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M. 4/ Chemistry Final Exam Preparation

Total questions: 84

Worksheet time: 14hrs 0mins

Name
Class
Date
1.
The relative molecular mass of a compound is equal to the sum of its
a)
Atomic mass
b)
Atomic number
c)
Oxidation number
d)
Valence electrons
2.
What is the relative molecular mass of fluorine gas, F2?
a)
19
b)
38
c)
9
d)
18
3.

What is the relative formula mass of ammonium nitrate, NH4NO3 ?

[Relative atomic mass: N, 14; H, 1; O, 16]

a)

76

b)

79

c)

80

d)

90

4.
What is the atomic mass of magnesium?
a)
2
b)
4
c)
12
d)
24
5.
What is the relative formula mass of NaOH?
a)
20
b)
39
c)
40
d)
45
6.

Calculate the relative formula mass of

copper (ii) chloride, CuCl2


[Relative atomic mass:

O = 16 ; Al = 27 ; S = 32 ; Cl = 35.5 ; Cu = 64 ]

(a)  

7.

Calculate the relative formula mass of

aluminium sulphate, Al2(SO4)3


[Relative atomic mass:

O = 16 ; Al = 27 ; S = 32 ; Cl = 35.5 ; Cu = 64 ]

(a)  

8.

What is the relative atomic mass (Ar) of Carbon?

a)

6

b)

12

c)

18

d)

7

9.

What is the relative atomic mass (Ar) of Xenon (Xe)?

a)

54

b)

77

c)

131

d)

132

10.

What is the relative atomic mass (Ar) of Chlorine (Cl)?

a)

35.5

b)

17

c)

18.5

d)

0.5

11.

What is the relative molecular mass (Mr) of Hydrochloric Acid (HCl)?

a)

18

b)

34.5

c)

36.5

d)

35.1

12.
What is the mole used for? 
a)
To measure the amount of grams in a substance
b)
To measure the amount of atoms or molecules in a substance
c)
To measure the amount of energy in a substance
d)
To measure the amount of bonding in a substance 
13.
What is Avogadro's Number? 
a)
6.02 x 1023
b)
- 6.02 1023
c)
6.02 x 1022
d)
6,020,000,000,000
14.
What is the molar mass of H2O?
a)
6.02 x 1023
b)
16 grams
c)
18 grams
d)
15.99999 grams
15.
What is the molar mass NaCl?
a)
58 grams
b)
22.95 grams
c)
162 grams
d)
6.02 x 1023
16.
How many atoms are in 1 mole of NaCl? 
a)
6.02 x 1023
b)
58 
c)
11
d)
17
17.
How many moles are in 32 grams of Oxygen (O)? 
a)
3
b)
2
c)
1
d)
4
18.
How many grams are in 1.2 x 1024 molecules of CO?
a)
28 grams
b)
56 grams
c)
6.02 grams
d)
1.2 grams
19.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.05 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5 moles
20.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
21.
What is the mass of one mole of aluminum?
a)
27 g
b)
13 g
c)
54 g
d)
14 g
22.
What is the molar mass of CO2?
a)
12
b)
16
c)
32
d)
44
23.

Calculate the molar mass of Ba(C2H3O2)2

a)

255.3 g/mol

b)

237.3 g/mol

c)

228.3 g/mol

d)

196.3 g/mol

24.

Calculate the molar mass for Al(OH)3

a)

78.0 g/mol

b)

72 g/mol

c)

28 g/mol

d)

25 g/mol

25.
What is the molarity of 2.5 mol of NaOH in 12.0 L of solution?
a)
0.21 M
b)
30 M
c)
4.8 M
d)
20.8 M
26.
What is the molality of a solution containing 1.3 mol in 13.4 kg of solution?
a)
9.7 m
b)
17.42 m
c)
0.097 m
27.
What is the molarity of 122.5 g of AlCl3 in 1.0 L of solution?
a)
1.225 M
b)
0.92 M
c)
0.1225 M
28.
What is the molality of 1.2 g of HCl in 750 g of solution?
a)
0.04 m
b)
0.00004 m
c)
0.0016 m
29.
What is the concentration, in percent by mass, of 0.62 g of solute in 45.0 g of solution?
a)
0.014 %
b)
1.4 %
c)
0.13%
30.
What mass of solute is needed to make 75.0 g of a 3.4% solution?
a)
2.55 g
b)
22 g
c)
0.05 g
31.
What is the volume of solution needed to make a 3.5% by volume solution using 2.0mL of solvent?
a)
57 mL
b)
0.57 mL
c)
7 mL
32.

Molar mass of NaOH is ______________________

a)

40 grams/mol

b)

50 grams/mol

c)

45 grams/mol

d)

38 grams/nol

33.
Which sweet tea would you expect to taste the sweetest?
a)
1M
b)
3M
c)
3.1M
d)
2.5M
34.
True or False? The higher the concentration of a solution the less solutes it has in it.
a)
True
b)
False
35.

Molarity is measured in _____.

a)

moles per g.

b)

mols per L.

c)

moles per mm.

d)

moles per mL.

36.

The _____ is the thing being dissolved.

a)

solute

b)

solvent

37.

What is a solvent?

a)

The substance that does the dissolving in a solution.

b)

The substance that is being dissolved in a solution.

c)

The mixing of different substances.

d)

The process in which neutral molecules lose or gain electrons.

38.

A solution that is considered unsaturated would _____.

a)

be dark in color.

b)

have a strong scent.

c)

have a large amount of solute.

d)

have a small amount of solute.

39.
How many moles of NaCl are present in a solution with a molarity of 8.59 M and a volume of 125 mL?
a)
1074 mol
b)
0.069 mol
c)
1.07 mol
d)
62.7 mol
40.

What are the units of molarity?

a)

M

b)

m

c)

Ml

d)

Mr

41.

A student is preparing solutions for a laboratory experiment by dissolving solid solutes in liquid solvents. Which action will increase the rate of solubility

a)

lowering the temperature of the solvent

b)

stirring the solute in the solution

c)

increasing the pressure on the solution

d)

increasing the particle size of the solute

42.

Which of the following types of solutions has more room to dissolve solute?

a)

supersaturated

b)

saturated

c)

unsaturated

43.
The concentration of a mixture can be increased in which of the following ways?
a)
Heating the mixture
b)
Adding more water “solvent”
c)
Adding more powder “solute”
d)
Stirring the mixture
44.
How many liters would you need to make a 1 M solution if you have 6 mol of Sodium Hydroxide? 
a)
2
b)
3
c)
4
d)
6 
45.
What is the molarity of 4 g of NaCl (MM=58.45) in 3,800 mL of solution?
a)
0.018 M
b)
0.0011 M
c)
1.052 M
d)
0.062 M
46.
Find the molarity of 186.55 g of sucrose, C12H22O11 (MM = 342) in 250 mL of water.
a)
2.18 M
b)
0.746 M
c)
1.18 M
d)
0.545 M
47.
How many grams of AgNO3 (MM = 169.87) are needed to prepare 0.125M solution in 250 mL of water? 
a)
.03g
b)
0.5g
c)
5.3g
d)
84.9g
48.
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
49.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
50.
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
51.
Which one is an empirical formula?
a)
H2O2
b)
C2H6O12
c)
CaCl2
d)
N2O8
52.
What is the empirical formula for C3H8
a)
CH
b)
C3H8
c)
C6H16
d)
CH2.7
53.

C4H6

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

54.

Br2O6

a)

BrO3

b)

Br6O2

c)

BrO

d)

Br2O6

55.

C2H4

a)

CH

b)

CH2

c)

C4H2

d)

C2H4

56.

P2O6

a)

P2O6

b)

PO

c)

PO3

d)

P3O

57.

C25H45

a)

C25H45

b)

CH

c)

C5H9

d)

C9H5

58.

Si2F6

a)

SiF

b)

Si2F6

c)

SiF3

d)

Si6F2

59.

P3O4

a)

PO

b)

P3O4

c)

P4O3

60.

C2H6O

a)

CHO

b)

C2H6O

61.

S2O8

a)

S2O8

b)

SO

c)

SO4

d)

S8O2

62.

C2F6

a)

CF

b)

C2F6

c)

C6F2

d)

CF3

63.

N2S3

a)

NS

b)

N3S2

c)

N2S3

64.

What is the empirical formula for N2S3?

a)

NS

b)

N3S2

c)

N2S3

d)

N1S1.5

65.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
66.
What is the percent composition by mass of sulfur in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
67.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
68.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
69.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
70.
What is the percent composition by mass of oxygen in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
71.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
72.
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
73.
An empirical formula:
a)
is a formula that calculates the coefficients of a compound in a balanced equation.
b)
is the simplest whole-number ratio of moles of elements in the compound.
74.
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
75.
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
76.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
77.
Whats the empirical formula of a molecule containing 18.7% of Lithium, 16.3% of Carbon and 65.0% of oxygen?
a)
CO2Li3
b)
Li2CO3
c)
Li3CO2
d)
LiCO5
78.
What is the molecular formula for a compound with the empirical formula: K2SO4 and a molecular mass of 696g.
a)
K2SO4 
b)
K8SO16
c)
K8S4O8 
d)
K8S4O16 
79.
What is the molecular formula if the empirical formula is CH2O and the molecular molar mass is 180.18?
a)
CH2O
b)
C2H4O2
c)
C4H8O4
d)
C6H12O6
80.
A compound consists of 72.2% magnesium(Mg) and 27.8% nitrogen(N) by mass. What is the empirical formula?
a)
Mg4N3
b)
MgN2
c)
Mg3N2 
d)
MgN
81.
You are given the following percentages: 40.05% S and 59.95% O. Find the empirical formula for these elements.
a)
SO
b)
SO2
c)
SO3
d)
SO4
82.
What is the empirical formula if you have 81.82% carbon and 18.18% hydrogen?
a)
C3H8
b)
CH4
c)
C2H2
d)
C4H10
83.
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
84.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%

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