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CALORIMETRY

Total questions: 50

Worksheet time: 1hrs 18mins

Name
Class
Date
1.

If ΔT is positive then heat is being ___________by the reaction, and if  ΔT is negative then heat is being _____________by the reaction.

a)

absorbed, released

b)

released, absorbed

c)

heat is staying the same

d)

There is no way to know what is going on with the heat.

2.

What is calorimetry?

a)

The process of measuring the amount of heat that is absorbed or released in a chemical reaction

b)

The process of measuring the amount of time it takes for certain reactions to take place

3.
For the formula:
 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
4.
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
5.

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

6.
The total energy of all the particles in a substance is called: 
a)
temperature
b)
thermal energy
c)
degrees
d)
mass
7.

If the specific heat of water is 4.18 J/g∙°C, how much heat is required to increase the temperature of 1.2 kg of water from 23 °C to 39 °C? (show your work)

a)

-80,256 J

b)

80.256 J

c)

80,256 J

d)

-80.256 J

8.
What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water.  The water weighs 75. g and had an initial temperature of 20.00 °C?  (Specific heat of water is 4.18 J/g°C) (show your work)
a)
0.111 J/g°C
b)
1.29 J/g°C
c)
0.129 J/g°C
d)
22225.85 J
9.

For a skillet, used for cooking, do you want a high or low specific heat

a)

High, so that it will need more energy to heat up

b)

Low, so that it will change temperature quickly

10.
The SI unit of heat and energy is the __________.
a)
calorie
b)
heat
c)
joule
d)
watt
11.
A sample of iron receives 50.J of heat energy that raises the temperature of the iron by 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?  (show your work)
a)
25g
b)
30g
c)
20g
d)
50g
12.
A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius. Is the reaction endothermic or exothermic?
a)
Exothermic
b)
Endothermic
13.
In an exothermic process, the surroundings are gaining energy.
a)
True
b)
False
14.

What does "q" mean?

a)

A measure of heat energy

b)

A change in heat energy

c)

A measure of kinetic energy

d)

A change in temperature

15.
What is a tool that measures the heat of chemical reactions?
a)
calorimeter
b)
 calorie
c)
Styrofoam™ cup
d)
none of these
16.
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.
17.
A metal cube at temperature of 10°C immersed in a liquid at temperature of 70°C.
What is the temperature of the metal cube when thermal equilibrium is achieved between the cube and the liquid?
a)
Between 10°C and 70°C
b)
More than 70°C
c)
Less than 10°C
d)
Same as the room temperature
18.

The specific heat of water is 4.18 J/g°C.

If 980. J of energy is added to 6.20 g of water at 18.0 °C, what is the final temperature of the water?

a)

37.8 °C

b)

-19.8 °C

c)

19.8 °C

d)

55.8 °C

19.

What does "ΔT" mean?

a)

A change in health

b)

A change in heat

c)

A change in height

d)

A change in temperature

20.

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

21.
What is the specific heat of an unknown substance if 100.0 g of it at 200.0 °C reaches an equilibrium temperature of 27.1 °C when it comes in contact with a calorimeter of water.  The water weighs 75. g and had an initial temperature of 20.00 °C?  (Specific heat of water is 4.18 J/g°C) (show your work)
a)
0.111 J/g°C
b)
1.29 J/g°C
c)
0.129 J/g°C
d)
22225.85 J
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) [specific heat of water is 4.185 J/goC]

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.
For the formula:
 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
24.
LT3: 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
25.
The unit Joules is for ___________
a)
heat energy
b)
temperature
c)
specific heat
26.

78.9 g of copper is dropped into a calorimetry containing 112 g of water. The water temp is initially 13oC. The final temp for both the metal and water is 27.6oC. What was the initial temp of the copper? (ccopper = 0.39 J/goC, cwater = 4.18 J/goC)

a)

7690oC

b)

249.9oC

c)

30.77oC

d)

13oC

27.

175 g of aluminum are heated to 100oC. It is then dropped in a calorimeter that contains 40.0 g of water at a temp of 1.8oC. Determine the final temp of the metal and the water. (caluminum = 0.90 J/goC) (cwater = 0.90 J/goC)

a)

16051 oC

b)

324.86oC

c)

49.41oC

d)

100oC

28.

Which best explains why metal is a good material to make frying pans?

a)

Metal is a good conductor of heat and transfers heat from the stove to the food.

b)

Metal is a good conductor of heat and does not transfer heat from the stove to the food.

c)

Metal is a poor conductor of heat and transfers heat from the stove to the food.

d)

Metal is a poor conductor of heat and does not transfer heat from the stove to the food.

29.

Which material heats up quickest?

a)

Aluminium

b)

Concrete

c)

Diamond

d)

Glass

e)

Water

30.

Some 1kg of water and 1kg of diamond are heated to the same temperature. Which is true?

a)

They both require the same amount of energy

b)

The diamond needs around 8 times more energy

c)

The water needs about 8 times more energy

d)

The diamond heats up slower than the water

e)

The water ends up colder

31.
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
32.

Heat energy ALWAYS moves from _____ to _____.

a)

solid to liquid

b)

ice to water

c)

hot to cold

d)

solid to gas

33.

If the specific heat of water is 4.18 J/kg∙°C, how much heat is required to increase the temperature of 1200 g of water from 23 °C to 39 °C?

a)

-80,371

b)

44,938

c)

80,256

d)

112,575

34.

The letter used for specific heat is .......

a)

C

b)

Q

c)

m

d)

T

35.

What does "ΔT" mean?

a)

A change in health

b)

A change in heat

c)

A change in height

d)

A change in temperature

36.
In an exothermic process, the surroundings are gaining energy.
a)
True
b)
False
37.

Identify the given ΔT in problem:

a)

15.75 g

b)

1086.75 J

c)

150°C

d)

unknown (aka ?)

38.

1 cal = ___ J

a)

4.184

b)

0.24

c)

0.42

d)

4184

39.

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

40.

Why does an ice cube melt when dropped into hot liquid?

a)

The liquid absorbs heat from the ice.

b)

Heat from the liquid transfers to the ice.

c)

Heat from the ice transfers to the liquid.

d)

Cold from the ice transfers into the liquid.

41.

When a hot block of metal is dropped into a cup of cold water, heat is transferred

a)

from the water to the metal

b)

from the metal to the water

42.

In an endothermic process, the surroundings are gaining energy.

a)

True

b)

False

43.

Identify the m in problem:

a)

15.75 g

b)

1086.75 J

c)

150°C

d)

unknown (aka ?)

44.

Identify the value for q in problem:

a)

15.75 g

b)

1086.75 J

c)

150°C

d)

unknown (aka ?)

45.

Identify the specific heat value in problem:

a)

15.75 g

b)

1086.75 J

c)

150°C

d)

unknown (aka ?)

46.

Identify the mass in the problem

a)

10.0 g

b)

33°C

c)

0.90 J/g°C

d)

unknown (aka ?)

47.

If 95.0 g of water increases in temperature from 23.1oC to 36.5oC, the water...

a)

absorbs 5320 J of heat

b)

releases 5320 J of heat

c)

absorbs 14500 J of heat

d)

releases 1273 J of heat

e)

absorbs 1273 J of heat

48.

How much heat is transferred when a 24.3 g object with a specific heat capacity of 0.73 J/goC cools from 86oC to 54oC?

a)

-568 J

b)

1530 J

c)

+567 J

d)

-958 J

49.
The first law of thermodynamics is a restatement of the
a)
Zeroth law of thermodynamics
b)
law of heat addition
c)
principle of entropy
d)
conservation of energy
50.
The amount of energy required to raise the temperature 1ºC for every kilogram is called____?
a)
Thermal Energy
b)
Specific Heat
c)
Temperature
d)
Kinetic Energy

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