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Heat & Energy Review

Total questions: 48

Worksheet time: 57mins

Name
Class
Date
1.

In chemistry, heat is defined as....

a)

the flow of energy (thermal energy)

b)

temperature

c)

warmth / hot

2.

The symbol "q" represents

a)

quantity

b)

temperature

c)

heat energy

3.

The symbol Δ\Delta means:

a)

change in 

b)

millimeter

c)

triangle

4.

Specific heat capacity is defined as the amount of heat energy required to....

a)

lower the temperature of a substance by 1 degree Celsius

b)

raise the temperature of a all substances by 1 degree Celsius

c)

raise the temperature of 1gram of a substance by 1 degree Celsius

5.

What is the symbol for specific heat?

a)

J

b)

m

c)

c

6.

A measure of the average kinetic energy (motion) of the particles in an object is

a)

Temperature

b)

Mass

c)

Enthalpy

7.

Which is the correct formula for calculating heat energy?

a)

E = q m c T

b)

q = m T

c)

q = m c  Δ\Delta  T

8.

How much energy (q) is required to heat 75 g of water from 200 K to 300 K? (The specific heat of water is 4.18 J/g.K).
q = mc Δ\Delta T

a)

7500 J

b)

25000 J

c)

31350 J

9.

Number 2 represents a ________

a)

solid

b)

liquid

c)

gas

10.
Particles in a _____________ are tightly packed together.
a)
solid
b)
liquid
c)
gas
d)
plasma
11.
When objects absorb heat, the particles...
a)
gain energy and vibrate at fixed position.
b)
gain energy and increase in size.
c)
gain energy and move slower.
d)
gain energy and move faster.
12.

Kinetic energy is what type of energy?

a)

chemical

b)

electric

c)

motion

d)

sound

13.

The faster the particles move, the less kinetic energy there is.

a)

True

b)

False

14.

REVIEW: What is the temperature of 25 degrees Celcius in Kelvin?

a)

298

b)

300

c)

273

d)

77

15.

SI unit of energy

a)

Calorimeter

b)

Calorie

c)

Joule

d)

Enthalpy

e)

Specific heat

16.

The energy required to melt a solid at its melting point

a)

Heat of reaction

b)

Heat of formation

c)

Hess's Law of heat summation

d)

Heat of fusion

e)

Heat of solution

17.

Which of these phase changes is an endothermic process?

a)

Condensation

b)

Evaporation

c)

Freezing

d)

All phase changes are endothermic

18.

A process where the system absorbs heat is an ____________ process.

a)

Endothermic

b)

Polythermic

c)

Exothermic

d)

Ectothermic

19.

What is the amount of heat required to raise the temperature of 200.0 g of aluminum by 10°C? (specific heat of aluminum = 0.21 cal/g°C)

a)

420 cal

b)

4,200 cal

c)

42,000 cal

d)

420,000 cal

20.

What is the specific heat of a substance if 1560 J are required to raise the temperature of a 312-g sample by 15°C?

a)

0.033 cal/g°C

b)

0.33 cal/g°C

c)

0.99 cal/g°C

d)

1.33 cal/g°C

21.

The specific heat of silver is 0.24 J/g°C . How many joules of energy are needed to warm 4.37 g of silver from 25.0°C to 27.5°C?

a)

2.62 J

b)

0.14 J

c)

45.5 J

d)

0.022 J

22.

Deposition is the change from

a)

solid to gas

b)

gas to solid

c)

liquid to solid

d)

solid to liquid

23.

Sublimation is the change from

a)

solid to liquid

b)

solid to vapor

c)

gas to solid

d)

liquid to vapor

24.

While a substance is boiling the kinetic energy

a)

increases

b)

deceases

c)

stays the same

25.

Temperature is a measure of

a)

energy

b)

average potential energy

c)

average kinetic energy

d)

heat

26.

State at F

a)

solid

b)

liquid

c)

gas

d)

plasma

27.

phase change between b and c

a)

melting

b)

boiling

c)

vaporization

d)

condensation

28.

kinetic energy is changing between

a)

A and B

b)

B and C

c)

C and D

d)

D and E

e)

E and F

29.
Energy is transferred as heat between two objects of ___________ temperatures. 
a)
differing
b)
same
30.
As the kinetic energy of the molecules in a substance increases, the temperature of the substance __________.
a)
increases
b)
decreases
31.

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

32.

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

33.

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

34.
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°
35.

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

36.

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

37.
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
38.
The phase change from water vapor to liquid water is known as...
a)
evaporation
b)
precipitation
c)
condensation
d)
sublimation
39.
2. A change of state from a liquid to a solid is called....
a)
Melting
b)
Freezing
c)
Evaporation
40.
Endothermic phase changes include
a)
conduction, convection and radiation
b)
freezing and condensation
c)
vaporization and condensation
d)
melting, boiling, evaporation and sublimation
41.

In an endothermic reaction, energy is _________.

a)

absorbed

b)

released

42.

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

43.

What does Q stand for?

a)

Heat or Energy

b)

Mass

c)

specific heat or specific heat capacity

d)

Temperature

44.

What unit is Heat/Energy usually in?

a)

oC

b)

Joules

c)

J/goC

45.

What does m stand for and what is it's unit?

a)

temperature change, oC

b)

Heat, Joules

c)

mass, grams

d)

specific heat, J/goC

46.

How many Joules of energy are required to make 50.0 grams of ice at 0 οC completely melt?

a)

334 J

b)

0 J

c)

33,400 J

d)

16,700 J

47.

The heat absorbed while a solid is melting is known as....

a)

heat of fusion

b)

heat of solid

c)

heat of liquid

d)

heat of vaporization

48.

Calculate the energy needed to completely boil away 30 g of water at 100 ⁰C .

a)

67,800 J

b)

2260 J

c)

226,000 J

d)

100 J

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