°C to 35.0°C. It absorbed 246.4 J of energy as heat. What
is the specific heat of this piece of iron?
a)
240 J/g°C
b)
3.67 J/g°C
c)
1.34 J/g°C
d)
0.44 J/g°C
38.
Heat flows from
a)
cold to hot
b)
warm to cold
c)
freezing to boiling
d)
hot to cold
39.
How much heat is
required to raise the temperature of a sample of copper from 10.0°C to 55.0°C,
if its specific heat is 0.384 J/g°C and its mass is 10.00 g?
a)
16 J
b)
139 J
c)
173 J
d)
359 J
40.
If ΔH = -95 J
Then...
Then...
a)
The system is losing 95 J to the surroundings
b)
Both the system and surroundings are losing 95 J
c)
The system is gaining 95 J from the surroundings
d)
Both the system and surroundings are gaining 95 J
41.
H2 + 2 C + N2 + 270.3 kJ --> 2 HCN
Is this reaction endothermic or exothermic?
Is this reaction endothermic or exothermic?
a)
Endothermic
b)
Exothermic
42.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
43.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
44.
Refer the the following question:
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
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
45.
What mass of P4 must be reacted to produce 5905 kJ of energy?
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
a)
25.43 g
b)
563.0 g
c)
2.421 g
d)
300.0 g
46.
H2 + Cl2 --> 2 HCl + 1845 kJ
Is this reaction endothermic or exothermic?
Is this reaction endothermic or exothermic?
a)
Endothermic
b)
Exothermic
47.
Consider the reaction: 2 H2O + energy --> 2H2 + O2
a)
exothermic, releasing energy
b)
exothermic, absorbing energy
c)
endothermic, absorbing energy
d)
endothermic, releasing energy
48.
How many grams of water would require 2200 joules of heat to raise its temperature from 34°C to 100°C? The specific heat of water is 4.18 J/g∙C
a)
.125 g
b)
34,736 g
c)
7.97 g
d)
1.99 g
49.
How much energy must be used to produce 4.75 mol of gaseous water?
H2O (l) + 44.0 kJ --> H2O (g)
H2O (l) + 44.0 kJ --> H2O (g)
a)
209 kJ
b)
9.36 kJ
c)
206.8 kJ
d)
9.362 kJ
50.
When you dropped a hot metal sample into room temperature water in the lab what happened?
a)
the heat from the metal traveled into the water
b)
the cool from the water traveled into the hot metal
c)
both of the other answers are correct
51.
H2 + ½ O2 --> H2O + 285kJ is an example of a(n)
a)
Electrical equation
b)
Heat equation
c)
Thermochemical equation
52.
If ΔH is positive, heat would be shown on the _____ side of the thermochemical equation.
a)
Reactant
b)
Product
53.
A 24.0 gram sample of copper was heated from 25.0oC to 500.0oC, 4378J of heat were absorbed, what is the specific heat of copper?
a)
.384
b)
49909200
c)
2.60
d)
8.77
54.
As someone is running on the track they begin to perspire. This is an example of an
a)
endothermic process
b)
exothermic process
55.
1.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
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