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Kinetics & Thermodynamics

Total questions: 75

Worksheet time: 1hrs 3mins

Name
Class
Date
1.
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 
2.
Decreasing the particle size increases the reaction rate because
a)
It makes particles move faster
b)
It increases the likelihood of collisions with the correct geometry
c)
It decreases the surface area available to react
d)
It increases the number of collisions
3.
If a catalyst is added to a system at equilibrium and the temperature and pressure remain constant, there will be no effect on the
a)
rate of the forward reaction
b)
activation energy of the reaction
c)
rate of the reverse reaction
d)
heat of reaction
4.
Adding a catalyst to a chemical reaction changes the rate of reaction by causing
a)
a decrease in the activation energy
b)
an increase in the activation energy
c)
a decrease in the heat of reaction
d)
an increase in the heat of reaction
5.
When one mole of a certain compound is formed from its elements under standard conditions, it absorbs 85 kiloJoules of heat. A correct conclusion from this statement is that the reaction has a
a)
ΔH equal to –85 kJ/mole
b)
ΔH equal to +85 kJ/mole
c)
 Δequal to –85 kJ/mole
d)
 Δequal to +85 kJ/mole
6.
Which interval represents the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
E
7.
Which interval represents the heat of reaction for the reaction?
a)
A
b)
B
c)
D
d)
E
8.
Interval C in this potential energy diagram could be changed by adding a ________?
a)
Cookies
b)
More energy
c)
Catalyst
d)
Changing the temperature
9.

Given the reaction:

CH4(g) + 2 O2(g) → 2 H2O(g) + CO2(g)

According to Table I, what is the overall result when CH4(g) burns according to this reaction?

a)

Energy is absorbed and H is negative.Δ

b)

Energy is absorbed and ΔH is positive.

c)

Energy is released and ΔH is negative.

d)

Energy is released and ΔH is positive

10.
In table I the reaction of hydrogen and oxygen to form water is best described as
a)
exothermic, because energy is released
b)
endothermic, because energy is released
c)
exothermic, because energy is absorbed
d)
endothermic, because energy is absorbed
11.
Which numbered interval on the diagram would change when a catalyst is added?
a)
B & C
b)
C & D 
c)
E & C
d)
A & D 
12.

Which term refers to the difference between the potential energy of the products and the potential energy of the reactants for any chemical change?

a)

heat of deposition

b)

heat of fusion

c)

heat of reaction

d)

heat of vaporization

13.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
14.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
15.
Do reactants in an endothermic reaction have a higher or lower energy than the products? 
a)
Higher
b)
Lower
16.
During an endothermic reaction in a beaker if we are part of the surroundings and touched the beaker, it would feel _______. 
a)
Warm
b)
Cold
17.

Activation energy is required to start a chemical reaction. What is activation energy?

a)

The maximum amount of energy used

b)

The minimum amount of energy required to achieve the activated complex.

c)

The energy of the reactants

d)

The energy possessed by the products

18.
What kind of reaction is this?
a)
Endothermic
b)
Exothermic
c)
Cannot be determined
19.
Which letter corresponds to the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
D
20.

What letter represents the activation energy?

a)

A

b)

B

c)

C

d)

D

21.

The addition of a catalyst to this reaction would cause a change in which of the indicated energy differences?

a)

I

b)

II

c)

III

d)

I and II

22.

The catalyst alters the rate of a chemical reaction by,

a)

providing an alternative pathway with a lower Ea

b)

changing the products formed in the direction of the reaction

c)

providing a surface on which the molecules react

d)

increasing the frequencies of collisions between molecules

23.

Which of the following statements about catalyst is true?

a)

It does not take part in the reaction

b)

It increase the yield of the reaction

c)

It provides an alternative mechanism for the reaction

d)

It increases the number of collisions between reacting molecules per second

24.
Temperature is a measure of the...
a)
total energy in a substance
b)
total kinetic energy in a substance
c)
average potential energy in a substance
d)
average kinetic energy of molecules in a substance
25.
If a chemical reaction is EXOTHERMIC, the temperature would....
a)
Stay the same
b)
Increase
c)
Decrease
26.
Exothermic reactions...
a)
Absorb energy
b)
Release energy
c)
Release Color
d)
Absorb Color
27.
What type of reaction occurs in a hand warmer
a)
exothermic
b)
endothermic
28.

When Alka-seltzer tablets are dropped in water, a gas is formed and the temperature of the water decreases. Alka-seltzer in water is an example of a

a)

Endothermic reaction

b)

Exothermic reaction

c)

Dissolving a salt

d)

physical change

29.

Enthalpy deals with the measurement of

a)

Length

b)

Area

c)

Heat energy

d)

Volume

30.

Given the change of phase:

CO2(g) —> CO2(s)

As CO2(g) changes to CO2(s), the entropy of the system

a)

decreases

b)

increases

c)

remains the same

31.

Entropy can be described as

a)

the dispersal of matter

b)

the dispersal of energy

c)

the degree of disorder

d)

all of these

32.

Which phase change represents a decrease in entropy?

a)

solid to liquid

b)

gas to liquid

c)

liquid to gas

d)

solid to gas

33.

As NaCl dissolves according to the equation

NaCl(s) → Na+(aq) + Cl-(aq), the entropy of the system

a)

Increases

b)

Decreases

c)

Remains the same

34.

Which of the following would have the highest entropy?

a)

A cold solid

b)

A hot liquid

c)

A hot gas

d)

A cold gas

35.

Which of these have a DECREASE in entropy?

a)

CaCO3(s) → CaO(s) + CO2(g)

b)

2NO2(g) → N2O4(g)

c)

2NH3(g) → 3H2(g) + N2(g)

d)

C6H6(l) → C6H6(g)

36.

The entropy will usually increase when

a)

a molecule is broken into two or more smaller molecules

b)

a reaction occurs that results in an increase in the number of moles of gas

c)

a solid changes to a liquid

d)

all of these

37.

Reactions tend to be thermodynamically favored if they are exothermic.

a)

True

b)

False

38.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
39.

Systems in nature tend to undergo changes toward

a)

lower energy and less disorder

b)

lower energy and more disorder

c)

higher energy and less disorder

d)

higher energy and more disorder

40.

Identify whether the following result in an increase or decrease in entropy:


3 moles of gas (on reactant side) --> 6 moles of gas (product)

a)

increase

b)

decrease

41.
Entropy increases from solid, liquid to gas. Why?
a)
Molecular disorder increases
b)
Molecular randomness decreases
c)
Molecules are more energetic
d)
Molecules are more reactive
42.
Which interval represents the heat of reaction for the reaction?
a)
A
b)
B
c)
D
d)
E
43.
Entropy is a measure of:
a)
order
b)
disorder
44.
When ammonium nitrate dissolves in water, the solution gets cold. Which is true?
a)
Reaction is ENDOTHERMIC with positive ΔH
b)
Reaction is ENDOTHERMIC with -ΔH
c)
Reaction is EXOTHERMIC with a -ΔH
d)
Reaction is EXOTHERMIC with +ΔH
45.
Solid magnesium dissolves in a hydrochloric acid, releasing hydrogen gas and heat from a solution of magnesium chloride. What is the sign on ΔH for this reaction?
a)
Negative because it is exothermic
b)
Negative because it is endothermic
c)
Positive because it is exothermic
d)
Positive because it is endothermic
46.

high randomness indicates _________.

a)

low entropy

b)

high entropy

47.

dissolving sugar ________-.

a)

decreases the entropy

b)

increases the entropy

48.
Spontaneous reactions are driven by
a)
increasing enthalpy and increasing entropy.
b)
decreasing enthalpy and decreasing entropy.
c)
increasing enthalpy and decreasing entropy.
d)
decreasing enthalpy and increasing entropy.
49.

Based on Table I, what is the ΔH value for the production of 1.00 mole of NO2(g) from its elements at 101.3 kPa and 298 K?

a)

33.2 kJ

b)

-33.2 kJ

c)

132.8 kJ

d)

-132.8 kJ

50.

In terms of entropy and energy, systems in nature tend to undergo changes toward

a)

lower entropy and lower energy

b)

lower entropy and higher energy

c)

higher entropy and lower energy

d)

higher entropy and higher energy

51.

Systems in nature tend to undergo changes toward

a)

lower energy and lower entropy

b)

lower energy and higher entropy

c)

higher energy and lower entropy

d)

higher energy and higher entropy

52.

A chemical reaction occurs when reactant particles

a)

are separated by great distances

b)

have no attractive forces between them

c)

collide with proper energy and proper orientation

d)

convert chemical energy into nuclear energy

53.

Given the balanced equation representing a reaction:

CH4(g) + 2O2(g) → CO2(g) + 2H2O(g) + energy

Which change in reaction conditions will increase the frequency of effective collisions between reactant molecules?

a)

decreasing the pressure of the reactants

b)

decreasing the temperature of the reactants

c)

increasing the concentration of the reactants

d)

increasing the volume of the reactants

54.

The energy absorbed and the energy released during a chemical reaction are best represented by a

a)

cooling curve

b)

heating curve

c)

kinetic energy diagram

d)

potential energy diagram

55.

The amount of randomness of the atoms in a system is an indication of the

a)

entropy of the system

b)

polarity of the system

c)

excited state of the atoms

d)

ground state of the atoms

56.

A reaction is most likely to occur when the colliding particles have proper orientation and

a)

mass

b)

volume

c)

half-life

d)

energy

57.
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.
58.
The rate of a reaction increases as temperature__________________.
a)
Decreases
b)
Increases
c)
Stays the Same
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.
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
61.
Catalysts permit reactions to proceed along a ___________energy path.
a)
lower
b)
higher
62.
Smaller particle size allows for a _________ surface area to be exposed for the reaction.
a)
larger
b)
smaller
63.
The ___________ the surface area of the reactants, the faster the reaction rate.
a)
larger 
b)
smaller
64.
Increasing the temperature will increase the kinetic energy of particles, therefore increasing the collisions between particles.
a)
false
b)
true
65.
Usually lowering the temperature will slow down a reaction.
a)
false
b)
true
66.
Increasing the concentration of the reactants will slow down the reaction.
a)
false 
b)
true
67.
Exothermic reactions release heat to the surroundings.
a)
true
b)
false
68.
A catalyst increases the efficiency of collisions between reactants.
a)
true
b)
false
69.
If the enthalpy ter (ΔH) is negative the reaction is ____.
a)
Endothermic
b)
Exothermic
c)
Neutral
70.
If ΔH is positive, heat would be shown on the _____ side of the thermochemical equation.
a)
Reactant
b)
Product
71.
C+ O2 --> CO2 + 60kJ, what is the value for ΔH for the reaction?
a)
+60
b)
-60
c)
there is no way to know
72.
How would this reaction be classified?
2Na + Cl2 → 2NaCl + 25kJ energy
a)
Exothermic
b)
Endothermic
c)
Isothermic
d)
None of the above
73.
What is true of the reaction described below?
Br2 + Cl2 + 30.0 J of energy  → 2BrCl
a)
It is exothermic because energy was released.
b)
It is endothermic because energy is absorbed.
c)
It is exothermic because energy is absorbed.
d)
It is endothermic because energy is released.
74.

Which formula would be used to calculate the enthalpy of a chemical reaction given a potential energy diagram?

a)

PEproducts + PEreactants

b)

PEreactants + PEproducts

c)

PEproducts - PEreactants

d)

PEreactants - PEproducts

75.

The enthalpy of a reaction (ΔH) is

a)

the difference in potential energy between the activated complex and the reactants.

b)

the difference in potential energy between the products and the activated complex.

c)

the sum of the potential energy contained in the products and reactants.

d)

the difference between the potential energy of the products and reactants.

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