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Specific Heat and Calorimetry

Total questions: 39

Worksheet time: 1hrs 13mins

Name
Class
Date
1.

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

2.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
3.
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
4.
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
5.

If the specific heat of water is 4,184 J/g∙°C, how much heat is required to increase the temperature of 1200 g of water from 23 °C to 39 °C?

a)

-80,371.2 J

b)

44,938.6 J

c)

80,371.2 J

d)

112,575.9 K

6.
There are four cups of hot cocoa. The cup sizes are shown. The temperature of the cocoa in each cup is 25 degrees celsius. Which cup has the MOST thermal energy?
a)
Large cup (Trenta)
b)
Small cup (Tall)
c)
Medium cup (Venti)
d)
All three are the same temperature so they have the same thermal energy
7.
A high specific heat means...
a)
It requires less energy to change temperature
b)
It requires more energy to change temperature
c)
It heats up very quickly
8.
A high specific heat means...
a)
It requires less energy to change temperature
b)
It requires more energy to change temperature
c)
It heats up very quickly
9.

Observe the diagram. Which statement is true about the kinetic energy of the molecules in the containers?

a)

The molecules are moving faster in Diagram A

b)

The molecules are moving slower in Diagram A

c)

The molecules are moving at the same rate in both diagrams

10.
The measure of average kinetic energy of all the particles within an object is called ____________. 
a)
temperature
b)
conduction
c)
radiation
d)
heat 
11.
As the kinetic energy of the molecules in a substance increases, the temperature of the substance __________.
a)
increases
b)
decreases
12.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
13.
The symbol for specific heat is .......
a)
c
b)
Q
c)
m
d)
t
14.

A 300.0 g piece of copper is heated and fashioned into a bracelet. The amount of energy transferred by heat to the copper is 66,300 J. If the specific heat of copper is 0.3845 J/g 0C, what is the change of the copper's temperature?

a)

641 °C

b)

756 °C

c)

756 J

d)

641 J

15.
A material was cooled from 100ºC to 40ºC.  What is the temperature change?
a)
60ºC
b)
40ºC
c)
-60ºC
d)
-40ºC
16.

A metal cube at temperature of 70°C is immersed in water at temperature of 20°C. The final temperature of the mixture will be

a)

Between 20°C and 70°C

b)

More than 70°C

c)

Less than 20°C

d)

Same as the room temperature

17.

A metal cube at temperature of 70°C is immersed in water at temperature of 20°C. The metal _______ heat while the water __________ heat.

a)

gains, loses

b)

loses, gains

18.

A metal cube at temperature of 70°C is immersed in water at temperature of 20°C.

a)

The metal loses more heat than the water gains.

b)

The metal loses less heat than the water gains.

c)

The metal loses the same amount of heat that the water gains.

19.

A glass of water is placed in a freezer. Which way does energy flow?

a)

Into the freezer

b)

Into the glass of water

c)

Energy does not flow

20.
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
21.

If two objects have different temperatures when they come in contact, 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

22.
Calorimetry Question:
A piece of metal with a mass of 32.8 g is heated to 100.5°C and dropped into 138.2 g of water at 20.0°C.  The final temperature of the system is 30.2°C.  What is the specific heat capacity of the metal? (show your work)
a)
2.56 J/g°C
b)
0.391 J/g°C
c)
5.29 J/g°C
d)
3.50 J/g°C
23.
Calorimeters use insulating materials to:
a)
encourage affordable materials in science experiments in schools.
b)
preserve the heat of the environment outside the Styrofoam cup.
c)
prevent heat from escaping to the environment.
d)
keep the liquid inside the Styrofoam cup from overheating.
24.

Shown are the units for....

a)

specific heat capacity

b)

mass

c)

temperature

d)

energy

25.
The Law of Conservation of Energy states:
a)
Energy can created or destroyed but not transformed 
b)
Energy cannot be created or destroyed, it can only transformed
c)
Energy can't be created, destroyed or transformed
26.
According to the Law of Conservation of energy, the amount of energy before and after a reaction must be the same. Which statement below is true?
a)
The total amount of energy is conserved
b)
The total amount of energy is less after a reaction
c)
The total amount of energy is more after a reaction
27.

When cooking a pizza in an oven, the oven loses energy and so does the pizza

a)

True

b)

False

28.

Why is it possible to calculate the heat given off by the food based on the change in temperature of the water?

a)

Because the water absorbs the heat from the food

b)

Because the temperature of the water decreases

c)

Because the food increases the water volume

d)

Because the water changes its chemical composition

29.

What is the definition of a calorie?

a)

The amount of energy needed to raise 1 g H2O by 1ºC.

b)

The amount of energy needed to raise 1000 g H2O by 1ºC.

c)

The amount of energy needed to raise 1 L air by 1ºC.

d)

The amount of energy needed to raise 1 g H2O by 10ºC.

30.

Stored energy in chemical bonds

a)

thermochemistry

b)

chemical potential energy

c)

heat

d)

equilibrium

31.

The study of heat changes that occur during physical and chemical changes.

a)

Heat

b)

Equilibrium

c)

Specific Heat

d)

Thermochemistry

32.

To convert calories to joules, you need to____

a)

divide by 4.18

b)

multiply by 4.18

c)

add 4.18

d)

subtract 4.18

33.
Which of the following statements is true about energy conversion?
a)
1 Calorie is equal to 1 calorie
b)
1 kilocalorie is equal to 1 Calorie
c)
1 joule is equal to 1 calorie
d)
1 calorie is equal to 1 Calorie
34.
Which conversion is correct?
a)
1 Calorie = 4.184 joules
b)
1 calorie = 4.184 joules
c)
1 Calorie = 0.4184 joules
d)
1 kilocalorie = 0.4184 joules
35.
What is the energy equivalent of 5000 calories in joules?
a)
2092 joules
b)
209200 joules
c)
2092000 joules
d)
20920 joules
36.
Convert 300 kilocalories to joules.
a)
12552 joules
b)
125520 joules
c)
1255200 joules
d)
12552000 joules
37.
If a food label shows 300 Calories, how many kilocalories does this represent?
a)
0.3 kilocalories
b)
30 kilocalories
c)
300 kilocalories
d)
3,000 kilocalories
38.
A runner burns 2000 Calories during a marathon. How many joules of energy is this equivalent to?
a)
8,368 joules
b)
83,680 joules
c)
836,800 joules
d)
8,368,000 joules
39.
A snack contains 150 Calories. How many regular calories (small 'c') is this?
a)
150,000 calories
b)
1,500 calories
c)
15,000 calories
d)
1.5 calories

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