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Grade 10 final exam revision Term2

Total questions: 88

Worksheet time: 5hrs 39mins

Name
Class
Date
1.
A formula with the lowest whole # ratio of elements in a compound is called
a)
Molecular Formula
b)
Chemical Formula
c)
Empirical Formula 
d)
Distance Formula
2.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

3.

What is the empirical formula for N2S3?

a)

NS

b)

N3S2

c)

N2S3

d)

N1S1.5

4.

Si2F6

Choose the correct empirical formula...

a)

SiF

b)

Si2F6

c)

SiF3

d)

Si6F2

5.
A chemical formula that shows the actual # and kinds of atoms present in one molecule of a compound is called_________
a)
ionic formula
b)
covalent formula
c)
empirical formula
d)
molecular formula
6.

C2H6O

Which is the correct empirical formula

a)

CHO

b)

C2H6O

c)

C4H14O2

d)

None

7.
Given the following: 42.07% Na, 18.89% P, and 39.04% O, determine the empirical formula.
a)
 NaPO2
b)
Na2PO3
c)
Na3PO4
d)
NaPO4
8.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
9.
Glycerol has a molar mass of 92.09g/mol. Its percent composition is: 39.12% C, 8.75% H, and 51.12% O. What is the molecular formula for glycerol?
a)
C2H3O2
b)
CH2O
c)
C2H4O2
d)
C3H8O3
10.

For the following balanced chemical equation

2K + F2 --> 2KF

how many moles of KF are present?

a)

2 mol of KF

b)

1 mol KF

11.

6.0 mol of aluminium reacts with oxygen to form aluminium oxide. What is the amount of oxygen, in mol, needed for complete reaction?

4Al(s) + 3O2(g) → 2Al2O3(s)

a)

1.5

b)

3.0

c)

4.5

d)

6.0

12.

Nitrogen reacts with hydrogen to give ammonia, NH3 in a closed container. How many moles of H2 are needed to produce 25 mol of NH3?

N2 + 3H2 → 2NH3

a)

A) 12.5

b)

B) 25

c)

C) 37.5

d)

D) 50

e)

E) 62.5

13.

For the following balanced chemical equation

2Al(s) + 6HCl(l) → 2AlCl3(s) + 3H2(g)

how many moles of H2 are present?

a)

1 mol

b)

2 mol

c)

3 mol

d)

4 mol

e)

6 mol

14.

In a stoichiometric calculation to determine the mass of one substance that will react with a given amount, in moles, of a second substance, you need to know

a)

only the mole ratio of the unknown substance to the given substance.

b)

only the molar mass of the given substance.

c)

both the mole ratio of the unknown substance to the given substance and the molar mass of the unknown substance.

d)

the molar masses of all products and reactants.

15.

6.0 mol of aluminium reacts with oxygen to form aluminium oxide. What is the amount of oxygen, in mol, needed for complete reaction?

4Al(s) + 3O2(g) → 2Al2O3(s)

a)

1.5

b)

3.0

c)

4.5

d)

6.0

16.
For the Balanced Reaction: 3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe; What is the Ratio of moles of MgO to moles Fe?
a)
3mol Mg / 2 mol Fe
b)
2 mol Mg/ 3 mol Fe
c)
1 mol Fe/ 2 mol Fe
d)
3 mol MgO / 2 mol Fe
17.
N2 + 3H2 --> 2NH3
What is the total number of moles of NH3 produced when 10 moles of H2 reacts completely with N2?
a)
6.7
b)
2.0
c)
3.0
d)
15.0
18.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of water needed to make 2.5 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
19.
6CO2 + 6H2O --> C6H12O6 + 6O2 
What is the total number of moles of CO2 needed to make 2 moles of C6H12O6?
a)
2.5
b)
6
c)
12
d)
15
20.
What coefficient should be used to make the following equation balanced?
N2+O2--> _NO 
a)
1
b)
2
c)
3
d)
4
21.
Which problem is balanced?
(Check ALL answers)
a)
PbO2 + 2H2
b)
SO2 + H20 --> H2SO4
c)
2Na + 2H2O --> 2NaOH + H2
22.
How many HCl molecules do you need to balance this equation? 
Mg +  __HCl --->  MgCl2 + H2
a)
1
b)
2
c)
3
d)
4
23.

A balanced chemical equation allows one to determine the

a)

mole ratio of any two substances in the reaction.

b)

energy released in the reaction.

c)

electron configuration of all the elements in the reaction.

d)

mechanism involved in the reaction.

24.

In the equation 2Al2O3 ----> 4Al + 3O2, what is the mole ratio of aluminum to oxygen?

a)

10:6

b)

3:4

c)

2:3

d)

4:3

25.

Gas grills use propane fuel. The combustion of propane is represented in this equation:

C3H8 + 5O2 ----> 3CO2 + 4H2O. How many grams of propane will burn when 36.0 moles of water are formed?

a)

0.500 g C3H8

b)

9.00 g C3H8

c)

318 g C3H8

d)

397 g C3H8

26.

N2 + 3H2 → 2NH3

What is the mole ratio between N2 and NH3 in the above reaction?

a)

1 moles NH3 / 2 moles N2

b)

2 moles NH3 / 1 moles N2

c)

2 moles N2 / 3 moles NH3

d)

1 moles N2 / 3 moles NH3

27.
Calculate the % composition by mass of oxygen present in H2SO4.
a)
16.3%
b)
65.25%
c)
32.6%
d)
57.14%
28.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
29.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
30.
What is the percent composition of Benzene, C6H6?
a)
C = 50%
H = 50%
b)
C = 85.7 %
H = 14.3%
c)
C = 92.2%
H = 7.8%
d)
C = 71.9%
H = 28.1%
31.
If 15.6 g of hydrate are heated and only 11.7 g of anhydrous salt remain, calculate the % of water lost.
a)
25.9%
b)
19.2%
c)
37.9%
d)
76.3%
32.
Consider the Equation:
2H2  +   O2    −−〉 2H2O
How many moles of water can be formed from 3.91 g of O2?
a)
1.905
b)
.244
c)
2.2
d)
1.1
33.
What is the limiting reactant if 10.0 moles of NH3  react  with 30.0 moles of NO?
4NH3 + 6NO → 5N2 + 6H2O
a)
NH3
b)
NO
c)
N2
d)
H2O
34.
Use the following equation:
NaIO3(aq) + 6HI(aq) --> 3I2(s) + NaI(aq) + 3H2O(l)
How many moles of iodine can be made from 6.55 moles of NaIO3?
a)
4.55 moles I2
b)
23.18 moles I2
c)
19.65 moles I2
d)
34.99 moles I2
35.

If 4.50 g of HCl is reacted with 15.0 g of CaCO3 according to the following chemical equation,

2HCl + CaCO3 → CaCl2 + H2O + CO2

Calculate the theoretical yield (in gram) of CO2?

a)

2.05 g

b)

4.12 g

c)

3.02 g

d)

2.71 g

36.

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

37.

How many grams of MgCl2 will be produced when 6.00 g HCl combines with 5.00 g Mg?

Mg + 2HCl --> MgCl2 + H2

a)

19.6 g

b)

39.4 g

c)

7.72 g

d)

1.08 g

38.
N2 +  3H2 → 2NH3 
How many moles of hydrogen are needed to react with 5 moles of nitrogen?
a)
6
b)
2
c)
3
d)
15
39.
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
40.
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
41.

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%

42.

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

43.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
44.
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%
45.

11.

LiOH + KCl → LiCl + KOH


b) I actually produced 6 grams of lithium chloride and I began this reaction with 20.0 grams of lithium hydroxide. What is my percent yield?

a)

16.9%

b)

5.91%

c)

1.88%

d)

12.3%

46.
At a constant pressure, the volume decreases.  What happens to the temperature?
a)
increases
b)
decreases
c)
stays the same
47.
Which of the following is NOT a part of Kinetic Molecular Theory?
a)
Gas particles have mass and occupy space (the individual particles have volume)
b)
Gas particles do not have mass and occupy space (the individual particles have volume
c)
Gas particles move in straight lines
d)
The more heat energy the gas particles have, the faster they move
48.
Diffusion is
a)
the ability of one gas to mix with another gas.
b)
the rate at which a gas flows through the air.
c)
an explosion of gases.
d)
the ability of a gas to move from a high pressure to a low pressure.
49.
Calculate the relative ratio of the rates of effusion (diffusion) of oxygen to nitrogen. Remember to use the equation for Dalton's Law... 
a)
4.00
b)
1.07
c)
3.74
d)
0.94
50.
A gas
a)
has a definite shape but no definite volume
b)
has a definite volume but no definite shape
c)
has fast-moving particles
51.
Dalton's Law states...
a)
that at a constant temperature the volume of a confined ideal gas varies inversely with its pressure.
b)
that the total pressure exerted by the mixture of non-reactive gases is equal to the sum of the partial pressures of individual gases
c)
how gases tend to expand when heated
d)
that the density of an ideal gas at constant pressure varies inversely with the absolute temperature of the gas.
52.
Which equation represents Dalton's Law?
a)
e=mc2
b)
PV=nRT
c)
P1/T1=P2/T2
d)
Ptotal=P1, P2, P3...
53.
Three gases, Ar, N2 and H2 are mixed in a 500L container. Ar has a pressure of 255 torr, N2 has a pressure of 228torr and H2 has pressure of 752torr. What is the total pressure in the container?
a)
483torr
b)
270torr
c)
1235torr
54.
A mixture of hydrogen, nitrogen, and water vapor has a total pressure of 864 mmHg. The partial pressure of hydrogen is 220 mmHg and that of nitrogen is 410 mmHg. What is the partial pressure of water vapor?
a)
234 mmHg
b)
1.37 mmHg
c)
2.64 mmHg
d)
1, 494 mmHg
55.

Use Graham’s Law to calculate fast O2 gas will effuse compared to Cl2. SHOW YOUR WORK ON PAPER

a)

O2 effuses 1.5 times faster than Cl2

b)

O2 effuses 0.67 times as fast as Cl2

c)

O2 effuses 2.2 times faster than Cl2

d)

O2 effuses 0.45 times as fast as Cl2

56.
The rate of effusion is _______________ proportional to the square root of its' molar mass. 
a)
Directly
b)
Inversely 
57.
Lighter gases have a ________________ rate of effusion.
a)
faster 
b)
slower
c)
rate of effusion does not depend on mass.
58.
Which of the following would have a faster rate of effusion: 15g of Kr or 15g of N2?
a)
Kyrpton
b)
Nitrogen
c)
Both would have the same rate of effusion
59.

Grahams law refers specifically to

a)

the rate of diffusion

b)

the rate of effusion

c)

the temperature of gases

d)

the partial and total pressures of gases in a sample.

60.
how many times faster does He effuse compared to N2 (He = 4  N2 = 28)
a)
1.2 times faster
b)
2.65 times faster
c)
7 times faster
d)
0.377 times faster
61.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
62.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

63.

Intermolecular forces for: NH3

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

64.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
65.
Ionic Bonding involves...
a)
The transfer of protons
b)
The transfer of nuetrons 
c)
The transfer of electrons
d)
None Of the above
66.

Which substance has the weakest intermolecular forces?

a)

Substance A, boiling point of 75 °C

b)

Substance B, boiling point of 105 °C

c)

Substance C, boiling point of 25 °C

d)

Substance d, boiling point of 45 °C

67.

Intermolecular forces for: CO2

a)

Dispersion Force

b)

Dipole dipole

c)

Hydrogen bonding

68.
London forces are stronger in heavier atoms or molecules, and weaker in lighter atoms or molecules.  Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
I2
d)
Cl2
69.
Hydrocarbons will have which type of intermolecular forces?
a)
Dispersion
b)
dipole
c)
hydrogen bonds
70.
Which noble gas has the highest boiling point?
a)
Xe
b)
Kr
c)
Ar
d)
He
71.
Type of intermolecular force present in I2, Br2, and Cl2.
a)
dipole dipole
b)
H-bond
c)
dispersion
d)
metallic
72.
H2S has what kind of intermolecular force?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
73.
Intermolecular forces are the forces
a)
within molecules
b)
between molecules
74.
Which of the following has the highest boiling point?
a)
H2
b)
NH3
c)
N2
d)
O2
75.
Which of the following has the lowest boiling point?
a)
CaCl2
b)
PH3
c)
Cl2
d)
N2
76.
Intermolecular force present in HCl?
a)
dipole dipole
b)
dispersion
c)
H-bond
d)
ionic
77.

Which intramolecular force has the greatest strength?

a)

ionic bond

b)

nonpolar covalent

c)

polar covalent

78.

Which of these is the weakest intermolecular force?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

79.

Which intermolecular force do all molecules have?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

80.

Which intermolecular force requires hydrogen and one of the following: nitrogen, oxygen, fluorine?

a)

Dipole-dipole

b)

Hydrogen bonding

c)

London dispersion forces

81.

Which intermolecular force is characterized by partial charges?

a)

Dipole-dipole forces

b)

Hydrogen bonding

c)

London dispersion forces

82.
All molecules have London forces between them, but dipole-dipole and hydrogen bonding are so much stronger that when they are present we can ignore London forces.  Which of these has ONLY London forces?
a)
I2
b)
NH3
c)
OCl2
d)
SH2
83.

Which substance would have the weakest intermolecular forces of attraction?

a)

CH4

b)

NaCl

c)

H2O

d)

MgF2

84.
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
85.
SO2 + PCl5 --> SOCl2 + POCl3
How much SOCl2 is produced when 16.2g SO2 react with 13.7g PCl5? 
a)
7.87g
b)
30.1g
c)
26.4g
d)
19.8g 
86.
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
87.
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
88.
4NH3 + 5O2 --> 4NO + 6H2O
How many grams of NO are formed if 6.30g of ammonia react with 1.80g of oxygen? 
a)
0.37g
b)
0.045g
c)
1.35g
d)
11.1g

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