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Thermochemistry Review

Total questions: 55

Worksheet time: 2hrs 36mins

Name
Class
Date
1.
The specific heat of aluminum is 0.21 J/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)

105 J

c)
1.05 J
d)
0.105 J
2.

20 g of water. specific heat of water is 4.18 J/g°C.  temperature changes from 20° C to 25° C, how much heat energy (q) moves from the water to the surroundings?

a)

  • 418 J

b)
210 J
c)
80 J
d)
4.18 J
3.
What does temperature measure?
a)
Heat
b)
ºC
c)
Kinetic Energy
d)
Thermal Energy
4.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
5.
For an endothermic reaction, the heat is on the ____ side.
a)
reactant
b)
product
c)
either side
6.
For an exothermic reaction, the heat is on the ____ side
a)
reactant
b)
product
c)
either side
7.
What type of reaction is shown in the picture?
a)
endothermic
b)
exothermic
8.
In an exothermic process, the surroundings are are gaining energy.
a)
True
b)
False
9.
If two objects have different temperatures, 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
10.

___________________ is the capacity to do work or supply heat.

a)

energy

b)

heat changes

c)

specific heat

d)

thermochemistry

11.

Ice cream melting is an example of an __________ process. (heat enters the system from the surroundings)

a)

endothermic

b)

exothermic

12.

Sweating is an __________________ process because heat is released.

a)

endothermic

b)

exothermic

13.

what does c stand for?

a)

heat capacity

b)

specific heat

c)

mass

d)

temperature

14.

Mass must always be in ________ for energy calculations.

a)

kilograms

b)

grams

c)

joules

d)

calories

15.

What is the specific heat of water?

a)

4.184 J/gC

b)

1.00 cal/gC

c)

All of the above

d)

none of the above

16.

When heat flows from system to the surroundings that is an example of an ________________ process.

a)

exothermic

b)

endothermic

17.

What device is used to measure the amount of heat involved in a chemical reaction or physical process?

a)

barometer

b)

calorimeter

c)

thermometer

18.

Kinetic energy is energy gained _______________

a)

while at rest

b)

during motion

19.

What is calorimetry?

a)

process of measuring kinetic and potential energy

b)

process of measuring heat flow of chemical reactions

c)

process of measuring pressure and temperature of a substance

20.

Heat flows from _______ to _________.

a)

warm to cool

b)

cool to warm

21.

What area of study in chemistry is concerned with the heat transfers that occur during chemical reactions?

a)

stoichiometry

b)

thermochemistry

c)

inorganic chemistry

d)

physical chemistry

22.

The specific heat of a substance varies with the mass of a sample. True or False?

a)

True

b)

False

23.

1 calorie = _______ Joules

a)

1000

b)

1

c)

500

d)

4.184

24.

Samples of two different substances having the same mass always have the same heat capacity. True or False?

a)

True

b)

False

25.

The unit for q (heat energy) can be in joules or calories. True or false?

a)

true

b)

false

26.

The law of conservation of energy states that

a)

in any chemical or physical change, energy cannot be created or destroyed, only changed in form.

b)

heat changes occur during chemical and physical changes.

c)

energy is the capacity to do work or to supply heat

d)

there are two types of energy, kinetic and potential

27.

1000 calories = ____ kcal

a)

10

b)

100

c)

1

d)

1000

28.

In energy calculations, temperature must be in which unit?

a)

Fahrenheit

b)

Kelvin

c)

Celsius

29.

How can you find the change in temperature?

a)


Tfinal + TinitalT_{final}\ +\ T_{inital}

b)

Tfinal − TinitialT_{final}\ -\ T_{initial}

c)

none of the above

30.

What is thermochemistry?

a)

study of heat changes that occur during a chemical reaction & physical changes of state

b)

the study of heat and chemistry

c)

the study of heat

d)

the study of chemistry

31.

When you add heat energy...

a)

Temperatures increase

b)

Molecules move slower

c)

Molecules move faster

d)

Temperatures decrease

32.

How does heat move?

a)

From cold to hot

b)

From hot to cold

33.

What is chemical potential energy?

a)

Energy from chemicals

b)

Energy to make chemicals

c)

Energy stored in chemical bonds

d)

Energy from the sky

34.

When a hot object and a cold object come together, heat will move from the warmer one to the colder one until they are the same temperature. What is this called?

a)

Equal

b)

Equilibrium

c)

Equality

35.

What is temperature?

a)

a measure of cold

b)

a measure of heat

c)

a measure of how something feels

36.

Match the following

a)

Q

1.

heat

b)

M

2.

mass

c)

C

3.

specific heat

d)

ΔT\Delta T

4.

change in temperature

37.

Calorimetry is...

a)

A method of measuring temperature

b)

A technique used to measure the amount of energy released or absorbed

c)

accurate and precise measurement of heat change for chemical and physical processes

d)

A method of measuring the amount of energy in a system

38.

Match the following

a)

Jg ∘C or calg ∘C\frac{J}{g\ \circ C}\ or\ \frac{cal}{g\ \circ C}

1.

c

b)

g or kg

2.

m

c)

ΔT\Delta T

3.

C or K

d)

c

4.

J or cal, kJ or Kcal

39.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

40.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

41.

What does q stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

42.

What does c stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

43.

What does ΔT\Delta T   stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

44.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
45.

What are chemical reactions that absorb energy?

a)

endothermic

b)

fast

c)

slow

d)

exothermic

46.

What is the study of heat changes that accompany chemical reactions and phase changes?

a)

energy

b)

chemistry

c)

work

d)

thermochemistry

47.

Consider the reaction: 2 H2O + energy --> 2H2 + O2

a)

exothermic because releasing energy

b)

exothermic because absorbing energy

c)

endothermic because absorbing energy

d)

endothermic because releasing energy

48.

A 500g piece of aluminum has a temperature of 7°C. What is the heat energy produced? Specific heat of Aluminum is 0.900 J/gºC.

a)

3000 J

b)

3000 g

c)

3150 J

d)

3150 g

49.

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 0.10 J/g°C, what is the mass of the iron sample?

a)

25g

b)

30g

c)

20g

d)

50g

50.

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?

a)

2.34 J/g°C

b)

0.472 J/g°C

c)

6.13 J/g°C

d)

0.163 J/g°C

51.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
52.
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
53.

READ CAREFULLY! YOU HAVE TIME!

A substance with a low specific heat requires less energy to heat up and a substance with high specific heat require more energy to heat up and heats up slower

a)

TRUE

b)

FALSE

54.
___________ is measured by the unit Joules.
a)
Heat energy
b)
Temperature
c)
Specific heat
55.

How many joules of heat are required to raise the temperature of 225 g of aluminum from 20°C to 100°C? (specific heat of aluminum = 0.21 J/g°C)

a)

3780 J

b)

0.59 J

c)

85 J

d)

58 J

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