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Heat of Fusion, Heat of Vaporization, and Specific Heat

Total questions: 45

Worksheet time: 2hrs 8mins

Name
Class
Date
1.
When water is heated from 10°C to 15°C What is the change in temperature?
a)
10 °C
b)
5 °C
c)
15 °C
d)
25 °C
2.

How much energy is required to heat up 12000 g of copper from 10 °C to 120 °C. The specific heat capacity is 0.390 J/g°C.

a)

46800 J

b)

561600 J

c)

514800 J

3.

How many Joules of energy are required to make 100 grams of ice at 0 οC completely melt? The specific latent heat of fusion of ice is 334 J/g

a)

200 J

b)

400 J

c)

33,400 J

d)

2,000,000 J

4.

The heat absorbed by melting a solid is known as

a)

latent heat of fusion

b)

latent heat of solid

c)

latent heat of liquid

d)

latent heat of vaporisation

5.

Water molecules have the greatest kinetic energy in

a)

Ice at 0 ⁰C

b)

Water at 90 ⁰C

c)

Water at 373 K

d)

Steam at 150 ⁰C

6.

The amount of energy required to raise the temperature 1ºC for every gram is called____?

a)

Thermal Energy

b)

Specific Heat

c)

Temperature

d)

Kinetic Energy

7.

How much energy is needed to raise the temperature of 5.0 grams of lead from 25°C to 35°C? [specific heat (c) = 0.129 J/(g•°C)]

a)

6.45 J/(g•°C)

b)

6.45 J

c)

16.1 J/(g•°C)

d)

d.16.1 J

8.

Which of the following best explains why the sand at the beach is hotter than the water?

a)

Sand has a higher specific heat than water.

b)

Sand has a lower specific heat than water.

c)

There is more water than sand at the beach.

d)

There is more sand than water at the beach.

9.
The specific heat(c) of copper is 0.39 J/g °C. 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
10.

Consider the following temperature-time graph when a solid is heated. which part of the graph involves latent heat of vaporization?

a)

Part I

b)

Part II

c)

Part III

d)

Part IV

11.

What is the formula to calculate heat energy required to raise the temperature of any substance?

a)

Q = m c ∆T

b)

Q = m c

c)

Q = ½ m v

d)

m = Q c

12.

If the specific heat of water is 4.186 J/g∙°C, how much heat is required to increase the temperature of 1200g of water from 23 °C to 39 °C?

a)

-80,371.2 J

b)

44,938.6 J

c)

80,371.2 J

d)

-44,938.6 J

13.
What would be the effect on the particles if more heat is supplied to the system?
a)
They would slow down
b)
They would stop moving
c)
They would speed up
d)
There would be no effect
14.
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)
25 g
b)
30 g
c)
20 g
d)
50 g
15.

Using the heat equation, what would the formula look like if we were solving for change in temperature?

a)

Q m = ∆T C

b)

Q / (m C) = ∆T

c)

Q m / C = ∆T

d)

m c Q = ∆T

16.
What unit do you use to measure Thermal Energy?
a)
J/Kg ºC
b)
Kg
c)
ºC
d)
J
17.

The symbol for specific heat is .......

a)

C

b)

Q

c)

m

d)

T

18.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
19.

You have 20 g of water with specific heat of 4.18 J/g°C. The temperature changes from 25° C to 20° C. How much heat energy (Q) moves from the water to the surroundings?

a)

- 418 J

b)

209 J

c)

83 J

d)

418 J

20.
Calculate the heat absorbed by 105.0 grams of water when it is heated to cook spaghetti. The initial temperature of the water is 20.0°C, and the final temperature of the water is 99.0°C. The specific heat of water is 4.18 J/g•°C.
a)
8778 J/g°C
b)
0.0005 J/g°C
c)
34673 J/g°C
d)
43451.1 J/g°C
21.
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
22.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
23.
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
24.
What does temperature measure?
a)
Heat of Molecules
b)
ºC
c)
Average Kinetic Energy of Molecules
d)
Thermal Energy
25.

Equal mass samples of Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using 10,000 JOULES of thermal energy. What material would have the LARGEST change in temperature?

a)

Copper

b)

Carbon Steel

c)

Zinc

d)

Stainless Steel

26.

Equal mass samples of Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using 10,000 JOULES of thermal energy. Based on the chart, which material would be have the SMALLEST change in temperature?

a)

Copper

b)

Carbon Steel

c)

Zinc

d)

Stainless Steel

27.
If 200 grams of water is to be heated from 24.0° C to  100.0° C to make a cup of tea, what is the mass and what is the change in temperature?
a)
m=100g,  ∆t= 224 C
b)
m=200g,  ∆t=124 C
c)
m=100g,  ∆t=24 C
d)
m=200g,  ∆t=76 C
28.

20 g of water. specific heat of water is 4.18 J/g°C. temperature changes from 25° C to 20° C, what will the value of q be?

a)

positive

b)

negative

c)

equilibrium

d)

q does not exist

29.
A material was cooled from 100ºC to 40ºC.  What is the temperature change?
a)
60ºC
b)
40ºC
c)
-60ºC
d)
-40ºC
30.

The unit for specific heat is

a)

J

b)

J/gC

c)

g

d)

°C\degree C

31.

The unit for heat energy is

a)

°C\degree C

b)

J

c)

J/gC

d)

g

32.

What letter do we use to represent mass?

a)

Q

b)

m

c)

c

d)

ΔT\Delta T

33.

The unit for mass is

a)

g

b)

J

c)

J/gC

d)

°C\degree C

34.

What does  ΔT\Delta T  represent?

a)

 tf −tit_{f\ }-t_i  

b)

 ti −tft_{i\ }-t_f  

c)

t - celsius

d)

celsius - t

35.

Consider the following temperature-time graph when a solid is heated. which part of the graph involves latent heat of fusion?

a)

Part I

b)

Part II

c)

Part III

d)

Part IV

36.
The energy transferred between the particles of two objects because of the temperature difference between the two objects is called ________________.
a)
heat
b)
insulator 
c)
conductor 
37.
Exothermic reactions...
a)
Absorb energy
b)
Release energy
c)
Release Color
d)
Absorb Color
38.
In an endothermic reaction, heat is ,,,
a)
taken in
b)
given out
39.

When you place the metal in boiling water, heat flows from the _________ to the _______.

a)

metal to the boiling water

b)

bottom of the metal to the top half of the metal

c)

bottom of the water to the top of the water

d)

boiling water to the metal

40.

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

a)

45 C because molecules have more energy than in 106C

b)

106 C because molecules have more energy than in 45C

c)

106 C because molecules have less energy than in 45C

d)

45C because molecules have less energy than in 106 C

41.

DON'T RUSH, YOU HAVE TIME.

Water droplets condensing on the inside of a window on a cold day. Is this process exothermic or endothermic?

a)

Gases condense to form liquids. Gases are moving faster than liquids, the air around the window has a higher temperature/kinetic energy. Releasing energy to get water droplets, which is is Exothermic

b)

Gases condense to form liquids. Gases are moving faster than liquids, the air around the window has a higher temperature/kinetic energy. Releasing energy to get water droplets, which is is Endothermic

c)

Gases condense to form liquids. Gases particles are moving slower than liquids. Releasing energy to get water droplets, which is is Endothermic

d)

Gases condense to form liquids. Gases particles are moving slower than liquids. Releasing energy to get water droplets, which is is Exothermic

42.

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

43.

YOU HAVE TIME!

How much energy is needed to raise the temperature of a 20.0g piece of copper from 15.0 degrees Celsius to 25.0 degrees Celsius? (The specific heat of copper is 0.385 J/g C)

a)

20 X (25-15) =70 J

b)

20 X .385 X (25-15)= 77 J

c)

20 X .385 X (15-25)= 62 J

d)

20 X .385 X (15-0)= 77 J

44.
The diagram represents which type of reaction
a)
endothermic
b)
exothermic
45.
What kind of graph is this?
a)
endothermic
b)
exothermic

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