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Equilibrium, Keq, Ksp & Le Chatelier's Principle: Honors

Total questions: 34

Worksheet time: 49mins

Name
Class
Date
1.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
2.
Identify the labels (a) and (b) on the graph.
a)
a is concentration of reactants and b is the concentration of product
b)
a is concentration of product and b is the concentration of reactant
c)
a is the volume of reactants and b is the volume of product
d)
a the mass of reactants and b is the mass of product
3.
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
4.
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
5.
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
6.
2SO2(g)+O2(g)⇌2SO3(g)
Decreasing volume of container will
a)
shift equilibrium right
b)
shift equilibrium left
c)
change K
d)
have no change
7.
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]
8.

What is the effect of increasing the pressure on the following equilibrium: 2NO(g) + O2 (g) ⇌2NO2(g)?

a)

The yield of NO2 increases

b)

The yield of NO2 decreases

c)

The reaction is slower

d)

The concentration of O2 increases.

9.
For the reaction...
heat  +  N2  +  O2  <−>  2NO
If the heat is added to the chemical system, the concentration of O2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
triple
10.

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

11.
For the reaction...
H2 (g)  + Cl2 (g) <−>  2HCl (g)  +  heat
If the temperature is cooled, the _________ reaction will be favored.
a)
forward
b)
reverse
c)
forward and reverse
12.
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)
13.

For the following equilibrium reaction:

N2 (g) + 3 H2 (g) <==> 2 NH3 (g) ΔH=-386 kJ/mol

Predict the direction that the reaction will proceed, or shift, if...

H2 is removed

a)

right

b)

left

c)

no effect

14.

For the following equilibrium reaction:

N2 (g) + 3 H2 (g) <==> 2 NH3 (g) ΔH=-386 kJ/mol

Predict the direction that the reaction will proceed, or shift, if...

NH3 is added

a)

right

b)

left

c)

no effect

15.

For the following equilibrium reaction:

N2 (g) + 3 H2 (g) <==> 2 NH3 (g) ΔH=-386 kJ/mol

Predict the direction that the reaction will proceed, or shift, if...

The reaction is heated.

a)

right

b)

left

c)

no effect

16.

What are the two factors that help determine that equilibrium is reached?

a)

Forward reaction rate is faster than the reverse and the concentrations are equal

b)

Forward and reverse reaction rates are equal and concentrations are equal

c)

Forward and reverse reaction rates are equal and concentrations are constant

17.
Given: 2A(g) <=> 2B(g) + C(g). At a particular temperature, Kc = 16000.
Raising the pressure, by decreasing the volume of the container, will...
a)
cause the value of Kc to increase
b)
cause the value of Kc to decrease
c)
have no effect on the value of Kc as temperature does not change
d)
favour the forward reaction
18.
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
19.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
20.

At elevated temperatures ammonium carbonate, NH2COONH4, is in equilibrium with NH3 and CO2 according to the equation;

NH2COONH4(s) ↔ 2 NH3(g) + CO2(g)

What is the equilibrium expression for this reaction?

a)

K = 2 [NH3][CO2]

[NH2COONH4]

b)

K = [NH3]2[CO2]

[NH2COONH4]

c)

K = 2 [NH3][CO2]

d)

K = [NH3]2[CO2]

21.
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.
22.
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
23.
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.
24.

Which is NOT a way to stress a closed chemical system at equilibrium?

a)

change temperature

b)

add a reactant

c)

take away a chemical in the reaction

d)

add a catalyst

25.

If I add a chemical to a system at equilibrium, increasing its concentration,

a)

the reaction will shift to the same side of the equation where it appears to make more of it

b)

the reaction will shift to the opposite side of the equation where it appears to use some of it up

c)

the reaction will not shift

d)

byproducts (other unwanted chemicals) will be formed to use the excess

26.

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

27.

Which quantities go into an equilibrium constant expression?

a)

solid amounts

b)

exo or endothermic heat quantities

c)

pure liquid amounts

d)

concentrations of chemicals

28.

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

29.

Consider the following reaction:

Fe +3 + SCN-1 ↔ 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.

30.
Consider the following equation 
H2 (g) + I2 (g) <===> 2 HI(g)  
Calculate Keq if at 300oK the concentrations are [H2] = 0.40 M   [I2] = 0.45 M ; [HI] = 0.30 M
a)
0.42
b)
0.5
c)
1.67
d)
0.6
31.
Which of the following shows the correct dissolution reaction for BaCl2?
a)
Ba 2+(aq) + Cl2-(aq) -> BaCl2(s)
b)
BaCl2(aq) -> Ba 2+(aq) + 2Cl-(aq)
c)
 BaCl2(s) -> Ba 2+(aq) + 2Cl-(aq)
d)
Ba 2+(aq) + 2Cl-(aq) -> BaCl2(s)
32.
a)

a

b)

b

c)

c

d)

d

e)

e

33.
a)

a

b)

b

c)

c

d)

d

e)

e

34.
a)

a

b)

b

c)

c

d)

d

e)

e

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