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WorksheetsEquilibrium
Total questions: 55
Worksheet time: 4hrs 52mins
Name
Class
Date
1.
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
2.
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
3.
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
4.
For the reaction...
SO2 + O2 <−> SO3
If the equilibrium shifts to the left, the concentration of SO3 will ___________.
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
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...
heat + N2 + O2 <−> 2NO
If NO is removed from the system, the concentration of N2 will _______.
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
7.
For the reaction...
heat + N2 + O2 <−> 2NO
If the heat is added to the chemical system, the equilibrium will shift _______.
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
8.
For the reaction...
heat + N2 + O2 <−> 2NO
If the heat is removed to the chemical system, the equilibrium will shift _______.
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
9.
For the reaction...
heat + N2 + O2 <−> 2NO
If the heat is removed from the chemical system, the concentration of N2 will _______.
heat + N2 + O2 <−> 2NO
If the heat is removed from the chemical system, the concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
10.
For the reaction...
heat + N2 + O2 <−> 2NO
If the heat is added to the chemical system, the concentration of O2 will _______.
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
11.
For the reaction...
H2 (g) + Cl2 (g) <−> 2HCl (g) + heat
If the temperature is cooled, the _________ reaction will be favored.
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...
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
13.
For the reaction...
N2 (g) + 3 H2 (g) <−> 2 NH3 (g)
If the pressure in the system is increased, _______ reaction will be favored.
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
14.
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
15.
What is the molarity for water if Keq = 1.2, [CO2] = 0.846M, & [CH4]= 0.0713M?
Copper (II) oxide (s) + carbon tetrahydride (g)<—> carbon dioxide (g) + copper (s) + water (g)
Copper (II) oxide (s) + carbon tetrahydride (g)<—> carbon dioxide (g) + copper (s) + water (g)
a)
0.101 M
b)
0.318 M
c)
0.0102 M
d)
3.77 M
16.
Determine the value of the equilibrium constant (Keq) for this reaction if the concentration of N2O4(g) is 0.400 mol/L and NO2 is 0.550 mol/L.
* Balance equation.
N2O4(g) ↔ NO2(g)
* Balance equation.
N2O4(g) ↔ NO2(g)
a)
1.38
b)
1.32
c)
0.22
d)
0.756
17.
What is [C] and [D]
a)
concentration of products
b)
concentration of reactant
c)
energy of products
d)
energy of reactant
18.
What is [A] and [B]?
a)
Concentration of Reactants
b)
Concentration of Products
c)
Energy of Reactants
d)
Energy of Products
19.
What is x and y?
a)
Coefficient of Products in the Balanced Reaction
b)
Coefficient of Reactants in the Balanced Reaction
c)
Order of Reaction with respect to the products
d)
Order of Reaction with respect to the Reactants
20.
What is n and m?
a)
Coefficient of Products in the Balanced Reaction
b)
Coefficient of Reactants in the Balanced Reaction
c)
Order of Reaction with respect to the products
d)
Order of Reaction with respect to the Reactants
21.
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.
22.
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.
23.
What kind of equilibrium does the reaction below show?
H2(g) +I2(g) ↔ 2HI(g)
H2(g) +I2(g) ↔ 2HI(g)
a)
Heterogeneous equilibrium, all the reactants and products are in the same physical state.
b)
Homogeneous equilibrium, all the reactants and products are in the same physical state.
c)
Heterogeneous equilibrium, the reactants and products are present in more than one physical state
d)
Homogeneous equilibrium, the reactants and products are present in more than one physical state
24.
What kind of equilibrium does the reaction below show?
CaCO3 (s) ↔ CaO (s) + CO2 (g)
CaCO3 (s) ↔ CaO (s) + CO2 (g)
a)
Heterogeneous equilibrium, all the reactants and products are in the same physical state.
b)
Homogeneous equilibrium, all the reactants and products are in the same physical state.
c)
Heterogeneous equilibrium, the reactants and products are present in more than one physical state
d)
Homogeneous equilibrium, the reactants and products are present in more than one physical state
25.
For the reaction...
SO2 + O2 <−> SO3
If the equilibrium shifts to the left, the concentration of SO2 will ___________.
SO2 + O2 <−> SO3
If the equilibrium shifts to the left, the concentration of SO2 will ___________.
a)
increase
b)
decrease
26.
A 1.00 L vessel was found to contain 0.281 mol of CO, 0.889 mol of O2, and a Keq = 1.21 What is the molarity of CO2? * Balance equation.
CO2(g) ↔ CO(g) + O2(g)
CO2(g) ↔ CO(g) + O2(g)
a)
0.0580 M
b)
0.488 M
c)
0.241 M
d)
Not enough info given
27.
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
28.
What color does acid turn litmus paper?
a)
It turns litmus paper purple.
b)
It turns red litmus paper blue.
c)
It turns blue litmus paper blue.
d)
It turns blue litmus paper red.
29.
What color does bases turn litmus paper?
a)
It turns litmus paper purple.
b)
It turns blue litmus paper red.
c)
It turns red litmus paper blue.
d)
It turns red litmus paper re
30.
Drain cleaner has a pH of 13. What is drain cleaner?
a)
An acid.
b)
A strong base.
c)
Neutral.
d)
A weak base.
31.
What might happen if you mixed a strong acid with an equally strong base?
a)
You would see an explosive chemical reaction.
b)
The acid would destroy the base.
c)
The base would destroy the acid.
d)
You'd wind up with a pH-neutral substance.
32.
What is the pH of a solution that has a [H+] of 2.5 x 10-5 M?
a)
4.60
b)
5.0
c)
2.5
d)
7
33.
What is the pOH of a solution where the [OH-] is 7.3 x 10-2 M?
a)
-1.14
b)
2.0
c)
1.14
d)
7.3
34.
What is the [OH-] if the [H+] is 1.0 x 10-3M?
a)
1.0 x 10-3 M
b)
6.02 x 10-23 M
c)
1.0 x 10-14 M
d)
1.0 x 10-11 M
35.
What is the [H+] if the pH is 4.0?
a)
1.0 x 10-10 M
b)
1.0 x 10-4 M
c)
1.0 x 10-14 M
d)
1.0 x 10-7 M
36.
What is the pOH of a solution that has a pH of 2?
a)
10
b)
12
c)
14
d)
1
37.
What is the [OH-] if the pH is 4.9?
a)
7.94 x 10-10 M
b)
1.3 x 10-5 M
c)
7.94 x 10-14 M
d)
4.9 x 10-10 M
38.
What is the pH of a solution where the [H+] is 1.0 x 10-11 M?
a)
11
b)
13
c)
14
d)
1
39.
What is the molarity of a solution made by diluting 26.5 mL of 6.00M HNO3 to a volume of 250. mL?
a)
15.9 M
b)
0.636 M
c)
0.642 M
d)
1.59 M
40.
The following neutralization reaction occurs in the classroom.
HCl + KOH --> H2O + KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if the is 15.0mL of acid neutralized?
HCl + KOH --> H2O + KCl
If a student uses 25.0 mL of a 0.5M solution of KOH, what is the molarity of the acid if the is 15.0mL of acid neutralized?
a)
0.8M
b)
1.2M
c)
12.5M
41.
The pH scale is a range from:
a)
1-7
b)
0-14
c)
1-14
d)
1-20
42.
What is the conjugate acid in the following equation?
a)
PO43-
b)
HNO3
c)
NO3-
d)
HPO42-
43.
What is the conjugate base in the following reaction?
a)
HCO3-
b)
HCl
c)
H2CO3
d)
Cl-
44.
HCl
a)
acid
b)
base
c)
neutral
45.
Be(OH)2
a)
acid
b)
base
c)
neutral
46.
What is the product of the reaction of a weak acid and strong base
a)
water only
b)
neutral salt and water
c)
salt and water
d)
salt only
47.
Which is the stronger acid?
a)
pH 1
b)
pH 4
c)
pH 8
d)
pH 13
48.
Write a balanced chemical equation from the following neutralization reactions:
iron (III) hydroxide + sulfuric acid ------->
iron (III) hydroxide + sulfuric acid ------->
a)
2 FeOH3 + 3 H2SO4 ---> 2 Fe(SO4)2 + 5 H2O
b)
2 Fe(OH)3 + 3 H2SO4 ---> 1 Fe2(SO4)3 + 6 H2O
c)
2 Fe(OH)3 + 3 H2S ---> 1 Fe2S3 + 6 H2O
49.
Write the equilibrium constant expression for the following reaction:
5A (g) + 1 B(g) + 1 C(s) ---> 10 D(g) + 6 E(g)
5A (g) + 1 B(g) + 1 C(s) ---> 10 D(g) + 6 E(g)
a)
Keq = [D]10[E]6 / [A]5 [B] [C]
b)
Keq = [D]10[E]6 / [A]5 [B]
c)
Keq =[A]5 [B] [C] / [D]10[E]6
d)
Keq =[A]5 [B] / [D]10[E]6
50.
Dihydrogen monosulfide gas decomposes into hydrogen gas and sulfur (S2) gas.Given the equilibrium constant Keq = 2.27 x 10-3, what is the concentration of hydrogen gas if [S2] = 0.0540 mol/L and [H2S] = 0.184 mol/L ?
a)
0.00142 M
b)
0.0879 M
c)
0.0377 M
51.
Adjusting the concentrations of either the reactants or products in a reaction puts stress on the equilibrium.
a)
True
b)
False
52.
A homogeneous equilibrium reaction has reactants and products that are in the same physical state.
a)
True
b)
False
53.
At equilibrium, the concentrations of reactants and products are not constant.
a)
True
b)
False
54.
A heterogeneous equilibrium reaction has reactants and products that are in the same physical state.
a)
True
b)
False
55.
In an exothermic reaction, an increase in temperature favors the formation of products.
a)
True
b)
False
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