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Cfe Q3

Total questions: 88

Worksheet time: 21hrs 21mins

Name
Class
Date
1.

Use the information in your databook to calculate the enthalpy change for the following reaction:

H2(g) + Cl2(g) --> 2HCl(g)

a)

172

b)

200

c)

-185

d)

450

2.

1. Chloromethane can be produced by the reaction of methane with chlorine.


CH4(g) + Cl2(g) --> CH3Cl(g) + HCl(g)

Using bond enthalpies from the data booklet, calculate the enthalpy change, in kJmol−1, for this reaction

a)

26

b)

-234

c)

15

d)

-115

3.

1. 0.22g of propane (C3H8) was used to heat 200cm3 of water. The temperature of water was raised by 35oC. Calculate the enthalpy of combustion of propane.

a)

-5852

b)

-3218

c)

2297

d)

3456

4.

The enthalpy of combustion can be described as

a)

When 1 mole of solute dissolves in water

b)

When 1 mole of substance is fully combusted in oxygen

c)

1 one mole of water is produced in a neutralisation reaction

5.

6.9 g of ethanol (C2H5OH) was burned and the heat produced was used to raise the temperature of one litre of water by 49oC. Assuming all the heat released by the burning ethanol was absorbed by the water; calculate the enthalpy of combustion of ethanol.

a)

204

b)

1365

c)

-1365

d)

-768

6.

1. The enthalpy of combustion of methanol (CH3OH) is -715kJ mol-1. What mass of methanol would be burned to produce 71.5kJ of energy?

a)

6.4

b)

32

c)

3.2

d)

7.15

7.

Use Hess's Law to calculate the enthalpy of combustion of methane

a)

- 891 KJ mol-1

b)

- 605 KJ mol-1

c)

- 1041 KJ mol-1

d)

- 1435 KJ mol-1

8.

Calculate the enthalpy of combustion of ethane using Hess's Law

a)

- 1561 KJ mol-1

b)

- 1731 KJ mol-1

c)

- 1167 KJ mol-1

d)

- 989 KJ mol-1

9.

Using bond enthalpies in the data booklet, calculate the energy to convert 2 moles of O2 molecules into 4 moles of oxygen atoms in the below reaction.


2 O2 ------------> 4 O

a)

996 KJ

b)

1192 KJ

c)

- 996 KJ

d)

996 KJmol-1

10.
Equilibrium is a __________ process
a)
Static
b)
Dynamic
c)
Probabilistic
d)
Fictitious
11.
At equilibrium the concentration of all species in the reaction is _________.
a)
Constant
b)
Increasing
c)
Decreasing
d)
Oscillating
12.
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
13.
At what time the reaction reached equilibrium?
a)
t1
b)
t2
c)
t3
d)
t4
14.
This symbol indicates that a reaction is ____________
a)
reversible
b)
irreversible
15.
When the system X + 2 Y <=> Z has reached equilibrium, which of the following is TRUE?
a)
Forward reaction and Backward reaction stop.
b)
Forward reaction has sped up and backward reaction has slowed down.
c)
Forward and backward reactions occur at the same rate.
d)
Forward reaction has slowed down and backward reaction has sped up.
16.
For the reaction...
SO2 + O2  <=>  SO3
If the concentration of SO2 is increased, the equilibrium position of the reaction will shift ___________.
a)
to the left
b)
to the right
c)
to the left and right 
d)
neither left nor right
17.
For the reaction...
N2  +  O2  <=>  2NO
If  O2 is removed, the  concentration of N2 will _______.
a)
increase
b)
decrease
c)
remain the same
d)
double
18.
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)
19.
For the reaction...
N2  +  O2  <=>  2NO:  Δ H = +182 kJ mol-1.
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
20.
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
21.
Le Chatelier's Principle states that.... 
If a (dynamic) equilibrium is disturbed by changing the conditions, the position of equilibrium................
a)
moves to increase the change
b)
moves to counteract the change
c)
does not change
22.
Changes in pressure will only affect substances that are in the __________ state.
a)
gaseous
b)
liquid
c)
solid
23.

Increasing the temperature of the reaction in the Haber Process shifts results in equilibrium

a)

moving to the right

b)

moving to the left

c)

unchanged

24.

As pressure in the Haber Process is increased equilibrium shifts

a)

to the right

b)

to the left

c)

unchanged

25.
The ______________ yield is the maximum amount of product possible in a reaction. This determines the amount of product that should be produced in a perfect setting
a)
Percent
b)
actual
c)
stoichiometry
d)
theoretical
26.

When reacting Na with Cl2, we calculated that the theoretical yield should be 13 grams. Our actual yield was 12.5 grams. What is the percent yield?

a)

90.4%

b)

104%

c)

96.15%

d)

1.04%

27.
In a lab, a scientist calculate he should produce 12.3 grams of product in his experiment. When he is finished collecting his product it weighs 10.1 grams. What is his percent yield?
a)
82%
b)
0.82%
c)
10.1 %
d)
100%
28.
If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
a)
theoretical yield
b)
mole ratio
c)
actual yield
d)
percentage yield
29.
7. The amount of product that actually forms when a chemical reaction is carried out in a laboratory is called the _________ yield.
a)
actual
b)
theoretical
c)
percent
30.
CH4  +  2O2  →  CO2  +  2H2O
24 grams of CH4 was added to the above reaction. Calculate the theoretical yield of CO2.
a)
66 grams
b)
132 grams
c)
33 grams
d)
8.72
31.

2Fe2O3 + C → Fe + 3CO2

You add 28 grams of carbon. You find the actual yield to be 181.2 grams of CO2. What is the percent yield of CO2? (Hint: calculate theoretical yield of CO2 first)

a)

58.83%

b)

308%

c)

6435%

d)

15.5

32.
P4 + 6Cl2 --> 4PCl3 
The reaction of 75.0g P4 with excess chlorine gas produces 110g PCl3 in lab. Find the theoretical yield and calculate percent yield for the reaction. 
a)
78%
b)
64%
c)
27%
d)
33%
33.

The reaction of 25.0 g benzene, C6H6, with excess HNO3 resulted in 21.4 g C6H5NO2. What is the percentage yield?

C6H6 + HNO3 → C6H5NO2 + H2O

a)

100%

b)

27.39%

c)

54.29%

d)

85.62%

34.

Percent yield can never be greater than ________.

a)

theoretical yield

b)

100%

c)

both a and b

d)

50%

35.
Which type of reaction takes place in the presence of oxygen and produces carbon dioxide and water?
a)
double replacement 
b)
decomposition 
c)
combustion 
d)
single replacement
36.
The word oxidation describes 
a)
gain of electrons
b)
loss of electrons 
c)
number of electrons remains the same
d)
number of electrons transfered
37.
The word reduction describes 
a)
gain of electrons 
b)
loss of electrons 
c)
number of electrons remains the same
d)
transfer of electrons
38.
The Law of Conservation of Mass states
a)
that matter exists in all states and reacts the same
b)
that matter can only be changed into new substances by introducing a catalyst
c)
that matter exists in the same state throughout any chemical change
d)
that matter cannot be created or destroyed and that the mass of the products must equal the mass of the reactants
39.
How many Al atoms are in this compound?         4Al2O3
a)
2
b)
8
c)
6
d)
4
40.
How many F atoms are in this compound?
6MgF2 
a)
2
b)
6
c)
8
d)
12
41.

Why are chemical equations always balanced? Select ALL that apply.

a)

Matter cannot be created.

b)

Matter cannot be destroyed.

c)

Matter can only be rearranged/conserved.

d)

Matter doesn't matter.

42.

In a chemical reaction, if the reactants are heated, the reaction usually happens

a)

slower

b)

faster

c)

at the same rate

d)

in a smaller volume

43.
True or False
In a chemical reaction, no new atoms are created, and no atoms are destroyed. 
a)
true
b)
false
44.
Which of the following answers will balance the equation below?
__K + __Br2 --> __KBr
a)
2, 1, 1
b)
2, 3, 2
c)
2, 1, 2
d)
1, 2, 3
45.
If the reactants on the left side of a chemical equation are C₃H₈ + 5O₂, the products in a balanced equation could be
a)
4CO₂ + 3H₂O
b)
3CO₂ + 4H₂O
c)
2CO₂ + 3H₂O
d)
3CO + 4H₂O
46.
What is a limiting reactant?
a)
the reactant that determines how much product can be made
b)
the reactant that is in excess
c)
the product that you can make the most of
d)
the amount of reactants that react with each other
47.
When 12 moles of O2 reacts with 1.1 mole of C10H8 what is the limiting reactant?  C10H8 + 12 O2 --> 10 CO2 + 4 H2O
a)
Oxygen
b)
C10H8
c)
Water
d)
Carbon Dioxide
48.
The limiting reactant
a)
slows the reaction down
b)
is used up first
c)
is the reactant that is left over
d)
controls the speed of the reaction
49.

It refers to the substance(s) that are considered to be "ingredients" of a chemical reaction.

a)

reactants

b)

products

c)

catalysts

d)

enhancers

50.

Use the equation 2 Al + 3 Cl2 ---> 2 AlCl3. If 2 moles of aluminum and 2 moles of chlorine are reacted, identify the limiting reactant.

a)

AlCl3

b)

Cl2

c)

Al

51.
When does a chemical reaction stop?
a)
When the lab is finished
b)
When the excess reactant is used up
c)
When the limiting reactant is used up
d)
Chemical reactions never stop
52.
What is the limiting reactant if 10 moles of NH3  react  with 30.0 moles of NO?
4NH3+6NO --> 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
water
53.

The excess reactant

a)

is the reactant that is left over

b)

is used up first

54.

Why is it important to identify the limiting reagent?

a)

The limiting reagent speeds up the reaction.

b)

The limiting reagent controls the amount of product formed.

c)

If there is no limiting reagent, the reaction will not occur.

d)

No stoichiometry calculations can be done without a limiting reagent.

55.
Zn + 2HCI → ZnCI2 + H2. If 0.3 mol Zn and 0.52 mol HCI added, which is limiting?
a)
Zn
b)
HCI
c)
ZnCI2
d)
None of the above
56.

The quantity, 22.4 L, is called the ........................ of a gas.

a)

molar volume

b)

molar mass

c)

Atomic volume

57.

Oxidation is the _________ of electrons.

a)

loss

b)

gain

c)

sharing

d)

transfer

58.

Reduction is the ___________ of electrons.

a)

loss

b)

gain

c)

sharing

d)

transfer

59.

In the reaction Zn + 2HCl --> ZnCl2 + H2

which element, if any, is oxidized?

a)

Zinc

b)

Hydrogen

c)

Chlorine

d)

None

60.
In the reaction
2Ca(s) + O2(g) --> 2CaO(s), calcium is __________
a)
Reduced
b)
Synthesized
c)
Oxidized
d)
None of the above
61.
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
62.
Which of the following half reactions correctly represents a reduction half reaction?
a)
Fe →Fe2+ + 2e-
b)
Pb4+ + 2e- →Pb2+
c)
2O-2 →O2 + 4e-
d)
Fe + 3e- →Fe3+
63.

The forward reactions in the Electrochemical Series are examples of...

a)

Oxidation

b)

Reduction

64.

Gaining hydrogen is an example of...

a)

oxidation

b)

reduction

65.

Gaining oxygen is an example of...

a)

oxidation

b)

reduction

66.

A redox equation has...

a)

electrons on the left side

b)

electrons on the right side

c)

electrons on both sides

d)

no electrons on either side

67.

In a redox reaction, spectator ions...

a)

become oxidised

b)

become reduced

c)

remain unchanged

68.
acid + base ₋>
a)
salt + hydrogen
b)
salt + water
c)
salt + carbon dioxide + water
d)
salt
69.
HCl + NaOH → 
a)
NaH + ClOH
b)
NaCl + H2
c)
NaCl + H2O
d)
NaCl + Cl2
70.
I am titrating 1M HCl with 1M NaOH.  I have 25mL of HCl. How much NaOH will I need?
a)
2.5mL
b)
5mL
c)
25mL
d)
50mL
71.
what is the reading on this burette?
a)
4.40mL
b)
3.50mL
c)
3.60mL
d)
4.50mL
72.
I have 25mL of 1M HCl which neutralises 20mL of NaOH. What is the concentration of the NaOH?
a)
0.8 M
b)
1 M
c)
1.25 M
73.

MnO4- + 5Fe2+ + 8H+ --> Mn2+ + 4H2O + 5Fe3+

What volume of 0.01M MnO4- reacts with 0.002 moles of Fe2+

a)

0.1 dm3

b)

0.04 dm3

c)

0.4 dm3

d)

1.0 dm3

74.

2MnO4- + 6H+ + 5H2O2 --> 2Mn2+ + 8H2O + 5O2

How many moles of H2O2 react with 0.4 moles of MnO4- reacts

a)

0.4

b)

0.2

c)

1.0

d)

5.0

75.

2MnO4- + 6H+ + 5H2O2 --> 2Mn2+ + 8H2O + 5O2

What volume of 0.5M H2O2 react with 0.01 moles of MnO4- reacts

a)

0.01 dm3

b)

0.05 dm3

c)

0.04 dm3

d)

0.1 dm3

76.

Ink can be separated by a method of -----------------------------------------------

a)

distillation

b)

filtration

c)

chromatography

d)

sedimentation

77.

On the chromatogram given, ___________ is a mixture.

a)

red

b)

orange

c)

green

d)

black

78.

A pure substance shows ____ spot on a chromatogram

a)

0

b)

1

c)

2

d)

3

79.
The diagram below shows a chromatogram obtained when a sample X was analysed together with four other known dyes P, Q, R and S. Dye Q was known to cause cancer. Which of the following dye(s) is/are safe for use?
a)
P only
b)
S only
c)
P and S
d)
P and X
80.

C6H8O7 + 3NaOH → C6H5O7Na3 + 3H2O


Calculate the percentage atom economy for the production of sodium citrate, C6H5O7Na3.

a)

82.7%

b)

90%

c)

93.5%

81.

Iron can be produced from iron(III) oxide.


2Fe2O3(s) + 3C(s) → 4Fe(s) + 3CO2(g)


The atom economy for the production of iron is

a)

69.9%

b)

62.8%

c)

58.2%

d)

32.5%

82.

100 cm3 of propane is mixed with 600 cm3 of oxygen and the mixture is ignited.


C3H8(g) + 5O2(g) → 3CO2(g) + 4H2O(ℓ)


At the end of the reaction, the total volume of gas would be

a)

300cm3

b)

400cm3

c)

700cm3

d)

800cm3

83.

In a redox titration with potassium permanganate, no indicator was added, why?

a)

a pH meter is used

b)

It is a self-indicating reaction

84.

In a redox titration, what is the purpose of adding concentrated sulphuric acid to the reaction mixture?

a)

to increase the pH

b)

to provide H+ ions

c)

to slow down the reaction

d)

to heat it up

85.

This chromatogram from a gas chromatography shows that there is a higher concentration of sucrose than glucose

a)

true

b)

false

86.

Stachyose has a higher retention time than sucrose, this means that it spends less time on the gas chromatography column

a)

true

b)

false

87.

These are results from a titration experiment. The average volume used for calculations must be taken from results that are concordant (within 0.2cm3 of eachother). Which results can be used to obtain the average.

a)

3, 4 and 5

b)

2, 3, 4 and 5

c)

4 and 5

d)

all of them

88.

The first titration result is never used to calculate the average, this is because it is used as a 'rough' guide to the endpoint.

a)

true

b)

false

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