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T2- Final Revision Quiz

Total questions: 85

Worksheet time: 1hrs 10mins

Name
Class
Date
1.
Is the combustion of gasoline endothermic or exothermic?
a)
Endothermic
b)
Exothermic
2.
What is the symbol for heat?
a)
q
b)
H
c)
J
d)
∘C
3.

What are chemical reactions that absorb energy?

a)

endothermic

b)

fast

c)

slow

d)

exothermic

4.

What is the study of heat changes that accompany chemical reactions and phase changes?

a)

energy

b)

chemistry

c)

work

d)

thermochemistry

5.

What is the formula for calculating heat?

a)

q = mcΔT

b)

H = ΔH x moles

c)

H = ΔH x grams

d)

products - reactants

6.

Convert 42 kJ into joules

a)

0.042 J

b)

175.73 J

c)

42000 J

d)

10.04 J

7.

What are the two main types of energy?

a)

endothermic and exothermic

b)

spontaneous and nonspontaneous

c)

potential and kinetic

d)

entropy and enthalpy

8.

Consider the reaction: 2 H2O + energy --> 2H2 + O2

a)

exothermic because releasing energy

b)

exothermic because absorbing energy

c)

endothermic because absorbing energy

d)

endothermic because releasing energy

9.
The heat required to raise the temperature of a SUBSTANCE by 1∘C
a)
calorie
b)
joule
c)
specific heat
d)
4.184 J
10.
The heat required to raise the temperature of WATER 1∘C
a)
calorie
b)
joule
c)
specific heat
d)
energy
11.
Heat flows from _______ to ______ objects
a)
cooler to warmer
b)
warmer to warmer
c)
warmer to cooler
d)
cooler to cooler
12.

A 500g piece of aluminum has a temperature of 7°C. What is the heat energy produced? Specific heat of Aluminum is 0.900 J/gºC.

a)

3000 J

b)

3000 g

c)

3150 J

d)

3150 g

13.

What does temperature measure?

a)

heat

b)

average kinetic energy

c)

space

d)

time

14.

How much heat does an aluminum block absorb if 10.00 grams is heated from 25.0oC to 50.0oC? *Specific heat of aluminum is 0.900 J/goC

a)

450 J

b)

-450 J

c)

225 J

d)

-225 J

15.

A 24.0 gram sample of copper was heated from 25.0oC to 500.0oC, 4378 J of heat were absorbed, what is the specific heat of copper?

a)

0.384 J/g°C

b)

49909200 J/g°C

c)

2.60 J/g°C

d)

8.77 J/g°C

16.

The specific heat of platinum is 0.133 J/g°C. How much heat is released when a 10 g piece of platinum cools from 100°C to 50°C?

a)

66.5 J

b)

665 J

c)

0.0266 J

d)

0.665 J

17.

Releasing heat into the surroundings occurs during an ___________________ reaction.

a)

Exothermic

b)

Endothermic

c)

Kinetic Energy

d)

Thermal Energy

18.

A sample of iron receives 50 J of heat energy that raises the temperature of the iron 25.0°C. If iron has a specific heat of 0.10 J/g°C, what is the mass of the iron sample?

a)

25g

b)

30g

c)

20g

d)

50g

19.

If 238 J of heat is absorbed by a sample of metal with a mass of 40.7 g, and it raises the temperature from 20.0°C to 32.4°C, what is the specific heat capacity of the metal?

a)

2.34 J/g°C

b)

0.472 J/g°C

c)

6.13 J/g°C

d)

0.163 J/g°C

20.

Which of the following values would represent the pH of a strong base?

a)

1

b)

8

c)

7

d)

13

21.

Complete the definition below:

Acids are....

a)

hydrogen donors.

b)

hydrogen acceptors.

c)

proton donors.

d)

proton acceptors.

22.

Acids which dissociate almost completely in aqueous solutions are known as:

a)

Dilute acids

b)

Strong acids

c)

Weak acids

d)

Concentrated acids

23.

Acids react with active metals to liberate:

a)

Oxygen

b)

Carbon dioxide

c)

Nitrogen

d)

Hydrogen

24.
When dissolved in water, bases produce:
a)
acids
b)
salts
c)
hydrogen ions
d)
hydroxide ions
25.

If a solution is basic which ion will be more present?

a)

H+

b)

K+

c)

OH-

d)

H-

26.

This ion is responsible for the properties of acids

a)

Sodium ion

b)

Hydrogen ion

c)

Hydroxide ion

d)

Oxide ion

27.

Predict the products for the following reaction: LiOH + H2SO4 -->

(Hint: it is a neutralization reaction)

a)

LiSO4 + H2O

b)
LiSO4 + H2(OH)
c)

Li2SO4 + H2O

d)
Li2SO4 + H2(OH)
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 are the formulas for the following?
--sulfuric acid--
--nitric acid--
a)
H2SO, HNO
b)
H2SO3, HNO3
c)
H2S, H3N
d)
H2SO4, HNO3
30.
Strong acids and bases...
a)

do not dissociate into ions (non-electrolyte)

b)

partially dissociate into ions (weak electrolyte)

c)

completely dissociate into ions (non-electrolyte)

d)

completely dissociate into ions (strong electrolyte)

31.

A substance that does not dissociate completely. Ranges from 4-7 on the pH scale.

a)
Strong Acid
b)
Strong Base
c)
Weak Acid
d)
Weak Base
32.

Hydrochloric (HCl) is a

a)

Weak Acid

b)

Weak Base

c)

Strong Acid

d)

Strong base

33.

Sodium hydroxide (NaOH) is a

a)

Weak Acid

b)

Weak Base

c)

Strong Acid

d)

Strong base

34.

Methanoic (HCOOH) is a

a)

Weak Acid

b)

Weak Base

c)

Strong Acid

d)

Strong base

35.

Ammonia (NH3) is a

a)

Weak Acid

b)

Weak Base

c)

Strong Acid

d)

Strong base

36.

When a metal carbonate reacts with an acid, what will the products always be?

a)

A salt, water and oxygen

b)

A salt, water and carbon dioxide

c)

Water and hydrogen

d)

A salt and water

37.

When comparing a strong and weak acid of the same concentration, the strong acid will have...(choose 2 answers)

a)

A higher conductivity

b)

A lower conductivity

c)

A faster rate of reaction

d)

A slower rate of reaction

38.

When comparing a strong and weak acid of the same concentration, the strong acid will have...(choose 2 answers)

a)

A higher pH

b)

A lower pH

c)

a smaller temperature change on neutralisation with a strong base

d)

a bigger temperature change on neutralisation with a strong base

39.

For a solution at 25oC, pH + pOH =

a)

7

b)

14

c)

1.0 x 10-14

d)

-log (1.0 x 10 -14)

40.

If the pH of a solution is 4.0, what is the pOH?

a)

4.0

b)

10.0

c)

1.0 x 10 -4

d)

cannot be determined from the information

41.

If the [H3O+] of a solution is 1 x 10-3 M, the pH is

a)

11

b)

-3

c)

3

d)

1

42.

If the pH of a solution is 8 the [H3O+] is

a)

1.0 x 106 M

b)

8.0 x 101 M

c)

1.0 x 108 M

d)

1.0 x 10-8 M

43.

When the hydrogen ion concentration goes up, the pH ___

a)

gets lower

b)

stays the same

c)

gets higher

d)

goes toward 7

44.

If the [OH-] of a solution is 2.7 x 10-4 M, the pOH of the solution is

a)

10.44

b)

1.00

c)

3.57

d)

-4.43

45.

The pH of a solution is 8.43. What is the [H3O+] concentration?

a)

3.7 x 10 -9

b)

1.0 x 10-8.43

c)

2.7 x 10-6

d)

1.0 x 10-14

46.

What is the numerical value of Kw, the water dissociation constant?

a)

14.0 x 10-1

b)

7.0 x 10-2

c)

2.0 x 10-7

d)

1.0 x 10-14

47.

If a solution has a pOH of 1 what is the pH? Is it an acid or base? (pick 2)

a)

acid

b)

base

c)

13

d)

1

e)

neutral

48.

If the [H3O+] of a solution is 6.8 x 10-8 M, the pH is

a)

7.17

b)

3.2 x 10-5

c)

7.2

d)

7.62

49.

If the [H3O+] of a solution is 9.3 x 10-3 M, the pOH of the solution will be

a)

2.03

b)

1.02

c)

11.97

d)

12.98

50.

When a water molecule loses a hydrogen ion, or proton, it becomes ___

a)

a hydronium ion, H3O+

b)

a hydroxide ion, OH-

c)

a hydronium ion, OH-

d)

a hydroxide ion, H3O+

51.

If a solution has a pH of 1 what is the pOH? Is it an acid or base? (pick 2)

a)

acid

b)

base

c)

13

d)

15

e)

neutral

52.

If a solution has a pOH of 3.7, the [OH-] of the solution is

a)

5.0 x 10-11

b)

2.0 x 10-4

c)

10.3

d)

14

53.

When a hydrogen ion, or proton, attaches to a water molecule it forms ___

a)

a hydronium ion, H3O+

b)

a hydroxide ion, OH-

c)

a hydronium ion, OH-

d)

a hydroxide ion, H3O+

54.

Oranges have a [H3O+] of 1.7 x 10-2 M. Their pOH is

a)

1.77

b)

12.23

c)

10.91

d)

3.09

55.

Find the pH of a solution with [OH-] = 8.41 x 10-4.

a)

3.08

b)

10.92

c)

9.88

d)

11.23

56.

What is the pOH of a solution where the [OH-] is 7.3 x 10-2 M?

a)

-1.14

b)

1.14

c)

2.01

d)

11.99

57.

A solution of KOH is 2.5 x 10-5 M. What is the [H+] concentration? (Hint: Find pOH, then pH, then [H+].)

a)

4.60

b)

9.40

c)

3.98 x 10-10

d)

1.0 x 10-4.60

58.
If the pH of a solution is 5.6 the pOH is
a)
6.5
b)
12.4
c)
8.4
d)
5.6
59.

Using the equations below:

C(s) + O2(g) → CO2(g) ∆H = –390 kJ

Mn(s) + O2(g) → MnO2(s) ∆H = –520 kJ

what is ∆H (in kJ) for the following reaction?

MnO2(s) + C(s) → Mn(s) + CO2(g)

a)

910

b)

130

c)

-130

d)

-910

60.

Using the equations below

Cu(s) + 1/2O2(g) → CuO(s) ∆H = –156 kJ

2Cu(s) + O2(g) → Cu2O(s) ∆H = –170 kJ

what is the value of ∆H (in kJ) for the following reaction?

2CuO(s) → Cu2O(s) + 1/2O2(g)

a)

142

b)

15

c)

-15

d)

-142

61.

Consider the following equations.

Mg(s) + O2(g) → MgO(s) ∆H = –602 kJ

H2(g) + O2(g) → H2O(g) ∆H = –242 kJ

What is the ∆H value (in kJ) for the following reaction?

MgO(s) + H2(g) → Mg(s) + H2O(g)

a)

-844

b)

-360

c)

+360

d)

+844

62.

The following equations show the oxidation of carbon and carbon monoxide to carbon dioxide.

C(s) +O2(g) → CO2(g) ΔH = –x kJ mol–1

CO(g) + O2(g) → CO2(g) ΔH = –y kJ mol–1

What is the enthalpy change, in kJ mol–1, for the oxidation of carbon to carbon monoxide?

C(s) + O2(g) → CO(g)

a)

x + y

b)

-x - y

c)

y - x

d)

x - y

63.

The standard enthalpy change of formation values of two oxides of phosphorus are:

P4(s) + 3O2(g) → P4O6(s) ΔHf = –1600 kJ mol–1

P4(s) + 5O2(g) → P4O10(s) ΔHf = –3000 kJ mol–1

What is the enthalpy change, in kJ mol–1, for the reaction below?

P4O6(s) + 2O2(g) → P4O10(s)

a)

+4600

b)

+1400

c)

–1400

d)

–4600

64.
In an endothermic reaction the system is releasing energy.
a)
True
b)
False
c)
Sometimes
65.
In an exothermic reaction, heat is ...
a)
taken in
b)
given out
c)
nothing happens
d)
it gets colder
66.

A chemical reaction that requires energy is a(n)

a)
exothermic reaction 
b)
endothermic reaction 
c)
over reaction 
d)
redox reaction
67.

If N2 (g) + 2O2 (g) ⟶\longrightarrow   2NO2(g) has a ΔHrxn \Delta H_{rxn\ }  = 68, then what is the ΔHrxn\Delta H_{rxn}  if you reverse the reaction?

a)

86 kJ

b)

- 86 kJ

c)

68 kJ

d)

-68 kJ

68.
a)
-233
b)
-11.3
c)
-805
d)
-226
69.

What is the oxidation number of chlorine in ClO3- ?

a)

-1

b)

+1

c)

-1

d)

+5

70.

Oxidation is....

a)

Gain of electrons

b)

Loss of electrons

c)

Both the loss and gain of electrons

d)

None of these

71.

Reduction is....

a)

Gain of electrons

b)

Loss of electrons

c)

Both the loss and gain of electrons

d)

None of these

72.

Which of the following elements is the strongest oxidizing agent?

a)

Chlorine

b)

Aluminium

c)

Hydrogen

d)

Lithium

73.

What is the oxidation state of sulphur in SO42- (aq)?

a)

4

b)

6

c)

2

d)

0

74.

What is the oxidation state of Nitrogen in N2 (g)?

a)

4

b)

6

c)

2

d)

0

75.
What substance is oxidized in the following reaction?
4Fe + 3O2 --> 2Fe2O3
a)
Iron
b)
Fluorine
c)
Oxygen
76.

Substance that oxidizes another substance by accepting its electrons.

a)

reducing agent

b)

oxidation number

c)

combustion

d)

oxidizing agent

77.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
78.
Another name for a "oxidation-reduction" reaction is
a)
chemical reaction
b)
neutralization reaction
c)
redox reaction
d)
nuclear reaction
79.

What is the oxidation number of Nitrogen in HNO3

a)

-7

b)

-5

c)

+5

d)

+7

e)

+2

80.

The below reaction is an example of _________reaction.

F2 → 2 F- + 2 e-

a)

Oxidation

b)

Reduction

c)

Neutralization

d)

decomposition

e)

combustion

81.

Find the oxidation number of Ca in CaH2

a)

-2

b)

-4

c)

+2

d)

+4

e)

0

82.

Identify the substance that is reduced in the reaction between copper(II) ion and magnesium.

Cu2+ + Mg → Cu + Mg2+

a)

Cu2+

b)

Mg

c)

Cu

d)

Mg2+

83.

In a redox reaction, the species reduced

a)

gains electrons and is the oxidizing agent

b)

loses electrons and is the oxidizing agent

c)

loses electrons and is the reducing agent

d)

gains electrons and is the reducing agent

84.
Which statement is true:
Mg → Mg2+ + 2e–
a)
Mg gains 2 electrons
b)
Mg2+ loses 2 electrons
c)
Mg loses 1 electron
d)
Mg loses 2 electrons
85.
What substance is oxidized in the following reaction?
4Fe + 3O2 --> 2Fe2O3
a)
Iron
b)
Fluorine
c)
Oxygen

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