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CIE IG Chemistry Topic 3 Stoichiometry

Total questions: 75

Worksheet time: 2hrs 11mins

Name
Class
Date
1.
The relative atomic mass is the average mass of an atom compared to 
a)
the mass of a carbon-12 atom.
b)
1/12 the mass of a carbon-12 atom
c)
the mass of a hydrogen atom
d)
1/12 the mass of a hydrogen atom
2.
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
3.
What is the relative molecular mass of fluorine gas, F2?
a)
19
b)
38
c)
9
d)
18
4.
What is the unit of relative molecular mass?
a)
kilogram
b)
gram
c)
gram per mole (g/mol)
d)
no units
5.
The formula of a compound is M(OH)2. Given that the Mr of the compound is 98, calculate the Ar of M.
a)
32
b)
64
c)
81
d)
94
6.

Each element is defined by the number of

a)

Atoms

b)

Isotopes

c)

Neutrons

d)

Protons

e)

Nuclei.

7.

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

8.
What is the atomic mass of magnesium?
a)
2
b)
4
c)
12
d)
24
9.
What is the relative formula mass of NaOH?
a)
20
b)
39
c)
40
d)
45
10.

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)  

11.

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)  

12.

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

a)

6

b)

12

c)

18

d)

7

13.

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

a)

54

b)

77

c)

131

d)

132

14.

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

a)

35.5

b)

17

c)

18.5

d)

0.5

15.

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

a)

18

b)

34.5

c)

36.5

d)

35.1

16.
An element has two naturally occurring isotopes. One is 10.013 amu and is 19.9% abundant. The other is 11.01 amu and is 80.1% abundant. What is the average atomic mass? What element is it?
a)
9.012, Beryllium
b)
12.011, Carbon
c)
6.941, Lithium
d)
10.812, Boron
17.

Calculate the average atomic mass of silver.

a)

106.38649amu

b)

111.91896amu

c)

107.8677amu

d)

121

18.
Compute the average atomic mass for silicon:
a)
27.977
b)
28.09
c)
28.976
d)
The average mass cannot be determined from provided information.
19.

To calculate average atomic mass, you need

a)

the atomic mass of each isotope

b)

the percent abundance of each isotope

c)

the atomic mass and percent abundance of each isotope

d)

to find the average of the atomic masses of each isotope

20.
What do these isotopes of carbon all have in common?
a)
neutrons & mass number
b)
atomic number and neutrons
c)
atomic number and electrons
d)
protons, atomic number, and mass number
21.
How many neutrons does the isotope of lithium have?
a)
8
b)
3
c)
4
d)
5
22.
How many protons does this isotope of titanium have?
a)
48
b)
22
c)
26
d)
70
23.
What quantities vary between isotopes of an element?
a)
protons, electrons, and atomic mass
b)
protons, electrons, and atomic number
c)
neutrons and electrons
d)
neutrons and atomic mass
24.
which atom has  4 neutrons?
a)
Li-6
b)
Li-7
c)
Li-8
d)
they have the same # of neutrons
25.
How many neutrons in C-14?
a)
6
b)
7
c)
14
d)
8
26.
In what part of an atom can protons be found?
a)
inside the electron
b)
inside the neutron
c)
inside the atomic nucleus
d)
inside the electron shells
27.
If a sulfur atom has 16 protons, 16 electrons, and 16 neutrons, its atomic mass is:
a)
16
b)
32
c)
48
d)
64
28.
If a hydrogen atom has 1 proton, 1 electron, and 1 neutron, its atomic number is:
a)
1
b)
2
c)
3
d)
4
29.

What is meant by isotopes of an element?

a)

Atoms with different numbers of protons

b)

Atoms with different numbers of electrons

c)

Atoms with different numbers of neutrons

d)

Atoms with different atomic numbers

30.
What is the relative atomic mass of sodium?
a)
11
b)
23
c)
46
d)
64
31.
What is the relative molecular mass of fluorine gas, F2?
a)
19
b)
38
c)
9
d)
18
32.
What is the relative formula mass of NaOH?
a)
20
b)
39
c)
40
d)
45
33.

Find Atomic Mass: What is the mass of one mole of Lithium (Li)?

a)

6.9 grams

b)

14.0 grams

c)

22.9 grams

d)

56.9 grams

34.

Find Molecular Mass: Calculate the mass of one mole of CO2 (carbon dioxide).

a)

18.0 grams

b)

44.0 grams

c)

14.0 grams

d)

180.0 grams

35.

AgF....

a)

is an element because it has 2 different types of atoms.

b)

is a compound because it has 2 different types of atoms.

c)

is a compound because it has 2 of the same types of atoms.

d)

is an element because it has 2 of the same types of atoms.

36.

How many atoms of NITROGEN are in S(NH4)2 ?

a)

0

b)

1

c)

2

d)

4

37.

The mass of a tungsten atom is 2.4 times greater than the mass of a neon atom. What is the relative atomic mass of tungsten?

[RAM: Ne, 20]

a)

8

b)

22

c)

48

d)

52

38.

How many oxygen atoms have equal mass with two magnesium atoms?

[RAM: O, 16; Mg, 24]

a)

2

b)

3

c)

4

d)

5

39.

Four atoms of element X have the same mass with 11 atoms of sulphur. What is the relative atomic mass of element X?

[RAM: S, 32]

a)

44

b)

88

c)

128

d)

352

40.

An oxide of nitrogen has the formula, N2O4. What is its relative molecular mass?

[RAM: N, 14; O, 16]

a)

76

b)

78

c)

92

d)

120

41.

How many times is a water molecule heavier than a hydrogen molecule?

[RAM: H, 1; O, 16]

a)

2

b)

8

c)

9

d)

18

42.

Sodium thiosulphate has the formula of Na2S2O3 . 5H2O. What is its relative formula mass?

[RAM: H, 1; O, 16; Na, 23; S, 32]

a)

158

b)

232

c)

248

d)

264

43.

Silica gel contains a sodium compound with the formula Na2Si4Oy. If the relative formula mass of the compound is 302, what is the value of y?

[RAM: O, 16; Na, 23; Si, 28]

a)

8

b)

9

c)

10

d)

12

44.

The average mass of nitrogen gas is 28 times greater than that of the mass of 1/12 carbon-12 atom. Calculate the relative atomic mass of nitrogen.

a)

1

b)

2

c)

14

d)

28

45.

The relative molecular mass of substance PR2 is 95. If the relative atomic mass of an element of atom R is 35.5, calculate the relative atomic mass of an atom of element P.

a)

8

b)

24

c)

16

d)

64

46.

An oxide of element Q has a formula Q3O4 and relative formula mass of 145. Calculate the relative atomic mass of element Q.

[RAM: O = 16]

a)

18

b)

27

c)

44

d)

50

47.

What is the relative molecular mass of nitrogen gas ?

Ar N = 14 gram

a)

14

b)

16

c)

28

d)

7

48.
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
49.
Which of the following is considered an empirical formula?
a)
CH3COOH
b)
C6H12O6
c)
H2O
50.
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
51.
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
52.
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
53.

What is the empirical formula for C4H6?

a)

CH

b)

CH3

c)

C2H3

d)

C4H6

54.

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

55.

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

56.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
57.

A compound consists of 72.2% magnesium and 27.8% nitrogen by mass. What is the empirical formula?

a)

Mg4N3

b)

MgN2

c)

Mg3N2

d)

MgN

58.

Given the following, determine the empirical formula: 42.07% sodium, 18.89% phosphorus, and 39.04% oxygen.

a)

NaPO2

b)

Na2PO3

c)

Na3PO4

d)

Na3PO3

59.
What is the molar mass of NaOH?
a)
368 g/mole 
b)
40 g/mole
c)
57 g/mole
d)
23 g/mole
60.
What is the mass of one mole of AuCl3?
a)
96g
b)
130g
c)
232.5g
d)
303.5g
61.
What is the mass of one mole of (NH4)2CO3?
a)
144g
b)
138g
c)
96g
d)
74g
62.
36.0 g of Be contains how many moles?
a)
0.25 mol
b)
4.0 mol
c)
45 mol
d)
320 mol
63.
4.0 moles of H2O would have what mass?
a)
72 g
b)
23 g
c)
68 g
d)
4.5 g
64.
A mass of 6 g of Carbon contains
a)
1 mole of C
b)
2 moles of C
c)
0.5 moles of C
d)
72 moles of C
65.
How many moles are in 15 grams of lithium?
a)
0.5 moles
b)
104.1 moles
c)
2.2 moles
d)
50 moles
66.
How many moles are in 2.3 grams of phosphorus?
a)
0.07 moles
b)
71.3 moles
c)
13.5 moles
d)
20 moles
67.
Theoretical yield = 73g
Actual yield = 62g
Calculate the percent yield.
a)
1.16%
b)
116%
c)
85%
d)
76%
68.
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
69.
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
70.
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%
71.
CH4 + 2H2O --> CO2 + 4H2
What is the limiting reactant when 20g CH4 react with 15g H2O?
a)
CH4
b)
H2O
c)
CO2
d)
H2
72.
2 NaCl + Pb(NO3)2 --> 2 NaNO3 + PbCl2
 
How many grams of lead II chloride are produced from the reaction of 15.3 g of NaCl and 60.8 g of Pb(NO3)2? 
a)
21.5g
b)
51.1g
c)
43.4g
d)
36.4g
73.
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%
74.
Your percent yield is 80%. The actual amount of product produced was 29.1 grams. What is the theoretical yield?
a)
25.2 grams
b)
37.3 grams
c)
37.1 grams
d)
36.3 grams
75.
When reacting Na with Cl2, we calculated that the theoretical yield should be 12.5 grams. Our actual yield was 13.0 grams. What is the percent yield?
a)
100%
b)
104%
c)
96%
d)
1.04

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