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Energy Changes

Total questions: 77

Worksheet time: 2hrs 44mins

Name
Class
Date
1.

How does heat move?

a)

From warmer object to cooler object

b)

From cooler object to warmer object

2.

When particles move, they have --- energy.

a)

Potential

b)

Kinetic

c)

No energy

3.

---- is a measure of the average kinetic energy of particles in an object.

a)

Heat

b)

Temperature

4.

--- is the transfer of thermal energy from a warmer object to a cooler object.

a)

Heat

b)

Temperature

5.

What is collision theory?

a)

Molecules must collide in the correct orientation with enough energy to bond.

b)

Molecules need enough energy to collide and react.

c)

Atoms constantly collide and react.

d)

The minimum energy needed for atoms to react

6.

What is the rate of reaction?

a)

How much energy is needed for a reaction to occur.

b)

The energy required to break a bond.

c)

The time it takes for a reaction to occur.

d)

Collision Theory

7.

Increasing the temperature of your solution will.......

a)

Not affect the rate of reaction.

b)

Speed up the rate of reaction

c)

Slow down the rate of reaction

8.

Decreasing the concentration of a substance will usually........

a)

Slow down the reaction

b)

Speed up the reaction

c)

Have no affect on the reaction

9.

Which has more surface area?

a)

Large chunks of chalk

b)

Cube of sugar

c)

Powdered sugar

d)

Small chunks of sugar

10.

If you shrink the container size that your gas substance is in what will happen?

a)

The reaction rate will stay the same

b)

The reaction rate will speed up

c)

The reaction rate will slow down

11.
If the reactant particles collide with less than the activation energy, the particles will be rebound, and no reaction will occur.
a)
True
b)
False
12.
With the increase in temperature, the average kinetic energy of the molecules increases, leading to a decrease in number of collisions per unit time.
a)
True
b)
False
13.
The collisions which bring about a chemical reaction are called: 
a)
Consistent collisions
b)
 Normal collisions 
c)
Effective collisions 
d)
None of the above
14.
More collisions correspond to a: 
a)
Faster reaction rate  
b)
Slower reaction rate
c)
Constant reaction rate 
d)
None of the above
15.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
16.

How could we make this reaction happen more quickly?

a)

Decrease the concentration of the acid

b)

crush the chalk to increase the surface area

c)

Put the test tube in an ice bath

17.

A temperature increase causes the particles ......

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

18.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by giving them more energy

c)

by making them more available

19.

Which of the following increase the reaction rate?

a)

less surface area

b)

lower temperature

c)

increased concentration

20.

Rank the state os matter from FASTEST to SLOWEST particle speed.

a)

solid, liquid, gas

b)

liquid, solid, gas

c)

gas, liquid, solid

d)

gas, solid, liquid

21.

The higher the temperature a substance has the

a)

more energy it has

b)

less energy it has

22.

What does a catalyst do to speed up a reaction?

a)

It reduces the surface area of the reactants

b)

It increases the surface area of the reactants.

c)

It reduces the required energy for a chemical reaction to occur

d)

It increases the required energy for a chemical reaction to occur

23.

A reactants surface area is increased. What happens?

a)

more collisions occur

b)

the same number of collisions occur

c)

greater collision energy

d)

less collision energy

e)

the same collision energy

24.

A substance that is formed as the result of a chemical reaction.

a)

products

b)

reactants

c)

catalyst

d)

collision

25.
The phase change from water vapor to liquid water is known as...
a)
evaporation
b)
precipitation
c)
condensation
d)
sublimation
26.
2. A change of state from a liquid to a solid is called....
a)
Melting
b)
Freezing
c)
Evaporation
27.

Phase change going from a Gas to a Liquid...

a)

Sublimation

b)

Deposition

c)

Ionization

d)

Condensation

28.

What state/phase is the object likely from points A to B?

a)

Solid

b)

Liquid

c)

Gas

d)

Plasma

29.

What is happening to the particles in the substance between points D and E?

a)

Melting

b)

Freezing

c)

Vaporizing

d)

Sublimating

30.

Where on the graph are phase changes taking place?

a)

1

b)

2

c)

3

d)

4

e)

5

31.
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
32.
No Definite Shape and No Definite Volume
a)
Gas
b)
Liquid
c)
Solid
33.
Definite shape and a definite volume.
a)
Gas
b)
Liquid
c)
Solid
34.
No definite shape, but has a definite volume
a)
Gas
b)
Liquid
c)
Solid
35.

Between which two points is the gas heating up?

a)

A ----> B

b)

B <---- C

c)

C ----> D

d)

D ----> E

e)

E ----> F

36.
Between which points is the temperature of the substance remaining constant?
a)
A-B only. 
b)
A-B, C-D, E-F
c)
B-C only. 
d)
B-C, D-E
37.
A substance's heating curve is shown in the graph.  What is its boiling point?
a)
100 C
b)
60 C
c)
80 C
d)
20 C
38.
The graph shows a cooling curve for an unknown substance.  What is happening during segment DE?
a)
boiling
b)
condensation
c)
freezing
d)
melting
39.
What letter represents the energy of the products?
a)
A
b)
B
c)
C
d)
D
40.
What letter represents the energy of the products?
a)
A
b)
B
c)
C
d)
D
41.
What letter represents the activation energy?
a)
A
b)
B
c)
C
d)
D
42.
Is this reaction endothermic or exothermic?
a)
endothermic 
b)
exothermic
43.

What is the ΔH of this reaction?

a)

40 kJ

b)

20 kJ

c)

80 kJ

d)

-60 kJ

44.
What is the energy of the activated complex?
a)
75 kJ
b)
225 kJ
c)
300 kJ
d)
225 kJ
45.
What letter represents ΔH?
a)
A
b)
B
c)
C
d)
D
46.
What is the sign of ΔH for all endothermic reactions?
a)
Positive
b)
Negative
47.
What is the energy of the activated complex?
a)
75 kJ
b)
225 kJ
c)
300 kJ
d)
225 kJ
48.
What is the activation energy?
a)
40 kJ
b)
20 kJ
c)
100 kJ
d)
60 kJ
49.

What is the change of the heat of the reaction (ΔH)?

a)

-40 kJ

b)

-20 kJ

c)

100 kJ

d)

60 kJ

50.
Which letter represents the activation energy?
a)
B
b)
E
c)
C
d)
D
51.
What is the PE of the reactants?
a)
100 kJ
b)
175 kJ
c)
50 kJ
d)
75 kJ
52.
What is the PE of the products?
a)
100 kJ
b)
175 kJ
c)
50 kJ
d)
75 kJ
53.
What is the activation energy?
a)
100 kJ
b)
175 kJ
c)
50 kJ
d)
75 kJ
54.

What is the change of the heat of the reaction (ΔH)?

a)

100 kJ

b)

-175 kJ

c)

-50 kJ

d)

75 kJ

55.
What type of reaction is this?
a)
Endothermic
b)
Exothermic
56.
What is the equation to measure change in Thermal Energy?
a)
Q=mc∆t
b)
Q=mc
c)
Q= ∆mct
d)
m=QC
57.
How many Joules of energy are required to change 10 gram of ice at -2 C to water at 20 C?
a)
440 J
b)
880 J
c)
10,140 J
d)
66,000 J
58.

Calculate ΔT\Delta T  when a substance goes from 10*C to 75*C

a)

-65*C

b)

75*C

c)

10*C

d)

65*C

59.

Calculate A 50g sample is heated with 500 joules of energy and has a 10*C temperature change. Calculate it’s specific heat.

a)

1 j/g*C

b)

250000 j/g*C

c)

500 j/g*C

d)

10 j/g*C

60.

4180 j of heat energy are added to change the temperature of water by 10*C. How many grams of water are being heated? cwater=4.18 j/g*C

a)

4.18 j/g*C

b)

10000g

c)

174724g

d)

100g

61.

What heat energy is required to raise the temperature of a 1g sample of mercury (cHg=.16 j/g*C) by 100*C?

a)

16j

b)

.0016j

c)

16000j

d)

625 j

62.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

63.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

64.

What is meant by HEAT OF REACTION?

a)

Energy change in a chemical reaction

b)

Energy absorbed in a chemical reaction

c)

Energy released in a chemical reaction

d)

Energy required in a chemical reaction

65.

What is the sign of ΔH for endothermic reaction?

a)

positive

b)

negative

66.

Based on the diagram, Heat energy is ___________ to the surrounding.

a)

releases

b)

absorbs

67.

Based on the diagram, which of the following is true?

a)

The reaction is endothermic

b)

Thermometer reading increases

c)

The heat energy is absorbed from surrounding

68.

The reaction between calcium nitrate solution and sodium carbonate solution is endothermic. Which of the following represents this reaction?

a)
b)
69.

The reaction between calcium nitrate solution and sodium carbonate solution is endothermic. Which of the following represents this reaction?

a)
b)
70.

Based on the diagram, total energy content of the products is _________ than total energy of the reactants.

a)

less

b)

more

71.

During a chemical reaction, chemical bonds of the reactants are __________ and new bonds in the products are ___________.

a)

formed, broken

b)

broken, formed

c)

formed, formed

d)

broken, broken

72.

This reaction is an ______________ reaction.

a)

endothermic

b)

exothermic

73.

What is the value of x?

a)

+270 kJ

b)

+200 kJ

c)

–130 kJ

d)

+130 kJ

74.

What is the type the reaction and the activation energy?

a)

Exothermic, 30 kJ

b)

Exothermic, 70 kJ

c)

Endothermic, 30 kJ

d)

Endothermic, 70 kJ

75.

Calculate the heat of formation for the following reaction under standard conditions:

C(diamond) + O2 (g) --> CO2 (g)

a)

-391.62

b)

-395.38

c)

395.38

d)

394.88

76.

What is the change in enthalpy for the following formation reaction?

NaOH(s) + HCl(g) ---> NaCl(s) + H2O(g)

a)

519 kJ

b)

-133.8 kJ

c)

133.8 kJ

d)

-519 kJ

77.

Calculate the heat of reaction of HBr → H+ + Br-. ΔHf Br- = -121 kJ, ΔHf H+ = 0 kJ, ΔHf HBr = -36 kJ.

a)

+157 kJ

b)

+85 kJ

c)

-157 kJ

d)

-85 kJ

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