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Le Chatetier's Principle and equilibrium

Total questions: 50

Worksheet time: 1hrs 16mins

Name
Class
Date
1.

What two factors indicate that a reaction is at equilibrium?

a)

Concentrations are equal; the forward and reverse reactions are equal

b)

The concentrations are constant; the forward and reverse reactions are equal

c)

The concentrations are equal; the forward reaction is faster than the reverse reaction

d)

The concentrations are constant; the forward reaction is faster than the reverse reaction

2.

A double sided arrow (↔), indicates that a reaction is: (a)  

Choose from the below words
Reversible
Irreversible
Not reactive
3.

When the forward and reverse reactions are occurring at the same rate, the reaction is said to be at:

a)

Chemical equilibrium

b)

Chemical reaction

c)

Chemical constant

d)

Chemical peace

4.

If a reversible reaction has reached equilibrium, which of the following is true about the concentration of the reactants vs the products?

a)

Some reactants are present, as are some prooducts

b)

Only reactant is present, there are no products

c)

Only product is present, there are no reactants

5.

Which of the following is true if the value of the equilibrium constant, K, is greater than 1

a)

Products are favored over reactants

b)

Reactants are favored over products

c)

Reactants and products are equally favored

6.

Which of the following is true if the value of the equilibrium constant, K, is less than 1

a)

Products are favored over reactants

b)

Reactants are favored over products

c)

Reactants and products are equally favored

7.

How does a catalyst affect equilibrium?

a)

It makes the reaction occur faster, and makes the equilibrium shift to make more products

b)

It makes the reaction occur faster, but does not shift the placement of the equilibrium

c)

It does not change the rate of the reaction, but makes the equilibrium shift to make more products

d)

A catalyst has no effect on the rate of a reaction or the placement of the equilibrium

8.

Which of the following factors has no effect on the position of the chemical equilibrium for a reaction?

a)

Pressure

b)

Temperature

c)

Catalyst

d)

Concentration

9.

N2(g) + 3H2(g) ↔ 2 NH3(g) + heat

Adding H2 will cause the equilibrium to:

a)

Shift right

b)

Shift left

c)

Have no change

d)

Speed up

10.

N2(g) + 3H2(g) ↔ 2 NH3(g) + heat

Increasing the temperature will cause the equilibrium to:

a)

Shift right

b)

Shift left

c)

Have no change

d)

Speed up

11.

N2(g) + 3H2(g) ↔ 2 NH3(g) + heat

Removing N2 will cause the equilibrium to:

a)

Shift right

b)

Shift left

c)

Have no change

d)

Speed up

12.

N2(g) + 3H2(g) ↔ 2 NH3(g) + heat

Increasing the volume of the container (decreasing the pressure) will cause the equilibrium to:

a)

Shift right

b)

Shift left

c)

Have no change

d)

Speed up

13.

N2(g) + 3H2(g) ↔ 2 NH3(g) + heat

Increasing the pressure will cause the equilibrium to:

a)

Shift right

b)

Shift left

c)

Have no change

d)

Speed up

14.

N2(g) + 3H2(g) ↔ 2 NH3(g) + heat

Increasing the pressure causes the equilibrium to shift right. Why?

a)

To increase the pressure more, because there are fewer moles of gas in the products

b)

Because this makes the equilibrium constant, K, increase

c)

To reduce the pressure, because there are fewer moles of gas in the products

d)

To reduce the pressure, because there are more moles of gas in the products

15.
At what time (in seconds) is equilibrium established?
a)
0 seconds
b)
1 second
c)
5 seconds
d)
10 seconds
16.
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
17.
When writing an endothermic reaction, heat energy is stated as
a)
product
b)
catalyst
c)
reactant
18.
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
19.
For the reaction...
SO2(g) + O2(g) <−>  SO3(g)
If the concentration of SO2(g)  is increased, the equilibrium of the reaction will ___________.
a)
shift to the left
b)
shift to the right
c)
not shift
20.
For the reaction...
SO2(g) + O2(g) <−>  SO3(g)
If the equilibrium shifts to the right, the concentration of O2(g) will ___________.
a)
increase
b)
decrease
c)
remain the same
21.
For the reaction...
energy +  N2(g)  +  O2(g)  <−>  2NO(g)
If  O2(g) is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
22.
A +  B <--> C + D   ΔH= 151kJ
Rewrite the above equation with energy as a reactant or product:
a)
A +  B <--> C + D + energy
b)
A +  B + energy <--> C + D 
23.
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
24.
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
25.
When  ΔH  is negative it represents a(n)
a)
exothermic reaction 
b)
endothermic reaction 
26.
  A(g) + B(aq) <> C(s) 
 ΔHrxn= -453 kJ/mol
If the [B] is decreased then the reaction is will shift to the _______. 
a)
Left
b)
Right
c)
Stays the same 
d)
Up
27.
What is the proper Keq for the following reaction? 
   2 NO(g)  +  O2(g) ⇌ 2 NO2(g)
a)
Keq = [NO2]2 / [NO]2[O2]
b)
Keq =  [NO]2[O2] / [NO2]2
c)
Keq = [NO]2[O2][NO2]2
d)
Keq = 2[NO][O2] / 2[NO2]
28.
What is [A] and [B]?
a)
Concentration of Reactants
b)
Concentration of Products
c)
Energy of Reactants
d)
Energy of Products
29.
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.
30.
Given: 2A(g) <-> 2B(g) + C(g). At a particular temperature, K = 1.6x104.
Raising the pressure by lowering the volume of the container will...
a)
cause [A] to increase
b)
cause [B] to increase
c)
have no effect
d)
cannot be determined
31.
2SO2(g)+O2(g)⇌2SO3(g)
Removing O2(g) will
a)
shift equilibrium right
b)
shift equilibrium left
c)
decrease temperature
d)
have no change
32.

Increasing the pressure on an equilibrium system will

a)

shift the reaction to the side with more moles of chemicals

b)

shift the reaction to the side with more moles of gas

c)

shift the reaction to the side with fewer moles of gas

d)

shift the reaction to the side with fewer moles of chemicals

33.

If an equilibrium constant, K, is 1.8 x 10-5, at equilibrium

a)

I will have more reactants

b)

I will have more products

c)

I will have roughly equal amounts of reactants and products

d)

it is impossible to tell how much reactants and products I will have

34.

For the reaction below, (metane gas reacting with dihydrogen sulfide) which change would cause the equilibrium to shift to the right?

CH4(g) + 2H2S(g) + heat↔ CS2(g) + 4H2(g)

a)

Decrease the concentration of dihydrogen sulfide.

b)

Increase the pressure on the system.

c)

Increase the temperature of the system.

d)

Increase the concentration of carbon disulfide.

e)

Decrease the concentration of methane.

35.

Consider the following reaction:

Fe +3 + SCN ↔ FeSCN 2+

(Light Yellow) (Deep Red)

Adding Fe(NO3)3 produced the following change in the equilibrium:

a)

The color in the test tube became a deeper red color because the equilibrium shifted to make more reactants.

b)

The color in the test tube became a deeper red color because the equilibrium shifted to make more products.

c)

The color in the test tube became a lighter color because the equilibrium shifted to make more reactants.

d)

The color in the test tube became a lighter color because the equilibrium shifted to make more products.

36.

Consider the following reaction:

Fe +3 + SCN ↔ FeSCN 2+

(Light Yellow) (Deep Red)

The reaction you studied became a deeper red color when placed in an ice bath. This means that the reaction is

a)

exothermic.

b)

endothermic.

c)

There is not enough information given to answer the qusestion.

d)

None of the above are correct.

37.

In the reaction, CO (g) + NO2 (g) ↔ CO2 (g) + NO (g), which of the following changes would result in the formation of more products at equilibrium?

a)

increasing the pressure

b)

removing CO (g) from the reaction

c)

adding NO2 (g) to the reaction

d)

adding CO2 to the reaction.

e)

None of the options would result in more products.

38.
Which is the reactant - and why?
a)
A, as concentration decreases
b)
B, as concentration decreases
c)
A, as concentration increases
d)
B, as concentration increases
39.
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
40.
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]
41.
N2O4(g) ↔ 2 NO2(g)
What is the concentration equilibrium constant expression?
a)
Kc = [NO2]2/[N2O4]
b)
Kc = [N2O4]/[NO2]2
c)
Kc = [N2O4]2/[NO2]
d)
Kc = [NO2]/[N2O4]2
42.
What is the equilibrium-constant expression for 
CO2(g) + H2(g) ↔ CO(g) + H2O(l)
a)
Kc= [CO][H2O] / [CO2][H2]  
b)
Kc= [CO2][H2] / [CO]
c)
Kc= [CO2][H2] / [CO][H2O]
d)
Kc= [CO] / [CO2][H2]  
43.
Consider the following reaction. What would be the equilibrium constant expression?
4Br2(g) + CH4(g) ↔  4HBr(g) + CBr4(g)
a)
[Br2]4  [CH4]/ [HBr]4  [CBr4]
b)
[HBr]4 [CBr4]/ [Br2]4 [CH4]
c)
[HBr ]/ [Br2]4 [CH4]
d)
[HBr]4 [CBr4]/ [Br2]4 [CH]4
44.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
45.
2A + 3B  <---->  2AB
The forward reaction points towards the __________.
a)
left
b)
right
c)
up
d)
down
46.
Equilibrium constant for the reaction below can be expressed as
a)
Kc = [A][B]/[C][D]
b)
Kc = [C][D]/[A][B]
c)
Kc = [AB]/[CD]
d)
Kc = [CD]/[AB]
47.

What is the reaction/equation for this Kc expression

a)

2N2 + O2 ⇌ 2NO

b)

N2 + O2 ⇌ NO

c)

NO ⇌ 2NO

d)

N2 + O2 ⇌ 2NO

48.

What is the equation/reaction for this Kc expression?

a)

O3 ⇌ 3O2

b)

2O3 ⇌ 3O2

c)

2O3 ⇌ O2

d)

3O2 ⇌ 2O3

49.

If Kc is large that means the concentration of the __________ is high and therefore the concencentration of the __________ is low.

a)

reactants, products

b)

species, products

c)

products, reactants

d)

species, reactants

50.
An equilibrium constant with a large magnitude indicates…
a)
A very fast reaction
b)
Higher concentration of products at equilibrium
c)
Higher concentration of reactants at equilibrium
d)

Nothing, without considering the coefficients of the reaction

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