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Energy in Reactions Review

Total questions: 70

Worksheet time: 2hrs 35mins

Name
Class
Date
1.

What type of reaction does this energy diagram represent?

a)

Endothermic

b)

Exothermic

2.

The total kinetic energy of the tiny particles that make up matter

a)

Chemical Process

b)

Products

c)

Reactants

d)

Thermal Energy

3.

When a reaction absorbs heat, we know it's an __________ reaction even though the product becomes colder.

a)

product

b)

endothermic

c)

exothermic

d)

thermal energy

4.

When a reaction releases heat, we know it's an __________ reaction even though the product becomes hotter.

a)

product

b)

endothermic

c)

exothermic

d)

thermal energy

5.

What does the "Ea" under the curve stand for?

a)

Activation Energy

b)

Endothermic Process

c)

EA Sports... IT'S IN THE GAME!

6.

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)

7.

A cast iron skillet is used to fry bacon. For optimal frying, the pan must be heated to about 178 oC from a room temperature of 22.0 oC. It is known that 1.58 x 105 J of heat energy are absorbed by the pan to reach the desired temperature and the specific heat of iron is 0.450 J/g oC. What must the mass of the skillet be?

a)

12.7 kg

b)

2.25 kg

c)

110 kg

d)

1.97 kg

8.
In an exothermic process the surrounding looses heat. 
a)
True
b)
False
9.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
10.
A reaction is performed in a beaker with a temperature probe recording the temperature changes of the reaction.  If the temperature began at 15.0 degrees Celsius and ended at 27.5 degrees Celsius.  If the reaction is our system, is the system endothermic or exothermic?
a)
Exothermic
b)
Endothermic
11.
Refer the the following question:
2N2 + 3H2 --> 2NH3 + 46 kJ
How much energy would be produced if only 1 mol of nitrogen was reacted?
a)
92 kJ
b)
0.143 kJ
c)
23 kJ
d)
15 kJ
12.
How much energy must be used to produce 4.75 mol of gaseous water?
H2O (l) +  44.0 kJ --> H2O (g)
a)
207 kJ
b)
9.36 kJ
c)
206.8 kJ
d)
9.362 kJ
13.
What mass of P4 must be reacted to produce 5905 kJ of energy?
P4 + 6Cl2 --> 4PCl3 + 2439 kJ
a)
25.43 g
b)
563.0 g
c)
2.421 g
d)
300.0 g
14.
Do reactants in an endothermic reaction have a higher or lower energy than the products? 
a)
Higher
b)
Lower
15.
Do the reactants in an exothermic reaction have a higher or lower energy than the products?
a)
Higher
b)
Lower
16.
H2 + Cl2 --> 2 HCl + 1845 kJ
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
17.
H2 + 2 C + N2 + 270.3 kJ --> 2 HCN
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
18.
Heat flows from _______ to ______ objects
a)
cooler to warmer
b)
warmer to warmer
c)
warmer to cooler
d)
cooler to cooler
19.
Energy can not be created or destroyed, it can only be transferred refers to the....
a)
law of conservation of energy
b)
law of conservation of mass
c)
life facts
d)
law of conservation of chemistry
20.
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
21.
The transfer of thermal energy between objects of different temperatures is called...
a)
temperature
b)
heat
c)
internal energy
d)
none of these
22.
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.
23.
H2 + 2 C + N2 + 270.3 kJ --> 2 HCN
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
24.
A chemical reaction that absorbs heat from the surroundings is said to be __________ and has a __________ ΔH at constant pressure.
a)
endothermic; positive
b)
endothermic; negative
c)
exothermic; negative
d)
exothermic; positive
25.
What kind of graph is this?
a)
endothermic
b)
exothermic
26.
Enthalpy is energy absorbed or relased during a chemical reaction as
a)
light.
b)
heat.
c)
sound.
d)
pressure.
27.
What is the symbol for heat?
a)
q
b)
H
c)
J
d)
∘C
28.

What is the formula for calculating heat?

a)

q = mcΔT

b)

H = ΔH x moles

c)

H = ΔH x grams

d)

products - reactants

29.

What does temperature measure?

a)

heat

b)

average kinetic energy

c)

space

d)

time

30.
Which of the letters (A-D) represents activation energy?
a)
A
b)
B
c)
C
d)
D
31.
Which of the letters (A-D) represents the potential energy of the reactants?
a)
A
b)
B
c)
C
d)
D
32.
Which of the letters (A-D) represents the potential energy of the products?
a)
A
b)
B
c)
C
d)
D
33.
Compared to the potential energy of the products, the potential energy of the reactants above is?
a)
greater than
b)
less than
c)
the same
d)
impossible to determine
34.
The minimum amount of energy needed to start a reaction is called the?
a)
surface energy
b)
activation energy
c)
concentration
d)
catalyst
35.

What is energy?

a)

moving energy

b)

stored energy

c)

renewable energy

d)

The ability to do work.

36.

What is kinetic energy?

a)

moving energy

b)

potential energy

c)

stored energy

d)

renewable energy

37.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
38.
For the reaction...
SO2 + O2  <=>  SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
a)
to the left
b)
to the right
c)
to the left and right 
d)
neither left nor right
39.
For the reaction...
SO2 + O2 <=>  SO3
If the equilibrium position shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
40.
For the reaction...
N2  +  O2  <=>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
41.
For the reaction...
N2 (g) +  3 H2 (g) <=> 2 NH3 (g)

If the pressure in the system is increased,  which substance(s) will increase in concentration?
a)
N2  (as 2 mol gas  → 4 mol gas)
b)
H2 (as 2 mol gas  → 4 mol gas)
c)
N2 and H2 (as 2 mol gas  → 4 mol gas)
d)
NH3 (as 4 mol gas  → 2 mol gas)
42.
For the reaction...
N2  +  O2  <=>  2NO:  Δ H = +182 kJ mol-1.
If the temperature is increased the equilibrium position will shift _______.
a)
to the left
b)
to the right
c)
to the left and right
d)
neither left nor right
43.
What is the Kc expression for this reaction?
   2 NO(g)  +  O2(g) ⇌  2 NO2(g)
a)
Kc = [NO2]2 / [NO]2 [O2]
b)
Kc =  [NO]2 [O2] / [NO2]2
c)
Kc = [NO]2 [O2] [NO2]2
d)
Kc = [NO2]2 / [NO]2 +  [O2]
44.
Consider the following reaction:
2SO2(g) + O2(g) <=> 2SO3(g):  ΔΗ = - 197 kJ mol -1
Which of the following will NOT shift the equilibrium position to the right?
a)
Adding more O2
b)
Adding a catalyst
c)
increasing the pressure
d)
Lowering the temperature
45.
An equilibrium constant with a large value, e.g. Kc = 1000, indicates…
a)
A very fast reaction
b)
Mostly products at equilibrium
c)
Mostly reactants at equilibrium
d)
Nothing useful at all
46.
Le Chatelier's Principle states that.... 
If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium................
a)
moves to increase the change
b)
moves to counteract the change
c)
does not change
47.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
48.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
49.
The following reaction :    
SO2 (g) +  NO2 (g) <=> SO3 (g) + NO (g)  
had reached a state of equilibrium, was found to contain  
0.40 mol L-1 SO3 , and 0.30 mol L-1 NO,
0.15 mol L-1NO2 , and 0.20 mol L-1 SO2.
Calculate the equilibrium constant  for this reaction. 
a)
4
b)
.42
c)
.25
d)
1
50.
What is the equilibrium expression for:
Fe3O4(s) + 4H2(g) <=> 3Fe(s) + 4H2O(g)
Kc =
a)
[Fe]3 [H2O]4  / [Fe3O4] [H2]4
b)
[Fe3O4] [H2]4 /  [Fe]3 [H2O]4
c)
[H2O]4 / [H2]4
d)
[Fe] [H2O] / [Fe3O4] [H2]
51.
For the reaction...
H2 (g)  + Cl2 (g) <=>  2HCl (g)  +  heat
If the pressure in the system is increased, the equilibrium position will _______.
a)
shift to the left
b)
shift to the right
c)
not shift position at all as 2 mol gas <=> 2 mol gas
52.
What are the two factors to look for when determining if the reaction is at equilibrium?
a)
Forward reaction rate is faster than the reverse and concentrations are equal
b)
Forward and reverse reaction rates are equal and concentration is conctant
c)
Forward and revers reaction rates are equal and concentration is equal
d)
Forward reaction rate is faster than the reverse and concentration is equal
53.
When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in
a)
Chemical Equilibrium
b)
Chemical Balance
c)
Chemical Constant
d)
Chemical Reaction
54.
How does a catalyst change during a reaction?
a)
It is part of the products
b)
It combines with the reactants
c)
It precipitates
d)
It remains unchanged
55.
How do catalysts increase the rate of reaction?
a)
The frequency of collisions is the increased
b)
the activation energy is lowered
c)
the energy of collisions is increased
d)
Both the frequency and energy of collisions is increased
56.

For the reaction...

SO2 + O2 ⇌ SO3

If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.

a)

left

b)

right

c)

left and right

d)

neither left or right

57.

The following factors affect the position of equilibrium EXCEPT

a)

Concentration

b)

State of Matter

c)

Temperature

d)

Pressure

58.

For the following reaction: H2(g) + Cl2 (g) ↔ 2HCl(g), calculate the concentration of HCl when Keq= 2.3x10-5, [H2]= 0.0056mol, [Cl2]= 0.0048mol.

a)

6.2 x 10-10 M

b)

2.5 x 10-5 M

c)

1.1 M

d)

1.2 M

59.
The rate of a chemical reaction is NOT affected by which of the following:
a)
temperature
b)
concentration
c)
particle size (surface area)
d)
All of these affect reaction rates
60.
The rate of a reaction increases as temperature__________________.
a)
Decreases
b)
Increases
c)
Stays the Same
61.
Products will form faster if____________
a)
the particle size of the reactants are larger.
b)
temperature is decreased.
c)
concentration of the reactants are increased.
d)
the reaction is not stirred.
62.
A ______________ is a substance that increases the rate of a reaction without being used up during the reaction. 
a)
catalyst
b)
product
c)
reactant
d)
solute
63.
Catalysts permit reactions to proceed along a ___________energy path.
a)
lower
b)
higher
64.
Smaller particle size allows for a _________ surface area to be exposed for the reaction.
a)
larger
b)
smaller
65.
The ___________ the surface area of the reactants, the faster the reaction rate.
a)
larger 
b)
smaller
66.
Increasing the temperature will increase the kinetic energy of particles, therefore increasing the collisions between particles.
a)
false
b)
true
67.
Usually lowering the temperature will slow down a reaction.
a)
false
b)
true
68.
Increasing the concentration of the reactants will slow down the reaction.
a)
false 
b)
true
69.

Enzymes in your body act as catalysts. Thus, the role of enzymes is to___________.

a)

inhibit chemical reactions.

b)

increase the rate of chemical reactions.

c)

decrease the rate of chemical reactions.

70.

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

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