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WorksheetsC6
Total questions: 25
Worksheet time: 17mins
Name
Class
Date
1.
For the reaction...
SO2 + O2 <−> SO3
If the concentration of SO2 is increased, the equilibrium of the reaction will shift ___________.
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
2.
For the reaction...
SO2 + O2 <−> SO3
If the equilibrium shifts to the right, the concentration of O2 will ___________.
SO2 + O2 <−> SO3
If the equilibrium shifts to the right, the concentration of O2 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
3.
For the reaction...
SO2 + O2 <−> SO3
If the equilibrium shifts to the right, the concentration of SO3 will ___________.
SO2 + O2 <−> SO3
If the equilibrium shifts to the right, the concentration of SO3 will ___________.
a)
increase
b)
decrease
c)
remain the same
d)
double
4.
For the reaction...
SO2 + O2 <−> SO3
If the concentration of O2 is decreased, the equilibrium of the reaction will shift ___________.
SO2 + O2 <−> SO3
If the concentration of O2 is decreased, the equilibrium of the reaction will shift ___________.
a)
left
b)
right
c)
left and right
d)
neither left nor right
5.
For the reaction...
heat + N2 + O2 <−> 2NO
If O2 is removed, the concentration of N2 will _______.
heat + N2 + O2 <−> 2NO
If O2 is removed, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
6.
For the reaction...
H2 (g) + Cl2 (g) <−> 2HCl (g) + heat
If the pressure in the system is increased, the equilibrium will _______.
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
7.
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?
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
8.
An equilibrium constant with a large magnitude indicates…
a)
A very fast reaction
b)
More products at equilibrium
c)
More reactants at equilibrium
d)
nothing, without considering the stoichiometry of the reaction
9.
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.
10.
At what time (in seconds) is equilibrium established?
a)
0 seconds
b)
1 second
c)
5 seconds
d)
10 seconds
11.
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
12.
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.
13.
What is [A] and [B]?
a)
Concentration of Reactants
b)
Concentration of Products
c)
Energy of Reactants
d)
Energy of Products
14.
What is the proper Keq for the following reaction?
2 NO(g) + O2(g) ⇌ 2 NO2(g)
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]
15.
A(n) ______ is a substance with a pH less than 7
a)
Acid
b)
Alkaline
c)
Base
d)
Buffer
16.
A(n) _______ is a substance with a pH greater than 7.
a)
Base
b)
Acid
c)
Buffer
d)
Water
17.
Which of the following substances would likely create the most conductive solution?
a)
a weak acid
b)
a weak base
c)
a strong acid
d)
an insoluble salt
18.
The pH scale is based off of the concentration of _________ ions.
a)
Oxygen
b)
Hydronium (H+)
c)
Nitrogen
d)
None of the others
19.
The pH of a solution at 25ₒC in which [OH-] = 3.9 x 10-5M is:
a)
4.41
b)
3.90
c)
9.59
d)
4.80
20.
When citric acid is produced by the cells of an orange and dissolves in water, it produces a relatively small number of hydronium ions. Citric acid is best described as a
a)
concentrated acid.
b)
weak acid.
c)
dilute acid.
d)
strong acid.
21.
Which is the weakest acid?
a)
HF
b)
HNO2
c)
CH3COOH
d)
HClO
22.
Consider the general equation for an acid in water:
HA(aq) + H2O ↔ H3O+ + A-
If there is a lot of product, what does that tell you about the acid?
HA(aq) + H2O ↔ H3O+ + A-
If there is a lot of product, what does that tell you about the acid?
a)
Ka > 1 Strong acid
b)
Ka > 1 Weak acid
c)
Ka < 1 Strong acid
d)
Ka < 1 Weak acid
23.
Calculate the pH of a 0.47M NH3 (Kb = 1.8 x 10-5) solution.
a)
2.54
b)
8.93
c)
5.07
d)
11.46
24.
Calculate the [H+] in a solution that has a pH of 2.73.
a)
5.4 x 10-12 M
b)
1.9 x 10-3 M
c)
2.7 M
d)
11.3 M
25.
What is the pH of a 0.25 M solution of LiOH?
a)
0.25
b)
13.4
c)
0.60
d)
12.3
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