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Worksheets

SHC Questions

Total questions: 167

Worksheet time: 3hrs 18mins

Name
Class
Date
1.

What is specific heat capacity?

a)

The power needed to raise the temperature of 1 kg of a substance by 1oC.

b)

The energy needed to raise the temperature of 1 kg of a substance by 1oC.

c)

The temperature increase of 1 kg of a substance when it is heated for 1 minute.

d)

The mass of a substance whose temperature will increase by 1oC when heated for 1 minute.

2.

What are the units for energy?

a)

Joules (J)

b)

Watts (W)

c)

Kilograms (kg)

d)

Seconds (s)

3.

What are the units for mass?

a)

Joules (J)

b)

Watts (W)

c)

Kilograms (kg)

d)

Seconds (s)

4.

What are the units for temperature?

a)

Joules (J)

b)

Watts (W)

c)

Kilograms (kg)

d)

Degree Celsius (oC)

5.

What are the units for specific heat capacity?

a)

Joules per kilogram degree Celsius (J/kgoC)

b)

Joules per kilogram degree Celsius (JkgoC)

c)

Joules per kilogram (J/kg)

d)

Joules per degree Celsius (J/oC)

6.

How do we say Δ in science and maths?

a)

Alpha

b)

Beta

c)

Gamma

d)

Delta

7.

What does Δ represent?

a)

The increase in

b)

The decrease in

c)

The change in

d)

All of the above

8.

The specific heat capacity of a substance is 1000 J/kgoC. How much energy is required to raise 1 kg of it by 1oC?

a)

10 J

b)

100 J

c)

1000 J

d)

10,000 J

9.

Water has specific heat capacity of 4180 J/kgoC and Lead has specific heat capacity 128 J/kgoC. Assume 1 kg of water and 1 kg of Lead are at 50oC. Which material would take longer to cool down to room temperature?

a)

Water

b)

Lead

c)

Both would cool down at same rate

d)

Impossible to tell

10.

What is the name of the variable that tells you how much heat energy is required to change the temperature of 1kg

of substance by 1oC?

a)

Specific Latent Heat Capacity

b)

Specific Heat Capacity

c)

Capacity of Material to withstand heat

11.

Which of these is the correct equation for density?

a)

Density = mass x volume

b)

Density = mass /volume

c)

Density = volume/mass

d)

Density = mass/volume^3

12.

Which state of matter does this particle diagram most closely represent?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

13.

Which state of matter is the most dense?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

14.

What state of matter does the following describe?

"a state of matter that has no fixed shape and no fixed volume"

(a)  

15.

What pieces of equipment would I use to find the volume of an irregularly shaped object?

a)

Newton meter and volume meter

b)

Balance, Ruler, then do length x mass x depth

c)

Balance and eureka beaker

d)

Eureka Beaker and measuring cylinder

16.

A substance is changing state from a gas to a liquid. What do we call this?

(a)  

17.

When a substance changes state, there is a change in mass. True or false?

a)

True

b)

False

18.

Internal energy is....(2 answers)

a)

...stored in the atoms and molecules that make up the system

b)

...the sum of the total kinetic energy and potential energy of particles

c)

... the stored in gases when they are moved around

d)

...increased by moving the substance from one place to another

19.

Look at the following equation E = m c ΔθE\ =\ m\ c\ \Delta\theta  What does the c stand for?

a)

Mass

b)

change in temperature

c)

Latent heat

d)

specific heat capacity

20.

Look at the equation: E=mcΔθE=mc\Delta\theta  Calculate the energy needed to heat 10kg of water (with a SHC of 4200J/kg*C) from 20*C to 30*C

a)

42,000J

b)

42J

c)

420,000J

d)

1,260,000J

21.

What is happening at D?

a)

Liquid changing state into a gas - potential energy of particles is constant

b)

Liquid being heated - kinetic energy of particles is increasing

c)

Liquid being heated, temperature remains constant as there is no energy transfer

d)

Liquid changing state into a gas - temperature of substance remains constant

22.

What happens to the particles in a gas when it is heated?

a)

Particles average kinetic energy increases

b)

Particles move more randomly

c)

They hit into each other less frequently

d)

The pressure of the gas decreases

23.

What is it called when a liquid changes state to a solid?

(a)  

24.

What is it called when a liquid changes state to a gas?

(a)  

25.

What does the Kinetic Theory of Matter suggest about particles?

a)

Particles are only present in gases.

b)

All particles are stationary.

c)

Particles do not exist in solids.

d)

Particles are always in motion.

26.

According to the Kinetic Theory, how does temperature affect particle motion?

a)

Temperature changes cause particles to disappear.

b)

The lower the temperature, the faster the particles move.

c)

Temperature has no effect on particle motion.

d)

The higher the temperature, the faster the particles move.

27.

What state of matter are particles packed tightly in a regular pattern?

a)

Solid

b)

Plasma

c)

Liquid

d)

Gas

28.

What is the process called when a solid turns into a liquid?

a)

Freezing

b)

Melting

c)

Sublimation

d)

Condensation

29.

What is density?

a)

A measure of how much space an object occupies, volume per object

b)

A measure of how much mass is packed into a given volume, mass per unit volue

c)

A measure of how much air an object contains, mass of air per object

d)

A measure of the weight of an object, in newtons

30.

What does the Law of Conservation of Mass state?

a)

Mass is only conserved in physical changes, not chemical reactions.

b)

Mass can be created and destroyed easily.

c)

Mass decreases over time in a closed system.

d)

Mass cannot be created or destroyed in a closed system.

31.

What happens to the particles of a substance during melting?

a)

Particles gain kinetic energy and start to vibrate faster.

b)

Particles lose all their energy.

c)

Particles spread out into a loser structure.

d)

Particles gain potential energy and bonds are broken.

32.

What is specific heat capacity?

a)

The amount of thermal energy needed to change the state of 1 kg of a substance.

b)

The amount of thermal energy needed to raise the temperature of 1 kg of a substance by 1°C.

c)

The amount of thermal energy a substance can hold at one time.

d)

The temperature increase when thermal energy is applied to a substance.

33.

What does absolute zero refer to?

a)

The highest possible temperature measured in Kelvin.

b)

The point at which a substance has maximum kinetic energy.

c)

The average temperature of space.

d)

The temperature at which all molecular motion stops.

34.

What is the Ideal Gas Law represented by?

a)

PV = nRT

b)

F = ma

c)

V = IR

d)

E = mc^2

35.

Increasing the temperature of a fixed volume of gas increases the pressure. Pick the 2 correct explanations for this.

a)

The rate of collisions between particles increases

b)

The force of the collisions between particles increases

c)

The rate of particle collisions with the walls increases

d)

The force of the collisions with the walls increases.

36.

If a fixed mass of air is compressed at constant temperature, the pressure increases. Pick 2 correct statements which together explain this.

a)

The mass of air is squashed more so exerts more pressure outwards

b)

There are more collisions per unit area of the walls

c)

The number of particles stays the same but the area of the walls decreases

d)

The particles are travelling faster so there is a higher rate of collisions with the walls

37.

Put these statements into a suitable order to explain evaporation

a)

Evaporation can take place at temps below the boiling point

b)

which is because the particles have a range of different Ek's

c)

and those with the highest Ek have enough energy to escape the surface

d)

which leaves the remaining particles with a lower average Ek

e)

and hence a lower temperature

1)
2)
3)
4)
5)
38.

Particles with higher velocity have higher​ (a)  

Choose from the below words
kinetic energy
speed
intelligence
power
39.

Comparing solids and liquids, which of the following are TRUE? (choose 2)

a)

Their densities are very similar

b)

Their arrangement is identical

c)

Their internal energy is the same

d)

Solids have a regular array whilst liquids have a random arrangment

40.

When explaining pressure in terms of the particle model, we should always... (pick 3)

a)

Discuss collisions between particles

b)

Discuss collisions with the walls of the container

c)

Use the formula P=F/A to help explain

d)

Remember to consider both the force per collision, and the rate of collisions

e)

Remember to consider both the force of the collisions and the number of collisions

41.
What is an object or group of objects?
a)
systematic
b)
system
c)
suspect
d)
suspicious 
42.
What is an energy transfer?
a)
Dancing 
b)
Movement of energy
c)
Movement of energy from one store to another
d)
something moving
43.
What is a store of energy in an object due to chemical reactions in it?
a)
gravitational store of energy 
b)
chemical store of energy
c)
gravitational potential energy
d)
chemicals
44.
What is an example of a chemical store of energy
a)
nothing
b)
food only
c)
batteries only
d)
batteries and food
45.
What is a kinetic store of energy?
a)
something moving
b)
energy stored in a moving object
c)
elastic potential energy
d)
an stationary object
46.
A store of energy in an object due to it's position in a gravitational field is...
a)
Gravitational Potential Energy Sort
b)
Potential Gravitational Energy Store
c)
Gravity Potential Energy Store
d)
Gravitational Potential Energy Store
47.
This is the type of energy stored in a stretched elastic band
a)
Elastic potential energy
b)
Elastic potential energy store
c)
Potential energy store
d)
Elastic
48.
A thermal store of energy is......
a)
the energy store of any cold object
b)
the energy store of any object 
c)
the energy store of any hot object
d)
any object
49.
A store of energy in the nuclei of atoms in an object is.....
a)
Nucler store of energy
b)
Nuclaer store of energy
c)
Nuclear sort of energy 
d)
Nuclear store of energy
50.
What is the name of the law for "energy can not be created or destroyed. In a closed system there is no net change to the amount of energy in the system"
a)
conservation of energy
b)
conserving energy
c)
energy of conservation
51.
Energy can not be created or destroyed!
a)
True
b)
False
52.
Heating is....
a)
the movement of energy from a colder object to a hotter object
b)
the movement of energy from a hotter object to a colder object
53.

What is the Equation for Kinetic Energy?

a)

Kinetic Energy = 0.5 x Mass x Speed²

b)

Kinetic Energy = 0.5 x Mass² x Speed

c)

Kinetic Energy = 0.5 x Mass² / Speed

54.

What are Equations for Gravitational Potential Energy?

a)

Gravitational Potential Energy = Mass x Gravitational Field Strength x Height

b)

Gravitational Potential Energy = Weight x Height

c)

Gravitational Potential Energy = Mass x Gravitational Field Strength / Height

d)

Gravitational Potential Energy = Weight / Height

55.

The formula for calculating kinetic energy (Ek) is...

a)

2 x speed x mass2

b)

1/2 x speed x mass2

c)

2 x mass x speed

d)

1/2 x mass x velocity2

56.

The units for kinetic energy are...

a)

Joules, J

b)

degrees celsius, oC

c)

kilograms, kg

d)

metres per second m/s

57.
In the equation for kinetic energy, 'm' stands for...
a)
metres
b)
miles
c)
mass
d)
millimetres
58.

What is the formula for elastic potential energy?

a)

Ee=1/2ke2

b)

Ep=1/2ke2

c)

Ee=2ke2

d)

Ep=2ke2

59.

Is Nuclear energy, as a source of electricity, renewable or non-renewable?

a)

Non-renewable

b)

Renewable

60.

What is the specific heat capacity of a material?

a)

The energy required to heat 1kg of an object by 1°C

b)

The energy required to heat a set mass of the material by a set temperature

c)

100

d)

4200

61.

Which material heats up quickest?

a)

Aluminium

b)

Concrete

c)

Diamond

d)

Glass

e)

Water

62.

Which material heats up slowest?

a)

Aluminium

b)

Concrete

c)

Diamond

d)

Glass

e)

Water

63.

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

64.

10 kg of aluminium is heated from 120C to 220C. How much energy is needed?

a)

8 970 000 J

b)

897 J

c)

8970 J

d)

89 700 J

e)

897 000J

65.

2kg of water and 4 kg of water are heated to the same temperature. Which is true

a)

They both require the same amount of energy

b)

2kg needs twice as much energy than the 4kg

c)

4kg needs twice the energy the 2kg needs

d)

4kg needs 4 times the energy the 2kg needs

e)

The 2kg is hotter

66.

What is the equation for specific heat capacity?

a)

Q=mcΔTQ=mc\Delta T

b)

Q=mcΔTQ=\frac{mc}{\Delta T}

c)

Q=ΔTmcQ=\frac{\Delta T}{mc}

d)

Q=cΔTmQ=\frac{c\Delta T}{m}

e)

Q=mΔcTQ=m\Delta cT

67.

What are the units for specific heat capacity?

a)

J kg / °C

b)

J / kg / °C

c)

J / °C

d)

J / kg

e)

kg °C / J

68.
1kg of water cools from 100C to 20C. What is true
a)
It gives out 336 kJ
b)
It gives out 336 J of energy
c)
It takes in 336 kJ
d)
It takes in 336 J
e)
It doesn't take in or give out any energy
69.

What is happening between D and E?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

Sublimation

70.

What is happening between B and C?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

Sublimation

71.

What is happening between A and B?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

None of these options

72.

What does a steep line show?

a)

High specific heat capacity

b)

Low specific heat capacity

c)

Nothing to do with specific heat capacity

73.

What does section B show?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

None of these options

74.

What does section D show?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

None of these options

75.

What does section C show?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

None of these options

76.

What state is the matter in at E?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

e)

Not enough information to say

77.

What state is the matter between C and D

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

e)

Not enough information to say

78.

If  Q=mcΔTQ=mc\Delta T  , what is ΔT\Delta T   

a)

ΔT=Qmc\Delta T=\frac{Q}{mc}  

b)

ΔT=mcQ\Delta T=\frac{mc}{Q}  

c)

ΔT=Qmc\Delta T=Qmc  

d)

ΔT=mQc\Delta T=\frac{m}{Qc}  

e)

c=QmΔTc=\frac{Q}{m\Delta T}  

79.

2 kg of glass is given 84 000 J. What is the change in temperature?

a)

+50°C

b)

-50°C

c)

0°C

d)

+100°C

e)

-100°C

80.

2 kg of glass at a temperature of 20°C is given 84 000 J. What is the final temperature?

a)

+50°C

b)

-50°C

c)

-30°C

d)

70°C

e)

20°C

81.

5 kg of water at a temperature of 60°C gives out 210 kJ of energy. What is the final temperature?

a)

50°C

b)

70 °C

c)

60.01 °C

d)

59.99 °C

e)

60 °C

82.

Which material heats up quickest?

a)

Aluminium

b)

Concrete

c)

Diamond

d)

Glass

e)

Water

83.

Which material heats up slowest?

a)

Aluminium

b)

Concrete

c)

Diamond

d)

Glass

e)

Water

84.

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

85.

10 kg of aluminium is heated from 120C to 220C. How much energy is needed?

a)

8 970 000 J

b)

897 J

c)

8970 J

d)

89 700 J

e)

897 000J

86.

2kg of water and 4 kg of water are heated to the same temperature. Which is true

a)

They both require the same amount of energy

b)

2kg needs twice as much energy than the 4kg

c)

4kg needs twice the energy the 2kg needs

d)

4kg needs 4 times the energy the 2kg needs

e)

The 2kg is hotter

87.

What is the equation for specific heat capacity?

a)

Q=mcΔTQ=mc\Delta T

b)

Q=mcΔTQ=\frac{mc}{\Delta T}

c)

Q=ΔTmcQ=\frac{\Delta T}{mc}

d)

Q=cΔTmQ=\frac{c\Delta T}{m}

e)

Q=mΔcTQ=m\Delta cT

88.

What are the units for specific heat capacity?

a)

J kg / °C

b)

J / kg / °C

c)

J / °C

d)

J / kg

e)

kg °C / J

89.
1kg of water cools from 100C to 20C. What is true
a)
It gives out 336 kJ
b)
It gives out 336 J of energy
c)
It takes in 336 kJ
d)
It takes in 336 J
e)
It doesn't take in or give out any energy
90.

What is happening between D and E?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

Sublimation

91.

What is happening between B and C?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

Sublimation

92.

What is happening between A and B?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

None of these options

93.

What does a steep line show?

a)

High specific heat capacity

b)

Low specific heat capacity

c)

Nothing to do with specific heat capacity

94.

What does section B show?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

None of these options

95.

What does section D show?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

None of these options

96.

What does section C show?

a)

Melting

b)

Boiling

c)

Condensing

d)

Freezing

e)

None of these options

97.

What state is the matter in at E?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

e)

Not enough information to say

98.

What state is the matter between C and D

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

e)

Not enough information to say

99.

If  Q=mcΔTQ=mc\Delta T  , what is ΔT\Delta T   

a)

ΔT=Qmc\Delta T=\frac{Q}{mc}  

b)

ΔT=mcQ\Delta T=\frac{mc}{Q}  

c)

ΔT=Qmc\Delta T=Qmc  

d)

ΔT=mQc\Delta T=\frac{m}{Qc}  

e)

c=QmΔTc=\frac{Q}{m\Delta T}  

100.

2 kg of glass is given 84 000 J. What is the change in temperature?

a)

+50°C

b)

-50°C

c)

0°C

d)

+100°C

e)

-100°C

101.

2 kg of glass at a temperature of 20°C is given 84 000 J. What is the final temperature?

a)

+50°C

b)

-50°C

c)

-30°C

d)

70°C

e)

20°C

102.

5 kg of water at a temperature of 60°C gives out 210 kJ of energy. What is the final temperature?

a)

50°C

b)

70 °C

c)

60.01 °C

d)

59.99 °C

e)

60 °C

103.

Which will heat up faster?

a)

copper

b)

granite

c)

iron

d)

basalt

104.

Which will heat up slower?

a)

water

b)

lead

c)

granite

d)

iron

105.

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.

106.
When a  piece of aluminum foil is taken out of the oven and cools from 100° to 50°, What is the change in temperature?
a)
50°
b)
0°
c)
100°
d)
150°
107.
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
108.

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

109.
What unit do you use to measure Thermal Energy?
a)
J/Kg ºC
b)
Kg
c)
ºC
d)
J
110.
The symbol for specific heat is .......
a)
c
b)
Q
c)
m
d)
t
111.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
112.
What  is the formula to calculate heat energy required to raise the temperature of any substance?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ½mv
d)
m=QC
113.

The specific heat of platinum is 0.133 J/g°C. How much heat(Q) is released when a 10 g piece of platinum cools from 100°C to 50°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

114.

What would be the effect on the particles if more heat is supplied to the system? (a)  

Choose from the below words
They would slow down
They would stop moving
They would speed up
There would be no effect
115.
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)
Venti
d)
All three are the same temperature so they have same thermal energy
116.

Water has a specific heat of 4184 J/KgºC.  Wood has a specific heat of 1760 J/KgºC.  What material needs more energy to raise the temperature 1ºC (a)  

Choose from the below words
Wood
Water
Both are the same
117.
A high specific heat means...
a)

it requires more energy to change temperature

b)

it requires less energy to change temperature

118.

You heat up 2 pans of water; one has 100 mL in it, and the other has 1000 mL. Which one heats up the fastest?

a)

100 mL

b)

1000 mL

c)

They both heat up at the same speed

119.

Which will heat up the fastest? (a)  

Choose from the below words
copper
granite
iron
basalt
120.
Question Image

Rank the materials in order of slowest to heat up to fastest to heat up.

a)

water

1.

1

b)

lead

2.

2

c)

granite

3.

3

d)

iron

4.

4

121.

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)

Sand has a greater mass than water.

d)

Water has a greater mass than sand.

122.

(a)   is the amount of energy required to raise the temperature of 1 kg of mass by 1 oC

123.

Copper, Stainless Steel, Carbon Steel, and Zinc were all heated using the same amount of thermal energy.  What material would be the coolest after being heated?

a)

Copper

b)

Carbon Steel

c)

Zinc

d)

Stainless Steel

124.
Object A has a specific heat of 4.45 J/g⁰C and object B has a specific heat of 1.82 J/g⁰C. Which object will heat up faster?
a)

Object A, it has a lower specific heat

b)

Object B, it has a lower specific heat

c)

Object A, it has a higher specific heat

d)

Object B, it has a higher specific heat

125.
If I have 2 blocks of Aluminium (one of 1kg and one of 10 kg) and heat them up with 6,000 Joules of energy.
Which one will have the SMALLEST change in temperature?
a)
1 kg
b)
10 kg
c)
They both heat up  to the same temperature
d)
It depends on the temperature of the room
126.

Heat will always transfer from the ___________ object to the ________ object.

a)

The hottest object to the coolest object.

b)

The coolest object to the hottest object.

c)

The solid object to the liquid object.

d)

The liquid object to the solid object.

127.
The flow of thermal energy from warmer objects to cooler objects 
a)

Thermal energy

b)

Temperature

c)

Heat

d)

Convection 

128.

Heat flows from an area of ​ (a)   temperature to an area of ​ (b)   temperature.

​ ​

Choose from the below words
high
low
129.

Car A has their AC set to 72oF. Car B has their AC set to 67oF. If it is 98oF outside, which car will heat flow into faster?

a)

Car A

b)

Car B

c)

Heat will flow into the cars at the same rate.

130.

The sun heats up the sand and sea water at the same period of time. Which is the correct observation from the situation given?

a)

sand gets hot slowly and sea water gets hot quickly

b)

sand gets hot quickly and sea water gets hot slowly

c)

both gets hot in a same time.

131.

"When 100 J of heat is supplied to objects X and Y, object X experiences a rise in temperature of 1°C and object Y 2°C. "

Based on the statement above, which objects have higher heat capacity?

a)

X

b)

Y

132.

When 100 J of heat is supplied to objects X and Y, object X experiences a rise in temperature of 1°C and object Y 2°C. This is due to object have different heat capacity. Based on below, which of the best assumptions on "object X have high heat capacity"

a)

Rise of temperature in object X is bigger.

b)

Rise of temperature in object X is smaller

133.

When 100 J of heat is supplied to objects W, X , Y and Z, object W experiences a rise in temperature of 4°C , object X =1°C, object Y = 3 °C and Z = 2°C. Arrange the object in ascending order according to their heat capacity.

a)

W, X, Y, Z

b)

Z, W, Y, X

c)

Y, X, W, Z

d)

X, Z, Y, V

134.

When 500 J of heat is supplied to objects M, N and O, object M experiences a rise in temperature of 5°C, object N= 3°C and object O = 7 °C. Which object has higher heat capacity?

a)

M

b)

N

c)

O

135.

When 500 J of heat is supplied to objects M, N and O, object M experiences a rise in temperature of 5°C, object N= 3°C and object O = 7 °C. Which object has smaller heat capacity?

a)

M

b)

N

c)

O

136.

If the water in beaker A and beaker B is heated for 5 minutes using the same Bunsen burner, which water in the beaker will show higher temperature?

a)

A

b)

B

137.

What does the specific heat capacity of water mean?

=4200 J kg-1°C-1

a)

4200 J heat required by 1 kg of water to raise the temperature by 2 ° C

b)

4200 J heat required by 2 kg of water to raise the temperature by 1 ° C

c)

4200 J heat required by 1 kg of water to raise the temperature by 1 ° C

138.

What are the units for specific heat capacity?

a)

Kg/JºC

b)

J/KgºC

c)

N/mºC

d)

Watts

139.
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
140.
_______________ describes how much energy is required to raise an object's temperature.
a)
Conduction
b)
Convection
c)
Specific Heat
d)
Radiation
141.
A pot of 2400g of water at a temperature of 25˚C is heated on a stove until the water boils (100˚C).  The specific heat of water is 4.18 J/(g˚C).
Determine the heat energy needed to heat the water in the pot to boiling.
a)
133.76J
b)
43,062.2J
c)
752,400J
d)
1,003,200J
142.
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
143.
___________ is measured by the unit Joules.
a)
Heat energy
b)
Temperature
c)
Specific heat
144.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
145.
The symbol for specific heat is .......
a)
c
b)
Q
c)
m
d)
t
146.
What unit do you use to measure Thermal Energy?
a)
J/Kg ºC
b)
Kg
c)
ºC
d)
J
147.
What is Specific Heat?
a)
The  amount of thermal energy required to increase the temperature of 1kg of a material by 1°C.
b)
The  amount of radiant energy required to increase the temperature of 1kgof a material by 1°C
c)
The  amount of energy required to increase the temperature of 1kgof a material by 1°C.
d)
The  amount of friction  required to increase the temperature of 1kgof a material by 1°C.
148.

Which material heats up slowest?

a)

Aluminium

b)

Concrete

c)

Diamond

d)

Glass

e)

Water

149.

10 kg of aluminium is heated from 120C to 220C. How much energy is needed?

a)

8 970 000 J

b)

897 J

c)

8970 J

d)

89 700 J

e)

897 000J

150.

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

a)

418 J

b)

209 J

c)

83 J

d)

4.18 J

151.
Energy is transferred as heat between two objects of ___________ temperatures. 
a)
differing
b)
same
152.
As the kinetic energy of the molecules in a substance increases, the temperature of the substance __________.
a)
increases
b)
decreases
153.
The measure of average kinetic energy of all the particles within an object is called ____________. 
a)
temperature
b)
conduction
c)
radiation
d)
heat 
154.
A high specific heat means...
a)
It heats up quickly with energy added
b)
It requires more energy to change temperature
155.
When you measure the temperature of hot soup, you are measuring the:
a)
thermal energy given off by the bowl
b)
specific heat of the bowl
c)
average kinetic energy of the particles in the soup
d)
thermal expansion of the particles in the soup
156.
The symbol for specific heat is .......
a)
c
b)
Q
c)
m
d)
t
157.
What  is the formula to calculate heat energy required to raise the temperature of any substance?
a)

E=mc∆t

b)

E=mc

c)

E= ½mv

d)

m=EC

158.

A 15.75-g piece of iron absorbs 1086.75 joules of heat energy, and its temperature changes from 25°C to 175°C. Calculate the specific heat capacity of iron.

a)

0.46 J/goC

b)

1.654 J/goC

c)

2,567,446.875 J/goC

159.

How many joules of heat are needed to raise the temperature of 10.0 g of aluminum from 22.0°C to 55.0°C, if the specific heat of aluminum is 0.903 J/g°C?

a)

298 Joules

b)

0.003 Joules

c)

297 J/g°C

d)

0.003 J/g°C

160.

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)

7,650,000 Joules

161.
When a  piece of aluminum foil is taken out of the oven and cools from 100° to 50°, What is the change in temperature?
a)
50°
b)
0°
c)
100°
d)
150°
162.

The specific heat of aluminum is 0.9025 J/g°C. How much heat(Q) is released when a 10.0 g piece of aluminum foil is taken out of the oven and cools from 100.0° to 50.0°?

a)

451 J

b)

45.1 J

c)

400 J

163.
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
164.

20.0 g of water. specific heat of water is 4.184 J/g°C. temperature changes from 25.0° C to 20.0° C, how much heat energy (Q) moves from the water to the surroundings?

a)

418 Joules

b)

209 J

c)

83 J

d)

4.18 J

165.
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=200g
∆t= 66
b)
m=200g
∆t=124
c)
m=200
∆t=100
d)
m=200g
∆t=76
166.

The specific heat(c) of copper is 0.38 J/g °C. What is the temperature change(∆t) when 100.0 Joules of heat(E) is added to 20.0 grams?

a)

13 °C

b)

13.2°C

c)

13.16 °C

167.
Which of the following is NOT true about heat? 
a)
Heat moves from hot to cold
b)
Heat is a form of energy
c)
Heat cannot be transferred
d)
Heat makes molecules speed up 

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