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Physics: Thermodynamics

Total questions: 85

Worksheet time: 7hrs 3mins

Name
Class
Date
1.

Transfer of heat from low temperature to high temperature is

a)

None of these

b)

Possible by doing some external work

c)

Possible by keeping both the bodies in contact

d)

Impossible

2.

-ΔH

a)

endothermic

b)

exothermic

c)

entropy

d)

gibe's free energy

3.
In heat transfer, heat always flows from the _______________ substance to the _______________ substance.
a)
Hotter to colder
b)
Colder to hotter
c)
Hotter to hotter
d)
Colder to colder
4.
Which statement is true?
a)
The quicker a molecule moves, the colder it is.
b)
The slower a molecule moves, the warmer it is.
c)
The quicker a molecule moves, the warmer it is
d)
The movement on molecule don�t affect its temperature
5.
Two objects at different temperatures are in contact. Which of the following happens to their thermal energy?
a)
Their thermal energies remain the same.
b)
Thermal energy passes from the cooler object to the warmer object
c)
Thermal energy passes from the warmer object to the cooler object.
d)
Thermal energy passes back and forth equally between the two objects.
6.
When the temperature of matter increases the particles...
a)
speed up and move closer
b)
speed up and move farther apart
c)
slow down and move closer together
d)
slow down and move farther apart
7.

True or False? Temperature is a measure of the total kinetic energy in a substance.

a)

True

b)

False

8.

Select the correct SI unit for Heat

a)

calorie

b)

joule

c)

kelvin

d)

celsius

9.

Select the correct symbol for Heat

a)

H

b)

t

c)

Q

d)

E

10.

What is the branch of physics concerned with heat and temperature?

a)

Kinematics

b)

Mechanics

c)

Optics

d)

Thermodynamics

11.

The law stating that energy is neither created nor destroyed; it only changes form. It is also known as the law of conservation of energy.

a)

First Law of Thermodynamics

b)

Second Law of Thermodynamics

c)

Third Law of Thermodynamics

d)

Fourth Law of Thermodynamics

12.

A law stating that all spontaneous processes result in an increase in the total entropy of the system and its surroundings.

a)

First Law of Thermodynamics

b)

Second Law of Thermodynamics

c)

Third Law of Thermodynamics

d)

Fourth Law of Thermodynamics

13.

Consider 2 blocks of Aluminium (one of 1kg and one of 10 kg) and being supplied with thermal energy.

Which one heats up the fastest?

a)

1 kg

b)

10 kg

c)

They both heat up at the same rate

d)

They don't heat up.

14.

The specific heat(c) of copper is 0.39 Jg-1K-1. 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

15.
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
16.
Heat energy moves from __________ things to _________ things.
a)
warm / cold
b)
cold / warm
c)
liquid / solid
17.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
18.

Specific heat of water is 4.18 J/g°C. Specific heat of wood is 1.760 J/g°C What material needs more heat energy to raise the temperature?

a)

Water

b)

Wood

c)

Both are same

19.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
20.
Temperature is a measure of the...
a)
total energy in a substance
b)
total kinetic energy in a substance
c)
average potential energy in a substance
d)
average kinetic energy of molecules in a substance
21.
A slower particle has a lower energy than an identical, faster particle.
a)
True
b)
False
22.
The transfer of thermal energy between objects of different temperatures is called...
a)
temperature
b)
heat
c)
internal energy
d)
none of these
23.
It is possible to reach absolute zero
a)
true
b)
false
24.
A substance with a high specific heat:
a)
Is always extremely hot.
b)
Requires a lot of energy to become hot.
c)
Is not heavy.
d)
Does not requires a lot of energy to become hot.
25.
The first law of thermodynamics states that energy is
a)
created
b)
destroyed
c)
conserved
d)
created and destroyed
26.
Which direction will the heat flow while this person holds a hot cup of tea?
a)
from the cup to her hand
b)
from her hand to the cup
c)
no heat is transferred
27.
Which direction will the heat flow while this ice cap melts?
a)
there is no heat transfer
b)
from the icecap to the water
c)
from the water to the icecap
28.
What is thermodynamics?
a)
movement of heat
b)
it's magic
c)
measurement of heat
d)
none of them
29.
The Law of _______________ states that energy cannot be created nor destroyed only transferred 
a)
Specific Heat
b)
Conservation of Energy
c)
Exothermic Reaction
d)
Potential Energy
30.
The capacity of a substance to store heat depends on what it's made of is:
a)
Heat Index
b)
Exact Heat Holding Power
c)
Specific Heat Capacity
d)
Elemental Heat Capacity
31.
The property of a thermometer that allows it to indicate temperature is
a)
thermal expansion
b)
heat capacity
c)
thermal equilibrium
d)
conduction
32.

The U in the equation stands for ...

a)

heat being added

b)

change in internal energy

c)

work being done

33.

The first law of thermodynamics is basically the same as ...

a)

Newton's first law

b)

The law of conservation of momentum

c)

The law of conservation of energy

d)

Newton's second law

34.
What is absolute zero?
a)
0 K
b)
273 K
c)
0oC
35.
Δt Stands for?
a)
Specific Heat
b)
Joules
c)
Mass
d)
Change in temp
36.
The variable M stands for? 
a)
mass
b)
time 
c)
heat
d)
joules
37.
the amount of thermal energy needed to change a substance from solid to liquid or from liquid to solid
a)
heat of fusion
b)
heat of vaporization
38.
the amount of thermal energy needed to change a substance from liquid to a gas or from gas to liquid
a)
heat of fusion
b)
heat of vaporization
39.

Formula for first law of thermodynamics

a)

ΔU= Q+W

b)

ΔU = Q

c)

ΔQ = U+ W

d)

W = P+ W

40.
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
41.
High temperature is connected to:
a)
Low kinetic energy.
b)
High kinetic energy.
c)
Zero net energy.
d)
Equal kinetic energies.
42.
The amount of thermal energy required to raise the temperature of one (1) kilogram of a substance by 1o C is known as:
a)
Specific heat
b)
Heat of fusion
c)
Heat of vaporization
d)
Melting point
43.
How much heat will be absorbed by 3 kg of water to raise the temperature from 10°C to 60°C? (Cp=4184 J/kg°C) Equation: Q=Cpm(Tf -Ti)
a)
627600 J
b)
41840 J
c)
167360 J
d)
376560 J
44.
How much heat will be absorbed by 1 kg of water to raise the temperature from 5°C to 15°C? (Cp=4184 J/kg°C) Equation: Q=Cpm(Tf -Ti)
a)
627600 J
b)
41840 J
c)
167360 J
d)
376560 J
45.
How much heat will be absorbed by 1 kg of water to raise the temperature from 2°C to 42°C? (Cp=4184 J/kg°C) Equation: Q=Cpm(Tf -Ti)
a)
627600 J
b)
41840 J
c)
167360 J
d)
376560 J
46.
How much heat will be absorbed by 3 kg of water to raise the temperature from 70°C to 100°C? (Cp=4184 J/kg°C) Equation: Q=Cpm(Tf -Ti)
a)
627600 J
b)
41840 J
c)
167360 J
d)
376560 J
47.
How much heat will be absorbed by 10 kg of water to raise the temperature from 60°C to 61°C? (Cp=4184 J/kg°C) Equation: Q=Cpm(Tf -Ti)
a)
41840 J
b)
313800 J
c)
418400 J
d)
836800 J
48.
How much heat will be absorbed by 15 kg of water to raise the temperature from 90°C to 95°C? (Cp=4184 J/kg°C) Equation: Q=Cpm(Tf -Ti)
a)
41840 J
b)
313800 J
c)
418400 J
d)
836800 J
49.
How much heat will be absorbed by 2 kg of water to raise the temperature from 0°C to 50°C? (Cp=4184 J/kg°C) Equation: Q=Cpm(Tf -Ti)
a)
41840 J
b)
313800 J
c)
418400 J
d)
836800 J
50.
How much heat will be absorbed by 2 kg of water to raise the temperature from 0°C to 100°C? (Cp=4184 J/kg°C) Equation: Q=Cpm(Tf -Ti)
a)
41840 J
b)
313800 J
c)
418400 J
d)
836800 J
51.
A student rubs his hands together. The work done by his hands is 100 J. The change in internal energy is 200 J. How much heat will be produced? (Q=ΔU-W)
a)
100 J
b)
125 J
c)
240 J
d)
120 J
52.
A student rubs his hands together. The work done by his hands is 75 J. The change in internal energy is 200 J. How much heat will be produced? Equation:Q=ΔU-W
a)
100 J
b)
125 J
c)
240 J
d)
120 J
53.
A student rubs his hands together. The work done by his hands is 60 J. The change in internal energy is 300 J. How much heat will be produced? Equation:Q=ΔU-W
a)
100 J
b)
125 J
c)
240 J
d)
120 J
54.
A student rubs his hands together. The work done by his hands is 120 J. The change in internal energy is 240 J. How much heat will be produced? Equation:Q=ΔU-W
a)
100 J
b)
125 J
c)
240 J
d)
120 J
55.
A system gains 350 J of heat from its surroundings, and 1540 J of work is done on the system. What is the change in internal energy? (ΔU=Q+W)
a)
1890 J
b)
1190 J
c)
4.4 J
d)
0 J
56.
A system gains 300 J of heat from its surroundings, and 890 J of work is done on the system. What is the change in internal energy? (ΔU=Q+W)
a)
1890 J
b)
1190 J
c)
4.4 J
d)
0 J
57.
How much energy must be added to a bowl of 0.2 kg of popcorn kernels in order for them to reach a popping temperature of 175°C? Assume their initial temperature is 21°C, and that the specific heat of popcorn is 1650 J/kg°C. Equation: Q=Cpm(Tf-Ti)
a)
0 J
b)
1650 J
c)
50820 J
d)
15280 J
58.

20 g of water has its temperature changes from 25° C to 20° C, how much heat energy (Q) moves from the water to the surroundings? The specific heat capacity of water is 4.18 J g-1 °C-1.

a)

418 Joules

b)

209 J

c)

83 J

d)

4.18 J

59.

Given that the specific heat capacity of water is 4.18 J g-1 °C-1 and the specific heat capacity of wood is 1.760 J g-1 °C-1. Which material needs more heat energy to raise the temperature?

a)

Water

b)

Wood

c)

Both are same

60.

The specific heat capacity of copper is 0.39 J g-1 °C-1. 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

61.
The temperature scale for Kelvin is based off of absolute zero
a)
True
b)
False
62.
In physics, there is no such thing as
a)
heat
b)
cold
c)
energy
d)
temperature
63.
Temperature only flows between objects when they are different temperatures
a)
True
b)
False
64.
Q=mc∆T is the equation we use for specific heat.
a)
True
b)
False
65.
A hot object is dropped into a container of cold water. What happens to the molecular motion of the hot object? What happens to the molecular motion of the cold object? 
a)
the molecules in both objects will slow down until they come to rest
b)
the molecules of the hot object slow down while the cold speed up
c)
the molecules of the hot speed up while the cold slows down
d)
the molecules in both objects will speed up until they reach identical speeds
66.
How much heat must be absorbed by 2.30 kg of water to raise the temperature from 12.0 °C to 55.0 °C?
a)
185 J
b)
413,000 J
c)
989,000 J
d)
1,200,000 J
67.
The specific heat of aluminum is 0.21 cal/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)
10.5 J
c)
1.05 J
68.
How many Joules of energy are required to change 10 gram of water from 20 C to 90 C?
a)
1400 J
b)
2800 J
c)
210,000 J
d)
1,400,000 J
69.
If the specific heat of water is 4,186 J/kg∙°C, how much heat is required to increase the temperature of 1.2 kg 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
70.
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
71.
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
72.
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
73.

How much heat is needed to change 12 grams of ice at 0 ºC to 12 grams of water at 0ºC?

a)

960 cal

b)

80 cal

c)

0 cal

d)

96 cal

74.

How much heat is needed to change 12 grams of water at 100 ºC to 12 grams of water vapor at 100ºC?

a)

648 cal

b)

540 cal

c)

6480 cal

d)

732 cal

75.

How much heat must be lost to change of 110 grams of water at 0 ºC to 110 grams of ice at 0ºC?

a)

110 cal

b)

54 cal

c)

8800 cal

d)

3764 cal

76.

How much heat is needed to raise the temperature of 45 grams of water at 5 ºC to 68ºC?

a)

24300 cal

b)

3060 cal

c)

3282 cal

d)

2835 cal

77.

How much heat must be lost to lower the temperature of 931 grams of ice at 0ºC to -130 0ºC?

a)

-60515 cal

b)

60515 cal

c)

-121030 cal

d)

121030 cal

78.

How much heat is needed to change the temperature of 315 grams of ice at -20 ºC to water at 60ºC?

a)

25200 cal

b)

28350 cal

c)

47250 cal

d)

18900 cal

79.

How much heat is needed to change the temperature of 98 grams of water vapor at 137 ºC to water at 5ºC?

a)

9310 cal

b)

64043 cal

c)

54733 cal

d)

62230 cal

80.

Latent heat is

a)

the heat absorbed or released at a boiling process during a change of phase

b)

the heat absorbed or released at a constant temperature during a change of phase

c)

the heat absorbed or released at a constant temperature during a change of phase of 1 kg object

d)

the heat absorbed or released by an object to increase or decrease its temperature by 1 degree Celcius

81.

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

82.

specific latent heat of vaporization is

a)

the amount of heat required to change 1 kg of the substance from the solid to liquid phase without change in temperature

b)

the amount of heat required to change 1 kg of the substance from the liquid to gaseous phase without change in temperature

c)

the amount of heat required to change the temperature 1 kg of the substance by 1 degree Celcius

83.

the symbol for specific latent heat is

a)

c

b)

L

c)

Q

d)

m

84.

What is the formula to calculate specific latent heat of vaporization?

a)

L = Q/m

b)

c = Q/(mΔƟ)

c)

Q = mcΔƟ

d)

Q = mL

85.

What is the S.I unit for specific latent heat

a)

J kg-1 oC-1

b)

J kg-1

c)

J

d)

oC

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