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QCE chem unit 3 topic 1 equilibrium

Total questions: 102

Worksheet time: 2hrs 10mins

Name
Class
Date
1.

Which of the following is true?

a)

Energy is found only in living objects

b)

Energy is a fuel

c)

Energy is a substance or fluid

d)

Energy is associated only with movement

e)

Any store of energy may be transferred into another store

2.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
3.
Which of the following is incorrect? 
A dynamic equilibrium can be achieved...
a)
From 100% reactants
b)
From 100% products
c)
In a closed system
d)
In an open system
4.

2SO2(g)+O2(g)⇌2SO3(g)

Removing O2(g) will

a)

shift equilibrium forward

b)

shift equilibrium reverse

c)

no shift

5.

2SO2(g)+O2(g)⇌2SO3(g)

Adding O2(g) will

a)

shift equilibrium forward

b)

shift equilibrium reverse

c)

no shift

6.

2SO2(g)+O2(g)⇌2SO3(g)

Adding SO2(g) will

a)

shift equilibrium forward

b)

shift equilibrium reverse

c)

no shift

7.
When the rate of the forward reaction is equal to the rate of backward reaction, the system is said to be in
a)
Chemical Equilibrium
b)
Chemical Balance
c)
Chemical Constant
d)
Chemical Reaction
8.
Define chemical equilibrium.
a)
A reaction is reversible.
b)
The concentration of the reactants is equal to the concentration of the products.
c)
The rate of a forward reaction is equal to the rate of the reverse reaction.
d)
The reaction stops and no further change in concentration occurs.
9.
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
10.
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?
a)
N2
b)
H2
c)
N2 and H2
d)
NH3
11.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
d)
plasma
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

b)

H2

c)

N2 and H2

d)

NH3

13.

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.

14.

2SO2(g)+O2(g)⇌2SO3(g)

Adding SO3(g) will

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase K

d)

have no change

15.
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
16.

For the reaction...

N2 + O2 <=> 2NO: Δ H = +182 kJ mol-1. (Forward reaction is endothermic)

If the temperature is increased the equilibrium position will shift _______.

a)

to the left

b)

to the right

c)

to the left and right

d)

neither left nor right

17.

why is medium temperature used in the Haber process?

a)

low temperature will form more ammonia

b)

high temperature will form more hydrogen and nitrogen

c)

the rate slows down

d)

to increase the rate but not negatively affecting the yield

18.

What is the purpose of a catalyst on an equilibrium reaction?

a)

to increase the rate of forward reaction

b)

to increase rate of backward reaction

c)

in increase both forward and backward reaction rates

d)

no effect

19.
The following factors affect the position of equilibrium EXCEPT
a)
Concentration
b)
Pressure
c)
Temperature
d)
States of matter
20.

2SO2(g)+1O2(g) ⇌ 2SO3(g) + Heat


Increasing the pressure on the system will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

slow rate of reaction

d)

have no change

21.

CoCI42- +6H2O →Co(H2O)62+ + 4CI-.


What would happen when H2O is added?

a)

Position of equilibrium will shift to left (and become more blue)

b)

Position of equilibrium will shift to right (and become more pink)

c)

Keq will increase as H2O is added

d)

Position of equilibrium will shift to left to reduce the added H2O

22.
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
23.
For the reaction...
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
24.

N2 (g) + 3H2 (g) < -> 2NH3 (g) + Heat

Removing H2

a)

Shift Left

b)

Shift Right

25.

2SO2(g)+O2(g) ⇌ 2SO3(g) + Heat


Increasing the temperature will...

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase pressure

d)

have no change

26.

CoCI42- +6H2O →Co(H2O)62+ + 4CI-.


What would happen when H2O is added?

a)

Position of equilibrium will shift to left (and become more blue)

b)

Position of equilibrium will shift to right (and become more pink)

c)

Keq will increase as H2O is added

d)

Position of equilibrium will shift to left to reduce the added H2O

27.

2SO2(g) + O2(g) ⇌ 2SO3(g) + Heat


Using a catalyst

a)

shift equilibrium right

b)

shift equilibrium left

c)

increase the rate of reaction

d)

have no change

28.
What is the Kc expression for this reaction?
   2 NO(g)  +  O2(g) ⇌  2 NO2(g)
a)
Kc = [NO2]2 / [NO]2 [O2]
b)
Kc =  [NO]2 [O2] / [NO2]2
c)
Kc = [NO]2 [O2] [NO2]2
d)
Kc = [NO2]2 / [NO]2 +  [O2]
29.
What are [A] and [B]?
a)
concentration of reactants
b)
concentration of products
c)
energy of reactants
d)
energy of products
30.
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
31.
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]
32.
If the equilibrium constant is much less than one (K << 1) then
a)
Equilibrium is not established.
b)
Equilibrium lies to the right (products are favored)
c)
Equilibrium lies to the left (reactants are favored)
d)
Neither products or reactants are favored.
33.
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
34.
A hydrogen ion, H+, is the same as a(n):
a)
neutron
b)
electron
c)
proton
d)
hydroxide ion
35.

A Bronsted Lowry acid:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

36.

A Bronsted Lowry base:

a)

donates H+ to another substance

b)

accepts H+ from another substance

c)

produces H+

d)

produces OH-

37.

In the equation below, what is the Bronsted Lowry acid (donates H+)?

HCl + NH3 → Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

38.

In the equation below, what is the Bronsted Lowry base (accepts H+)?

HCl + NH3 → Cl- + NH4+

a)

HCl

b)

NH3

c)

Cl-

d)

NH4+

39.

Which reactant in the following equation is a Bronsted Lowry acid?

H2O + HCl → H3O+ + Cl-

a)

Water

b)

Hydrogen chloride

c)

Hydronium

d)

Chloride

40.

Which product in the following equation is a conjugate base?

H2O + HCl → H3O+ + Cl-

a)

Water

b)

Hydrogen chloride

c)

Hydronium

d)

Chloride

41.

What is the Bronsted Lowry base in the following equation?

PO4-3 + HNO3 → NO3- + HPO4-2

a)

PO43-

b)

HNO3

c)

NO3-

d)

HPO42-

42.

What is the conjugate acid in the following equation?

PO4-3 + HNO3 → NO3- + HPO4-2

a)

PO43-

b)

HNO3

c)

NO3-

d)

HPO42-

43.

What is the conjugate base in the following reaction?

HCO3- + HCl → H2CO3 + Cl-

a)

HCO3-

b)

HCl

c)

H2CO3

d)

Cl-

44.

HSO4- + H2O → H3O+ +SO42-

Identify the Bronsted Lowry Acid in the above reaction.

a)

HSO4-

b)

H2O

c)

H3O+

d)

SO42-

45.

CO32- + H2O → HCO3- + OH-

Using the above reaction, which compound is the conjugate base?

a)

CO32-

b)

H2O

c)

HCO3-

d)

OH-

46.

Which of the following is the correct definition for a strong acid?

a)

Partially dissociates into ions when dissolved in water and the change is not reversible

b)

Fully dissociates into ions when dissolved in water and the change is not reversible

c)

Fully dissociates into ions when dissolved in water and the change is reversible

d)

Partially dissociates into ions when dissolved in water and the change is reversible

47.

Which of the following is the correct balanced equation showing the dissociation of sulfuric acid into ions?

a)

H2SO4 (aq) → H+ (aq) + SO4–(aq)

b)

H2SO4 (aq) ⇌ 2H+ (aq) + SO42- (aq)

c)

HSO4 (aq) → H+(aq) + SO4–(aq)

d)

H2SO4 (aq) → 2H+ (aq) + SO42- (aq)

48.

Which of the following statements is true?

a)

If the H+ ion concentration in a solution increases by a factor of 10, the pH of the solution increases by 1

b)

If the H+ ion concentration in a solution increases by a factor of 10, the pH of the solution decreases by 1

49.

An acid of concentration 1 mol/dm3 has a pH of 2. The acid is diluted to a concentration of 0.01 mol/dm3. What is its new pH?

a)

3

b)

4

c)

2

d)

1

50.

What is the Charge of a Proton?

a)

Positive

b)

Negative

c)

Neutral

51.

What is the Charge of an Electron?

a)

Positive

b)

Negative

c)

Neutral

52.

What does the Nucleus of an atom contain?

a)

Proton and Neutron

b)

Electron and Neutron

c)

Proton and Electron

53.

What ions do Metals form when they react?

a)

Negative

b)

Positive

54.

Select all the properties of a Metal:

a)

Brittle

b)

Malleable

c)

Strong

d)

Conductive

55.
What are the formulas for the following?
--hydrochloric acid--
--hydrobromic acid--
--hydroiodic acid--
a)
HClO3, HBrO3, HIO3
b)
HCl, HBr, HI
c)
HClO4, HBrO4, HIO4
d)
HClO, HBrO, HIO
56.
Name the following in order:
H2SO4, HNO3
a)
sulfurous acid, nitrous acid
b)
hydrosulfuric acid, hydronitric acid
c)
sulfuric acid, nitric acid
d)
hydrosulfurous acid, hydronitrous acid
57.
What are the formulas for the following?
--sulfuric acid--
--nitric acid--
a)
H2SO, HNO
b)
H2SO3, HNO3
c)
H2S, H3N
d)
H2SO4, HNO3
58.

Is this acid monoprotic, diprotic or triprotic


Hydrochloric Acid HCl

a)

Monoprotic acid

b)

Diprotic acid

c)

Triprotic acid

d)

Not an acid

59.

Is this acid monoprotic, diprotic or triprotic


Phosphoric Acid H3PO4

a)

Monoprotic acid

b)

Diprotic acid

c)

Triprotic acid

d)

Not an acid

60.

Is this acid monoprotic, diprotic or triprotic


Sulfuric Acid H2SO4

a)

Monoprotic acid

b)

Diprotic acid

c)

Triprotic acid

d)

Not an acid

61.

Is this acid monoprotic, diprotic or triprotic


Hydrogen Sulfide H2S

a)

Monoprotic acid

b)

Diprotic acid

c)

Triprotic acid

d)

Not an acid

62.

Is this acid monoprotic, diprotic or triprotic


Acetic Acid CH3COOH

a)

Monoprotic acid

b)

Diprotic acid

c)

Triprotic acid

d)

Not an acid

63.

Is this acid monoprotic, diprotic or triprotic


Phosphorous acid H3PO3

a)

Monoprotic acid

b)

Diprotic acid

c)

Triprotic acid

d)

Not an acid

64.

Is this acid monoprotic, diprotic or triprotic


Chromic acid H2CrO4

a)

Monoprotic acid

b)

Diprotic acid

c)

Triprotic acid

d)

Not an acid

65.

Concentration is

a)

the amount of solute in the solvent

b)

the amount of solvent in the solute

c)

a measure of how strong an acid or base is

d)

the size of the particles in a solution

66.

Which solution is more concentrated?

Solution 1:

500 mL of water

100 g of salt

pH = 3


Solution 2:

500 mL of water

90 g of salt

pH = 2.4

a)

Solution 1

b)

Solution 2

c)

They have the same concentration

d)

I have no idea

67.

Neutral solutions have a pH of:

a)

0

b)

1

c)

7

d)

14

68.

Which is true?

a)

pH of less than 7 is basic; pH of more than 7 is acidic

b)

pH of less than 7 is acidic; pH of more than 7 is basic

69.
What is the pH of a solution that has a [H+] of 2.5 x 10-5?
a)
4.60
b)
5.0
c)
2.5
d)
7
70.
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
71.
The lower the pH, the greater the concentration of :
a)
OH-
b)
H+
72.
What is the pH of a solution where the [H+] is 1.0 x 10-11?
a)
11
b)
13
c)
14
d)
1
73.
What is the pH of a 0.15 M solution of HClO4?
a)
0.82
b)
13.18
c)
0.15
d)
1
74.

What is the molarity of hydroxide ions in a solution with a pH of 4?

a)

1.0 X 10-4

b)

1.0 x 10-10

c)

10

d)

1.0 x 10-14

75.

Pure water (H2O) has a pH of 7 and would be classified as...

a)

a base

b)

a neutral substance

c)

both an acid and a base

d)

an acid

76.

Acidic solutions exhibit a higher ratio of H3O+ ions, known as...

a)

neutrons

b)

hydroxide

c)

electrons

d)

hydronium

77.

Buffer is defined as

a)

ability to change a pH

b)

ability to prevent pH from decreasing

c)

ability to resist a pH increase

d)

minimizes the changes in the concentrations of H+ and OH-

78.

Why do cells need a buffer system?

a)

Chemical processes in the cell are sensitive to the concentration of H+ and OH-

b)

Cells do not have a buffer system

c)

Cells need acids and bases to survive

d)

The pH range of cells can withstand large changes

79.
What kind of acid does not completely dissociate?
a)
weak
b)
strong
c)
ionic
d)
pH
80.

Which point on the titration curve corresponds to the point at which the moles of the added strong base are equal to the moles of the weak acid initially present?

a)

Q

b)

R

c)

S

d)

T

81.

At which point on the titration curve will pH = pKa?

a)

Q

b)

R

c)

S

d)

P

82.

Which acid base pair produced this titration curve?

a)

HCI + KOH

b)

HCI + NH3

c)

CH3COOH + KOH

d)

CH3COOH + NH3

83.
Which type of titration is shown by this titration curve?
a)
Titration of a strong acid by a strong base 
b)
Titration of a weak acid by a strong base 
c)
Titration of a strong base by a strong acid 
d)
Titration of a weak base by a strong acid
84.

Which curve is produced by the addition of a strong acid to a strong base?

a)

A

b)

B

c)

C

d)

D

85.
An indicator will ______________ when it is in contact with an acid or base
a)
Bubble
b)
Form a new substance
c)
Change color
d)
Stay the same color
86.
The pH of a strong base would be:
a)
1-2
b)
5-6
c)
8-9
d)
13-14
87.
One drawback to a pH Meter is that it
a)
Is very expensive
b)
is not very accurate
c)
only tells you if a substance is an acid or a base
d)
is messy
88.
One benefit of a pH Meter is that it
a)
is very expensive
b)
only tells you if a substance is an acid or a base
c)
is very accurate
d)
can be made from substances you have at home
89.

To prepare a solution of accurately known volume, use a

a)

measuring cylinder

b)

beaker

c)

concial flask

d)

volumetric flask

90.

To deliver a fixed accurate volume of a solution, use a

a)

pipette

b)

burette

c)

dropper

d)

beaker

91.

A standard solution is a solution with accurately known concentration.

a)

True

b)

False

92.

What is volumetric analysis?

a)

Estimate no of moles of component in the compound

b)

Estimate the amount of component in the compound.

c)

Estimate the volume of a component in the compound.

d)

Estimate mass of a component in the compound.

93.

What is the reading on this burette?

a)

24.2 mL

b)

24.0 mL

c)

25.8 mL

d)

23.9 mL

94.

Volumetric analysis can be defined as_____________

a)

The determination of the identity of the solution

b)

The determination of the mole of a mixture with a known solution

c)

The determination of the concentration of a solution using a solution of known concentration

95.

A chemical used to show the end point of titration is called

a)

base

b)

indicator

c)

pipette

d)

acid

96.

The burette readings should be recorded to

a)

2 significant figures

b)

3 significant figures

c)

2 decimal points

d)

3 decimal points

97.

20 cm3 of 1 mol dm–3 CH3COOH(aq) and 10 cm3 of 1 mol dm–3 H2SO4(aq) require the same number of moles of NaOH for complete neutralization.

a)

True

b)

False

98.

3.75 dm3 of distilled water are added to 250.0 cm3 of 3.20 mol dm–3 sodium hydroxide solution. What is the molarity of the diluted solution?

a)

0.200 mol dm-3

b)

0.213 mol dm-3

c)

2.00 mol dm-3

d)

2.13 mol dm-3

99.

Which of the following pairs of solutions, when mixed, would give a neutral solution?

a)

100 cm3 of 1 mol dm–3 H2SO4(aq) and 100 cm3 of 1 mol dm–3 NaOH(aq)

b)

100 cm3 of 1 mol dm–3 H2SO4(aq) and 100 cm3 of 2 mol dm–3 NaOH(aq)

c)

100 cm3 of 2 mol dm–3 H2SO4(aq) and 50 cm3 of 2 mol dm–3 NaOH(aq)

d)

200 cm3 of 2 mol dm–3 H2SO4(aq) and 100 cm3 of 1 mol dm–3 NaOH(aq)

100.

25.0 cm3 of sodium hydroxide solution is tritrated against 0.200 mol dm–3 hydrochloric acid until the indicator just changes colour. 27.5 cm3 of the acid are required to reach the end point.

Phenolphthalein is used as an indicator in the above experiment. What will be its colour change at the end point?

a)

From red to yellow

b)

From red to colourless

c)

From yellow to colourless

d)

From yellow to red

101.

25.0 cm3 of sodium hydroxide solution is tritrated with 0.200 mol dm–3 hydrochloric acid until the indicator just changes colour. 27.5 cm3 of the acid are required to reach the end point.

What is the molarity of the sodium hydroxide solution?

a)

0.100 mol dm-3

b)

0.110 mol dm-3

c)

0.200 mol dm-3

d)

0.220 mol dm-3

102.

In an experiment, 30.0 cm3 of a monobasic acid HA(aq) were titrated with 0.100 mol dm–3 NaOH(aq). The following graph shows the variation of pH of the solution mixture during the titration:

What is the concentration of HA(aq)?

a)

7.50 x 10–5 mol dm–3

b)

1.50 x 10–4 mol dm–3

c)

7.50 x 10–2 mol dm–3

d)

1.50 x 10–1 mol dm–3

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