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a little 8 and mostly 9

Total questions: 120

Worksheet time: 10hrs 0mins

Name
Class
Date
1.

At standard pressure and temperature, what will be the physical state of bromine?

a)

liquid

b)

gas

c)

solid

d)

plasma

2.
Which substance can not be broken down by a chemical change?
a)
ammonia
b)
methanol
c)
propane
d)
phosphorus
3.
What is the total amount of heat required to completely melt 347 grams of ice at its melting point? 
a)
334 J
b)
1450 J
c)
116000 J
d)
784000 J
4.
 Which statement describes particles of an ideal gas, based on the kinetic molecular theory? 
a)
Gas particles are separated by distances smaller than the size of the gas particles.
b)
Gas particles do not transfer energy to each other when they collide.
c)
Gas particles have no attractive forces between them. 
d)
Gas particles move in predictable, circular motion.
5.

How would you classify NaCl?

a)

element

b)

compound

c)

heterogeneous mixture

d)

homogeneous mixture

6.

Which statement accurately describes particles of an ideal gas, according to the kinetic molecular theory?

a)

The distance between the gas particles is much greater than the size of the particles

b)

As the gas particles collide, the total energy of the system increases

c)

The gas particles have strong intermolecular forces

d)

The gas particles move in a circular motion

7.

Which temperature is equal to 170 C?

a)

103 K

b)

443 K

c)

-103 K

d)

498 K

8.

What does ΔT\Delta T   stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

9.

What does q stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

10.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

11.

What type of reaction is this?

a)

Endothermic

b)

Exothermic

c)

Allergic

12.

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

13.

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

14.

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

15.

What does c stand for?

a)

Heat-Joules

b)

Mass-Grams

c)

Specific Heat-J/g*C

d)

Temperature Change-*C

16.

The potential energy diagram of a reaction is shown. Which statement below is correct relating to this reaction?

a)

#1 represents the enthalpy change for this exothermic reaction.

b)

#2 represents the enthalpy change for this endothermic reaction.

c)

#3 represents the enthalpy change for this endothermic reaction.

d)

#4 represents the enthalpy change for this exothermic reaction.

17.

During an exothermic reaction, heat content in the surroundings increases because

a)

heat energy is destroyed during reactions

b)

the reaction absorbs heat energy

c)

the energy contained in the reactants is lower then the products

d)

the energy contained in the products is lower than the reactants

18.

The amount of heat energy required to change the temperature of 12 g of gold from 45°C to 15°C is -47 J. What is the specific heat capacity of gold?

a)

0.13 J/(g°C)

b)

17,000 J/(g°C)

c)

1600 J/(g°C)

d)

0.065 J/(g°C)

19.

The graph represents the uniform heating of a substance, starting with the substance as a solid below its melting point. Which line segment listed below represents an increase in potential energy and no change in average kinetic energy?

a)

Line segment AB

b)

Line segment BC

c)

Line segment CD

d)

Line segment EF

20.
The specific heat of aluminum is 0.21 J/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
d)
0.105 J
21.
What does temperature measure?
a)
Heat
b)
ºC
c)
Kinetic Energy
d)
Thermal Energy
22.
For an endothermic reaction, the heat is on the ____ side.
a)
reactant
b)
product
c)
either side
23.
For an exothermic reaction, the heat is on the ____ side
a)
reactant
b)
product
c)
either side
24.
What type of reaction is shown in the picture?
a)
endothermic
b)
exothermic
25.
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
26.

Ice cream melting is an example of an __________ process. (heat enters the system from the surroundings)

a)

endothermic

b)

exothermic

27.

Sweating is an __________________ process because heat is released.

a)

endothermic

b)

exothermic

28.

Mass must always be in ________ for energy calculations.

a)

kilograms

b)

grams

c)

joules

d)

calories

29.

When heat flows from system to the surroundings that is an example of an ________________ process.

a)

exothermic

b)

endothermic

30.

What device is used to measure the amount of heat involved in a chemical reaction or physical process?

a)

barometer

b)

calorimeter

c)

thermometer

31.

Heat flows from _______ to _________.

a)

warm to cool

b)

cool to warm

32.

The unit for q (heat energy) can be in joules or calories. True or false?

a)

true

b)

false

33.

The law of conservation of energy states that

a)

in any chemical or physical change, energy cannot be created or destroyed, only changed in form.

b)

heat changes occur during chemical and physical changes.

c)

energy is the capacity to do work or to supply heat

d)

there are two types of energy, kinetic and potential

34.

1000 calories = ____ kcal

a)

10

b)

100

c)

1

d)

1000

35.

Which of these processes is endothermic?

a)

freezing

b)

condensation

c)

deposition

d)

sublimation

36.

A chemical reaction in a beaker causes the beaker to feel cold to the touch. What type of reaction occurred?

a)

endothermic

b)

exothermic

37.

Which of these is the unit for specific heat?

a)

J

b)

J/g

c)

J/goC

d)

oC

38.

Which of these phase changes requires energy to be released?

a)

boiling

b)

sublimation

c)

condensation

d)

melting

39.

Which type of energy is the energy stored in chemical bonds?

a)

kinetic energy

b)

potential energy

c)

chemical potential energy

d)

mechanical energy

40.

What is the specific heat of water?

a)

2.02 J/goC

b)

2.05 J/goC

c)

4.184 J/goC

d)

41.84 J/goC

41.

A piece of aluminum with a mass of 20.0 grams is heated from 30 oC to 95 oC. If the specific heat of aluminum is 0.904 J/goC, how much heat is gained by the aluminum?

a)

1717.60 J

b)

1175.20 J

c)

963.68 J

d)

542.4 J

42.

A 300 gram sample of a metal is cooled from 120 oC to 60 oC, and releases 4230 J of energy. What is the specific heat of the metal?

a)

7.61 x 107 J/goC

b)

4.26 J/goC

c)

0.47 J/goC

d)

0.235 J/goC

43.

4Fe(s) + 3O2(g) → 2Fe2O3(s) + 1625 kJ

Is this reaction endothermic or exothermic?

a)

endothermic

b)

exothermic

44.

Is the reaction represented in this graph endothermic or exothermic?

a)

endothermic

b)

exothermic

45.

A sample of H2O with a mass of 60 grams boils until it has completely changed to steam. How much heat was absorbed?

Hfus = 334 J/g

Hvap = 2260 J/g

a)

7525 J

b)

135,600 J

c)

1112.1 J

d)

20,040 J

46.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
47.

What are chemical reactions that absorb energy?

a)

endothermic

b)

fast

c)

slow

d)

exothermic

48.

What are the two main types of energy?

a)

endothermic and exothermic

b)

spontaneous and nonspontaneous

c)

potential and kinetic

d)

entropy and enthalpy

49.

Consider the reaction: 2 H2O + energy --> 2H2 + O2

a)

exothermic because releasing energy

b)

exothermic because absorbing energy

c)

endothermic because absorbing energy

d)

endothermic because releasing energy

50.
The heat required to raise the temperature of a SUBSTANCE by 1∘C
a)
calorie
b)
joule
c)
specific heat
d)
4.184 J
51.

What does temperature measure?

a)

heat

b)

average kinetic energy

c)

space

d)

time

52.

How much heat does an aluminum block absorb if 10.00 grams is heated from 25.0oC to 50.0oC? *Specific heat of aluminum is 0.900 J/goC

a)

450 J

b)

-450 J

c)

225 J

d)

-225 J

53.
Durning a phase change the temperature of a substance_________.
a)
always increases
b)
always decreases
c)
always stays the same
d)
varies
54.

The specific heat of platinum is 0.133 J/g°C. How much heat 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

55.

Releasing heat into the surroundings occurs during an ___________________ reaction.

a)

Exothermic

b)

Endothermic

c)

Kinetic Energy

d)

Thermal Energy

56.

If 238 J of heat is absorbed by a sample of metal with a mass of 40.7 g, and it raises the temperature from 20.0°C to 32.4°C, what is the specific heat capacity of the metal?

a)

2.34 J/g°C

b)

0.472 J/g°C

c)

6.13 J/g°C

d)

0.163 J/g°C

57.
Which of the following is an endothermic process?
a)
solid to gas
b)
liquid to solid
c)
solid to liquid
d)
gas to liquid
58.
In a chemical reaction, the difference between the potential energy of the products and the potential energy of the reactants is the...
a)
free energy
b)
heat of reaction
c)
heat of fusion
d)
activation energy
59.
Which of the letters (A-D) represents the potential energy of the reactants?
a)
A
b)
B
c)
C
d)
D
60.
Which of the letters (A-D) represents the potential energy of the products?
a)
A
b)
B
c)
C
d)
D
61.
What kind of reaction has a positive heat of reaction (ΔHr)?
a)
endothermic
b)
exothermic
62.
What kind of reaction has a negative heat of reaction (ΔHr)?
a)
endothermic
b)
exothermic
63.
What kind of reaction is this?
a)

endothermic

b)
exothermic
64.
Consider the reaction: 2 H2O + energy --> 2H2 + O2
a)
exothermic, releasing energy
b)
exothermic, absorbing energy
c)
endothermic, absorbing energy
d)
endothermic, releasing energy
65.
The minimum amount of energy needed to start a reaction is called the?
a)
surface energy
b)
activation energy
c)
concentration
d)
catalyst
66.
What kind of reaction moves from low PE to high PE?
a)
endothermic
b)
exothermic
67.

What happens when kinetic energy increases?

a)

Temperature increases.

b)

Temperature decreases.

c)

Temperature is not affected by kinetic energy.

68.

A sample of a compound has a mass of 30 g and a specific heat of 0.258 J/g*K. If its temperature drops 40 K, how much heat was released? ( q=mcΔTq=mc\Delta T  )

a)

309.6 J

b)

-309.6 J

c)

465 J

d)

-465 J

69.

When water evaporates, the process is...

a)

endothermic

b)

exothermic

70.

When wood is burned in a campfire, the process is...

a)

endothermic

b)

exothermic

71.

For an exothermic reaction, ΔH\Delta H  is...

a)

negative

b)

positive

72.

In the following reaction, A + 2B --> 3C, ΔH = 640 kJ\Delta H\ =\ 640\ kJ  . How much energy is needed to react 4 moles of A?

a)

2560 kJ

b)

1280 kJ

c)

1920 kJ

d)

3840 kJ

73.

In the following reaction, 2A + 2B --> C, ΔH=−60 kJ\Delta H=-60\ kJ  . What is the ΔH\Delta H  when 6 moles of A are reacted?

a)

-180 kJ

b)

-360 kJ

c)

180 kJ

d)

360 kJ

74.

If you touch an exothermic reaction, it will feel...

a)

hot

b)

cold

75.

If you touch an endothermic reaction, it will feel...

a)

hot

b)

cold

76.

The graph is showing an _________ reaction

a)

endothermic

b)

exothermic

77.
A slower particle has a lower energy than an identical, faster particle.
a)
True
b)
False
78.
When thermal energy is added to a substance, the substance's particles move:
a)
More rapidly at an increased diestance from each other.
b)
More rapidly with less distance between each other.
c)
More slowly with a greater distance between each other.
d)
More slowly with a reduced distance between each other.
79.
Thermal energy always moves:
a)
From a high temperature object to a lower temperature object.
b)
From a lower temperature object to a higher temperature object.
c)
From an object with lower kinetic energy to an object with higher kinetic energy.
d)
From an object of higher mass to an object of lower mass.
80.

Which of the following is an example of an endothermic process or reaction?

a)

condensing

b)

freezing

c)

combustion

d)

melting

81.

Which of the following is an example of an exothermic process or reaction?

a)

melting

b)

boiling

c)

photosynthesis

d)

freezing

82.

If the temperature of a sample is decreased, the particles

a)

slow down

b)

have a lower kinetic energy

c)

speed up

d)

slow down and have a lower kinetic energy

83.

What is the percent error when students find that a cheese puff has 2.8 Cal / gram and the manufacturer's value is 5.8 Cal / gram

a)

52 %

b)

48 %

c)

55 %

d)

45%

84.

Kinetic energy

a)

energy is neither created nor destroyed

b)

stored energy or energy of position

c)

energy of motion

d)

randomness in position or energy level

e)

the entropy of the universe is constantly increasing

85.

Potential energy

a)

energy is neither created nor destroyed

b)

stored energy or energy of position

c)

energy of motion

d)

randomness in position or energy level

e)

the entropy of the universe is constantly increasing

86.

What is the SI unit of heat and energy?

a)

calorie

b)

celsius

c)

joule

87.
Why does a higher temperature increase the rate of a reaction?
a)
it increases both the frequency and energy of particle collisions
b)
it only increases the frequency of particle collisions
c)
it only increases the energy of particle collisions
d)
it reduces the activation energy of the reaction
88.

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

89.

____ reactions usually feel cold.

a)

endothermic

b)

exothermic

90.
What type of reaction occurs in a hand warmer
a)
exothermic
b)
endothermic
91.

What is the ΔH of this reaction?

a)

40 kJ

b)

20 kJ

c)

80 kJ

d)

-60 kJ

92.
What letter represents ΔH?
a)
A
b)
B
c)
C
d)
D
93.
What is the activation energy?
a)
40 kJ
b)
20 kJ
c)
100 kJ
d)
60 kJ
94.
What is the PE of the reactants?
a)
100 kJ
b)
175 kJ
c)
50 kJ
d)
75 kJ
95.

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

a)

100 kJ

b)

-175 kJ

c)

-50 kJ

d)

75 kJ

96.
The faster an object moves, the ________ kinetic energy it has. 
a)
more
b)
less
c)
none of the above
d)
all of the above 
97.

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

98.

What is the name given to a catalyst in the human body?

a)

Biology

b)

Catalyst

c)

Chemical

d)

Enzyme

99.

When a catalyst is added to a reaction the rate of reaction,,,

a)

Increases

b)

Decreases

c)

Does not change

100.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy or reaction

b)

by making them more available

c)

by giving them more energy

101.

Which temperature is equal to 170 C?

a)

103 K

b)

443 K

c)

-103 K

d)

498 K

102.
The collisions which bring about a chemical reaction are called: 
a)
Consistent collisions
b)
 Normal collisions 
c)
Effective collisions 
d)
None of the above
103.
Which factors increase the rate of a reaction.
a)
increasing temperature
b)
increasing concentration
c)
increasing surface area
d)
all of these
104.
Increase in temperature of the reactants can do one of the following
a)
Slow collision frequency
b)
Allow less effective collision between the particles
c)
Neutralise the reaction
d)
increase collision between the particles thus increasing the rate.
105.
Why does a higher temperature increase the rate of a reaction?
a)
it increases both the frequency and energy of particle collisions
b)
it only increases the frequency of particle collisions
c)
it only increases the energy of particle collisions
d)
it reduces the activation energy of the reaction
106.

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

107.

When surface area is decreased the rate of reaction...

a)

Decreases, because there are LESS possible sites for correct collisions

b)

Increases, because there are LESS possible sites for correct collisions

c)

Decreases, because there are MORE possible sites for correct collisions

d)

Increases, because there are MORE possible sites for correct collisions

108.

Which has more surface area?

a)

Large chunks of chalk

b)

Cube of sugar

c)

Powdered sugar

d)

Small chunks of sugar

109.

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

a)

to slow down

b)

move faster

c)

collide higher

d)

in the right order

110.

How does a catalyst work in speeding up a reaction?

a)

By lowering the activation energy of reaction

b)

by giving them more energy

c)

by making them more available

111.

Which of the following increase the reaction rate?

a)

less surface area

b)

lower temperature

c)

increased concentration

112.

What factors effect rate of reaction?

a)

Temperature, Concentration, Pressure and Energy

b)

Surface Area, Concentration, Energy and Pressure

c)

Temperature, Pressure, Concentration and Surface area

d)

Pressure, Surface area, Density and Energy

113.
What makes an effective collision?
a)
When molecules collide.
b)
When molecules collide with the proper orientation.
c)
When molecules collide with proper orientation and enough kinetic energy.
d)
High Temperature.
114.

Why does a higher concentration increase the rate of reaction?

a)

it increases the amount of reactants

b)

it lowers the activation energy

c)

it increases the energy of particle collisions

d)

it increases the frequency of particle collisions

115.

What happens if molecules collide but not in the correct orientation

a)

Molecules always collide correctly

b)

All collisions result in products

c)

Explosion

d)

No reaction

116.
What two factors govern whether a collision between reacting particles will be effective?
a)
orientation and potential energy 
b)
kinetic energy and temperature 
c)
kinetic energy and orientation 
d)
potential energy and kinetic energy 
117.
Under the collision theory, the particles must collide with  ____ and ____ for a reaction to occur.
a)
sufficient rate and sufficient energy
b)
sufficient surface area and correct orientation
c)
sufficient catalyst and sufficient energy
d)
sufficent energy and correct orientation
118.
To slow down a chemical reaction you will do one of the following:
a)
Place the reactants in hot water
b)
Place the products in ice bath
c)
Place the reactants in a ice bath
d)
Keep stirring the reactants with a stirring rod
119.

Endothermic reactions absorb energy. How does it feel to the touch, and what happens to the temperature of the beaker/surroundings?

a)

your hand feels cool

the temperature goes up

b)

your hand feels cool the temperature goes down

c)

your hand feels warm

the temperature goes up

d)

your hand feels warm the temperature goes down

120.

Exothermic reactions release energy. What does your hand feel and what happens to temperature of the beaker/surroundings?

a)

your hand feels cool and the temperature goes down

b)

your hand feels cool and the temperature goes up

c)

your hand feels warm and the temperature goes down

d)

your hand feels warm and the temperature goes up

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