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Thermodynamics, Kinetics and Equilibrium Review

Total questions: 60

Worksheet time: 1hrs 19mins

Name
Class
Date
1.
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
2.
The transfer of thermal energy between objects of different temperatures is called...
a)
temperature
b)
heat
c)
internal energy
d)
none of these
3.
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.
4.
A substance with a high specific heat:
a)
Is always extremely hot.
b)
Requires a lot of energy to become hot.
c)
Is not heavy.
d)
Does not requires a lot of energy to become hot.
5.
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.
6.
The temperature of a glass of cold water will eventually...
a)
Match the temperature of the surrounding environment.
b)
Always be colder than the surrounding environment.
c)
Become warmer than the surrounding environment.
d)
Never change temperature.
7.
In which of the following systems is entropy increasing?
a)
Putting together a puzzle
b)
Putting books on a shelf
c)
Breaking a plate
d)
Filling a jar of salt
8.
The measure of average kinetic energy of all the particles within an object is called ____________. 
a)
temperature
b)
conduction
c)
radiation
d)
heat 
9.
Exothermic reactions...
a)
Absorb energy
b)
Release energy
c)
Release Color
d)
Absorb Color
10.
What happens to the bonds when 2 substances react
a)
They break so new bonds can form
b)
Nothing the bonds are too strong
c)
They change colour
11.
If they energy required to break the bonds is greater than the energy given out by making new bonds the reaction is
a)
Exothermic
b)
Endothermic
c)
Neutralisation
12.
If they energy required to break the bonds is greater than the energy given out by making new bonds the reaction is
a)
Exothermic
b)
Endothermic
c)
Neutralisation
13.
If they energy required to break the bonds is less than the energy given out by making new bonds the reaction is
a)
Exothermic
b)
Endothermic
c)
Neutralisation
14.

Two liquids of different temperatures are separated by a barrier. The hot liquid is on the left side and the cold one is on the right side. Which of the following describes how the molecules move in heat flow?

a)

Molecules from the left collide and transfer heat directly to the right side.

b)

Molecules from the left collide and transfer heat to the barrier, which transfers heat to the right side.

c)

Molecules from the right collide and transfer heat to the barrier, which transfers heat to the left side.

d)

Molecules from the right collide and transfer heat directly to the right side.

15.

Which of the following is the abbreviation for a unit of energy?

a)

K

b)

J

c)

N

d)

oC

16.

The amount of heat needed to raise the temperature of 25 g of a substance by 15°C is 915 J. What is the specific heat of the substance?

a)

2.05 J/g-°C

b)

2.44 J/g-°C

c)

2.13 J/g-°C

d)

2.22 J/g-°C

17.

A 200 g block of a substance requires 1.84 kJ of heat to raise its temperature from 25°C to 45°C. Use the table to identify the substance.

a)

gold

b)

aluminum

c)

iron

d)

copper

18.

According to the table, which gas would be most efficient—that is, have the greatest heat-storing ability—for transferring heat from a heat source to a heat exchanger?

a)

oxygen

b)

air

c)

hydrogen

d)

steam

19.

In the diagram, which letter represents the transition from liquid to gas?

a)

E

b)

B

c)

C

d)

D

20.

Enthalpy deals with the measurement of

a)

Length

b)

Area

c)

Heat energy

d)

Volume

21.
The amount of thermal energy required to raise the temperature of one (1) kilogram of a substance by 1o C is known as:
a)
Specific heat
b)
Heat of fusion
c)
Heat of vaporization
d)
Melting point
22.
It take 1.25 kJ of energy to heat a sample of silver (c = 0.24J/goC) from 12.0oC to 15.2oC.  What was the mass of the sample?
a)
960 g
b)
1628 g
c)
1.63 g
d)
567 g
23.
What is the correct formula to convert Celsius to Kelvin?
a)
K=C-273
b)
K=C+273
c)
K=C-100
d)
K=C+100
24.
H2 + Cl2 --> 2 HCl + 1845 kJ
Is this reaction endothermic or exothermic?
a)
Endothermic 
b)
Exothermic
25.
Which phase of matter has the greatest motion and least orderly arrangement?
a)
solid
b)
liquid
c)
gas
26.
If ΔH is positive, heat energy would be shown on the _____ side of the equation.
a)
reactant
b)
product
27.

Which of the following is (are) altered when a liquid at its boiling point is converted to a gas at the same temperature?

I. The size of the molecules

II. The distance between molecules

III. The average kinetic energy of the molecules

a)

I only

b)

II only

c)

III only

d)

I and II

28.
A catalyst works by
a)
changing the order of the reaction
b)
increasing the temperature
c)
lowering the activation energy
d)
making the activated complex
29.

If the temperature is reduced, a reaction rate will ______

a)

increase

b)

decrease

c)

stay the same

30.

If the concentration of a reactant is increased, the reaction rate will ___________.

a)

increase

b)

decrease

c)

stay the same

31.
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)
Cause particles to lose speed
d)
Increase collision between the particles thus increasing the rate.
32.
Which of these will NOT speed up the rate of reaction between a strip of magnesium and hydrochloric acid?
a)
tightly coil up the strip of magnesium
b)
cut up the strip of magnesium
c)
increase the concentration of the hydrocholoric acid
d)
increase the temperature of the hydrocholoric acid
33.
Grinding a seltzer tablet into powder increases the rate of reaction due to...
a)
increased concentration of reactants
b)
increased surface area
c)
increased speed of particles.
d)
better orientation of reactants
34.
What is the activation energy?
a)
The energy of the products
b)
The energy of the reactants
c)
The minimum energy needed by the reactants to form the products.
d)
The energy lost in the reaction
35.

Which of the following are true when a catalyst is used in a chemical reaction?

a)
  • Enthalpy of reaction is lower.
  • Activation energy for the reaction is lower.
b)
  • Enthalpy of reaction is same.
  • Activation energy for the reaction is lower.
c)
  • Enthalpy of reaction is the lower.
  • Activation energy for the reaction is same.
d)
  • Enthalpy of the reaction is same.
  • Activation energy for the reaction is same.
36.

Which of the following is a condition for effective collisions to occur?

a)

Particles should have enough energy

b)

Particles should be correctly oriented

c)

Both answers are correct

37.
Which letter corresponds to the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
D
38.
A+B →C+D    ΔH = -202kj/mol
How can above reaction be classified in terms of energy exchange during chemical change? 
a)
Combination reaction
b)
Endothermic reaction
c)
Transthermal reaction
d)
Exothermic reaction
39.
What is the rate equation of following chemical reaction?
2NaOH + H2SO4 → Na2SO4 + 2H2O
a)
Rate = k.[NaOH]2.[H2SO4]
b)
Rate = k.[NaOH].[H2SO4]
c)
Rate = k.[NaOH]2
d)
Rate = k.[NaOH]2.[H2SO4]2
40.

4 factors that affects reaction rate.

a)

temperature

b)

surface area

c)

presence of catalyst

d)

Chemical nature of reactant

e)

In solid form

41.

Which of the following are true of reaction rates?


I. The overall rate law is determined by the fastest step of a reaction


II. The presence of a catalyst will increase the number of molecules entering the transition state


III. An increase in temperature will increase the rate of a reaction


IV. Increasing the concentration of reactants will increase the rate at which products yield

a)

II+III+IV

b)

I+IV

c)

II + III

d)

I+II+III

42.

The iodide ion reacts with hypochlorite ion in the following way:

OCl- + I- ⟶ OI- + Cl-.

This rapid reaction gives the rate data shown. What is the rate law?

a)

rate = [OCl-]2[I-]

b)

rate = [OCl-][I-]2

c)

rate = [OCl-][I-]

d)

rate = [OCl-]

43.

Which of the following best describes why increasing temperature increase reaction rate?

a)

Activation energy is reduced.

b)

Collisions become more frequent.

c)

Collisions become more energetic.

d)

Collisions become more frequent and more energetic.

44.

An addition of a catalyst to the following reaction would have what effect?

a)

A would be increased

b)

B would be increased

c)

C would be decreased

d)

No change

45.
It is a chemical reaction where the reactants form products that, in turn, react together to give the reactants back.
a)
reversible reaction
b)
irreversible reaction
c)
decomposition reaction
d)
synthesis
46.
What is the equilibrium expression for:
Fe3O4(s) + 4H2(g) <--> 3Fe(s) + 4H2O(g)
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])
47.
When Keq > 1, 
a)
There are more products than reactants when the reaction reached equilibrium.
b)
There are more reactant than products when the reaction reached equilibrium.
c)
The amount of reactants is equal to the amount of products.
48.
Keq < 1
a)
There are more products than reactants when the reaction reached equilibrium.
b)
There are more reactant than products when the reaction reached equilibrium.
c)
The amount of reactants is equal to the amount of products.
49.
Define chemical equilibrium.
a)
A reaction is reversible.
b)
The concentration of the reactants is equal to the concentration of the products.
c)
The rate of a forward reaction is equal to the rate of the reverse reaction.
d)
The reaction stops and no further change in concentration occurs.
50.
For the reaction...
SO2 + O2 <−>  SO3
If the equilibrium shifts to the left, the concentration of SO3 will ___________.
a)
increase
b)
decrease
c)
stay the same
d)
triple
51.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If  NO is removed  from the system, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
52.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
left and right
d)
neither left nor right
53.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is removed to the chemical system, the equilibrium will shift _______.
a)
left
b)
right
c)
both left and right
d)
neither left nor right
54.
For the reaction...
H2 (g)  + Cl2 (g) <−>  2HCl (g)  +  heat
If the pressure in the system is increased, the equilibrium will _______.
a)
shift left
b)
shift right
c)
not shift
55.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased,  _______ reaction will be favored.
a)
 the forward
b)
the reverse
c)
neither
56.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased,  which substance will increase in concentration?
a)
N2
b)
H2
c)
N2 and H2
d)
NH3
57.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is decreased,  which substance will increase in concentration?
a)
N2
b)
H2
c)
N2 and H2
d)
NH3
58.
Which of the following is NOT true at equilibrium?
a)
The forward and reverse reactions proceed at the same rate.
b)
The concentrations of reactants and products do not change.
c)
The concentration of the reactants is equal to the concentration of the products.
d)
The forward and reverse reactions continue to occur.
59.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
d)
plasma
60.
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 constant
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

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