wayground logo

Free Printable Worksheets

Font size

S
M
L
XL
Worksheets

Kinetics, Thermodynamics & Equilibrium (focus on Le Chatlier's)

Total questions: 70

Worksheet time: 2hrs 49mins

Name
Class
Date
1.
2SO2(g)+O2(g)⇌2SO3(g) is an exothermic reaction.
an in Increase temperature will...
a)
shift equilibrium toward the right
b)
shift equilibrium toward the left
c)
increase pressure
d)
have no change
2.
An endothermic process the system _________ heat as the surroundings _______ heat. 
a)
gains, lose
b)
loses, gain
c)
gains, gain
d)
loses, lose
3.
The three factors that affect the equilibrium of a reaction are temperature, pressure and __________. 
a)
energy
b)
concentration 
c)
enthalpy 
d)
ice 
4.
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 nor right
5.
At what time does the reaction reach equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
6.
During equilibrium, the rates of the forward and the reverse reaction are ________
a)
the same 
b)
unequal
c)
unequal for exothermic reactions
d)
unequal for endothermic reactions
7.
The idea that when a system at equilibrium is stressed, it will react to relieve that stress and return to equilibrium is known as:
a)
Boyle's Law
b)
Le Chatelier's Principle
c)
Charles Law
d)
Denninger's Law
8.
Le Chaltelier's Principle states that if a chemical system at equilibrium is stressed,
a)
the system will adjust to increase the stress
b)
the system will adjust to reduce the stress
c)
the system will not adjust
9.

When you increase the pressure on an equilibrium system the system will shift to the side with ______.

a)

least amount of heat

b)

least moles of gas

c)

least moles

10.

Use the reaction below to answer question:

N2O4(g) ⇌ 2NO2 (g) ΔH = + 92 KJ


Which way will the reaction shift if pressure is increased?

a)

Left

b)

Right

c)

No shift

11.
Why is equilibrium called a dynamic state?
a)
Chemists try to convert as much reactants as possible into products.
b)
The reactions at equilibrium continue to take place once equilibrium is established.
c)
The products of a forward reaction are favored, so equilibrium lies to the right.
d)
All chemical reactions are considered to be reversible under suitable conditions.
12.
When writing an endothermic reaction, heat energy is stated as
a)
product
b)
catalyst
c)
reactant
13.
An exothermic reaction is allowed to reach equilibrium. If heat energy is then removed, the equilibrium will shift
a)
toward the middle
b)
toward the reactant side
c)
toward the product side
14.
When  ΔH is positive it represents a(n) 
a)
exothermic   reaction 
b)
endothermic reaction 
15.
The three factors that affect the equilibrium of a reaction are temperature, pressure and __________. 
a)
energy
b)
concentration 
c)
enthalpy 
d)
ice 
16.
When  ΔH  is negative it represents a(n)
a)
exothermic reaction 
b)
endothermic reaction 
17.

2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g)

Removing O2 (g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

decrease temperature

d)

have no change

18.

2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g)

Adding SO2 (g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase rate of reaction

d)

have no change

19.

2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g)

Removing SO3 (g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

20.

2 SO2 (g) + O2 (g) ⇌ 2 SO3 (g) is an exothermic reaction.

An increase in temperature will...

a)

shift equilibrium toward the right

b)

shift equilibrium toward the left

c)

increase pressure

d)

have no change

21.
For the reaction...
heat  +  N2(g)  +  O2(g)  <−>  2NO(g)
If the heat is removed to the chemical system, the equilibrium will _______.
a)
shift to the left
b)
shift to the right
c)
not shift
22.
For the reaction...
N2 (g) +  3 H2 (g) <−> 2 NH3 (g)

If the pressure in the system is increased, the reaction will __________________.
a)
 shift to the left
b)
shift to the right
c)
not shift
23.

If CH4(g) is increased in the reaction:

CH4(g) + 2O2(g) <--> CO2(g) + 2H2O(l)

How will equilibrium shift?

a)

Towards the reactants

b)

Towards the products

24.

If CO2(g) is increased in the reaction:

CH4(g) + 2O2(g) <--> CO2(g) + 2H2O(l)

How will equilibrium shift?

a)

Towards the reactants

b)

Towards the products

25.

If heat energy is increased in the reaction:

CH4(g) + 2O2(g) <--> CO2(g) + 2H2O(l) + heat

How will equilibrium shift?

a)

Towards the reactants

b)

Towards the products

26.

If heat energy is removed in the reaction:

CH4(g) + 2O2(g) <--> CO2(g) + 2H2O(l) + heat

How will equilibrium shift?

a)

Towards the reactants

b)

Towards the products

27.

Use the equation:

C(s) + O2(g) <--> CO2(g) + heat


If a catalyst were to be added to this system what would happen?

a)

Shift towards reactants

b)

Shift towards products

c)

No shift

28.

Use the equation:

C(s) + O2(g) <--> CO2(g) + heat


If temperature in this closed system decreased how would equilibrium shift?

a)

Shift towards reactants

b)

Shift towards products

c)

No shift

29.

Use the equation:

C(s) + O2(g) <--> CO2(g) + heat


If temperature in this closed system increased how would equilibrium shift?

a)

Shift towards reactants

b)

Shift towards products

c)

No shift

30.

Use the equation:

C(s) + O2(g) <--> CO2(g) + heat


If carbon dioxide gas concentration in this closed system increased how would equilibrium shift?

a)

Shift towards reactants

b)

Shift towards products

c)

No shift

31.

Use the equation:

C(s) + O2(g) <--> CO2(g) + heat


If carbon dioxide gas concentration in this closed system decreased how would equilibrium shift?

a)

Shift towards reactants

b)

Shift towards products

c)

No shift

32.

Use the equation:

C(s) + O2(g) <--> CO2(g) + heat


If the solid carbon concentration in this closed system decreased how would equilibrium shift?

a)

Shift towards reactants

b)

Shift towards products

c)

No shift

33.

Use the equation:

C(s) + O2(g) <--> CO2(g) + heat


If the solid carbon concentration in this closed system increased how would equilibrium shift?

a)

Shift towards reactants

b)

Shift towards products

c)

No shift

34.

What is true about chemical equilibrium? Check all that apply.

a)

The rate of the forward reaction is equal to the rate of the reverse reaction

b)

A double arrow, <-->, is used

c)

It occurs in a closed system

d)

The rate of bonds breaking is equal to the rate of bonds forming

35.

What is true about chemical equilibrium? Check all that apply.

a)

The rate of the forward reaction is equal to the rate of the reverse reaction

b)

A double arrow, <-->, is used

c)

It occurs in a closed system

d)

The rate of bonds breaking is equal to the rate of bonds forming

36.

What is true about chemical equilibrium? Check all that apply.

a)

The rate of the forward reaction is equal to the rate of the reverse reaction

b)

A double arrow, <-->, is used

c)

It occurs in a closed system

d)

The rate of bonds breaking is equal to the rate of bonds forming

37.

What is true about chemical equilibrium? Check all that apply.

a)

The rate of the forward reaction is equal to the rate of the reverse reaction

b)

A double arrow, <-->, is used

c)

It occurs in a closed system

d)

The rate of bonds breaking is equal to the rate of bonds forming

38.

What is true about chemical equilibrium? Check all that apply.

a)

The rate of the forward reaction is equal to the rate of the reverse reaction

b)

A double arrow, <-->, is used

c)

It occurs in a closed system

d)

The rate of bonds breaking is equal to the rate of bonds forming

39.

Is the following reaction endo or exothermic? USE TABLE I


4Al(s) + 3O2(g) <--> 2Al2O3(s)

a)

Endothermic

b)

Exothermic

40.

Is the following reaction endo or exothermic? USE TABLE I


H2(g) + I2(g) <--> 2HI

a)

Endothermic

b)

Exothermic

41.

Is the following reaction endo or exothermic? USE TABLE I


2C(s) + 2H2(g) <--> C2H4(g)

a)

Endothermic

b)

Exothermic

42.

Is the following reaction endo or exothermic? USE TABLE I


LiBr(s) <-H2O-> Li+(aq) + Br-(aq)

a)

Endothermic

b)

Exothermic

43.
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
44.
Two reactant particles collide with proper orientation.The collision will be effective if the particles have
a)
high activation energy
b)
high ionization energy
c)
sufficient kinetic energy
d)
sufficient potential energy
45.
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
46.
A piece of Mg(s) ribbon is held in a Bunsen burnerflame and begins to burn according to the equation:
2Mg(s) + O2 (g)  −>   2MgO(s).
The reaction begins because the reactants
a)
are activated by heat from the Bunsen burner flame
b)
are activated by heat from the burning magnesium
c)
underwent an increase in entropy
d)
underwent a decrease in entropy
47.

Compared to the rate of inorganic reactions, the rate of organic reactions generally is

a)

slower because organic particles are ions

b)

slower because organic particles contain covalent bonds which take a long time to break

c)

faster because organic particles are ions

d)

faster because organic particles contain covalent bonds

48.
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
49.
Which interval represents the activation energy of the forward reaction?
a)
A
b)
B
c)
C
d)
E
50.
Which interval represents the heat of reaction for the reaction?
a)
A
b)
B
c)
D
d)
E
51.
Interval C in this potential energy diagram could be changed by adding a ________?
a)
Cookies
b)
More energy
c)
Catalyst
d)
Changing the temperature
52.

Given the reaction:

CH4(g) + 2 O2(g) --> 2 H2O(g) + CO2(g)

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

53.

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

54.
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 
55.
Which term refers to the difference between thepotential energy of the products and the potential energy ofthe reactants for any chemical change?
a)
heat of deposition
b)
heat of fusion
c)
heat of reaction
d)
heat of vaporization
56.
Which is a factor that would not affect the rate of a reaction?
a)
Temperature
b)
Adding a catalyst
c)
Concentration
d)
The weather
57.
Which picture shows how a catalyst would change the rate? 
a)
Option 3
b)
Option 2
c)
Option 1
58.

Temperature is a measure of average ________ energy of individual atoms.

a)

heat

b)

potential

c)

mechanical

d)

kinetic

59.
ΔH value in an endothermic reaction is a positive number.
a)
True
b)
False
60.

Given the equation representing a reaction at equilibrium:

N2(g) + 3H2(g) --> 2NH3(g) + energy

Which change causes the equilibrium to shift to the right?

a)

decreasing the concentration of H2(g)

b)

decreasing the pressure

c)

increasing the concentration of N2(g)

d)

increasing the temperature

61.
Given the reaction at equilibrium: 
Which change will not affect the equilibrium concentrations of A(g), B(g), and A2B3(g)?
a)
adding more A(g)
b)
adding a catalyst
c)
increasing the temperature
d)
increasing the pressure
62.
Ammonia is produced commercially by the Haber reaction:   N2 + 3 H2 -->  2 NH3
The formation of ammonia is favored by
a)
an increase in pressure
b)
a decrease in pressure
c)
removal of N2(g)
d)
removal of H2(g)
63.

Which statement is true for a saturated solution at equilibrium?

a)

It must be a concentrated solution.

b)

It must be a diluted solution.

c)

Neither dissolving nor crystallizing is occurring.

d)

The rate of dissolving equals the rate of crystallizing.

64.
Given the reaction at equilibrium:
N2(g) + 3H2(g) ↔ 2NH3(g)
Increasing the concentration of N2(g) will increase the foward reaction rate due to
a)
a decrease in the number of effective collisions
b)
an increase in the number of effective collisions
c)
a decrease in the activation energy
d)
an increase in the activation energy
65.
Given the reaction at equilibrium:
N2(g) + O2(g) ↔ 2NO(g)
As the concentration of N2(g) increases, the concentration of O2(g) will
a)
decrease
b)
increase
c)
remain the same
66.
Given the reaction system in a closed container at equilibrium and at a temperature of 298 K:
N2O4 (g)  <-->  2NO2 (g)
The measurable quantities of the gases at equilibrium must be
a)
decreasing
b)
increasing
c)
equal
d)
constant
67.
Will grinding up a solid increase or decrease the rate of reaction?
a)
increase
b)
decrease
68.
What kind of reaction is this?
a)
Endothermic
b)
Exothermic
c)
Cannot be determined
69.

Check all of the following that can increase the rate of a chemical reaction:

a)

less surface area

b)

lower temperature

c)

increasing pressure

d)

increased concentration

70.
Which phase of matter has the greatest motion and least orderly arrangement?
a)
solid
b)
liquid
c)
gas

Similar Resources on Wayground

ÔN TẬP GHKI - HÓA 11- 24-25

68 questions

ÔN TẬP GHKI - HÓA 11- 24-25

quiz

Worksheet

•

11th Grade

Ionic and Covalent Bonds

66 questions

Ionic and Covalent Bonds

quiz

Worksheet

•

9th Grade

Practice Chemistry Regents (326)

69 questions

Practice Chemistry Regents (326)

quiz

Worksheet

•

12th Grade

Woleslagle - Honors Kinetics

70 questions

Woleslagle - Honors Kinetics

quiz

Worksheet

•

10th Grade

Year 9 Ultimate Exam revision

68 questions

Year 9 Ultimate Exam revision

quiz

Worksheet

•

9th Grade

VSEPR & Molecular Geometry

68 questions

VSEPR & Molecular Geometry

quiz

Worksheet

•

10th - 12th Grade

C1 - Review: Atomic History & Structure, Isotopes, Ions

66 questions

C1 - Review: Atomic History & Structure, Isotopes, Ions

quiz

Worksheet

•

10th Grade

Periodic Table and Atomic Structure Review

65 questions

Periodic Table and Atomic Structure Review

quiz

Worksheet

•

10th Grade