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Chemical Formulas and the Mole

Total questions: 48

Worksheet time: 2hrs 9mins

Name
Class
Date
1.

How many grams are there in 4 moles of H2O?

a)

64

b)

38

c)

72

2.

How many mole are there in 51 grams of NH3?

a)

1 mole

b)

2 moles

c)

3 moles

3.

How many grams are there in 2 moles of NH3?

a)

17 grams

b)

28 grams

c)

34 grams

d)

51 grams

4.

How many moles are there in 108 grams of H2O?

a)

7 moles

b)

6 moles

c)

5 moles

d)

4 moles

5.

What is the molar mass of Carbon?

a)

6

b)

14

c)

12.0

d)

4

6.

Fluorine is diatomic. What is the molar mass of Fluorine gas?

a)

19.0 g/mol

b)

9 g/mol

c)

38.0 g/mol

d)

18.0 g/mol

7.

What is the mass of one mole of water?

a)

33.0 g

b)

18.0 g

c)

17.0 g

d)

8.0 g

8.

What is the mass of 4.5moles of CH4?

a)

72.0 g

b)

68 g

c)

72.0 mol

d)

0.3 mol

9.

How many moles are in 150 grams of Na2SO4?

a)

142.1 g/mol

b)

1.1 mol

c)

21 315 g

d)

21 315 mol

10.
What is the mass of 0.75 moles of (NH4)3PO4?
a)
101.75 g
b)
121.75 g
c)
111.75 g
d)
131.75 g
11.
If I need 20.4 moles of sodium chloride, how much should I weigh out?
a)
0.549 g
b)
112 g
c)
1192 g
d)
5077 g
12.
Which is heaviest - a mole of copper or a mole of lithium?
a)
mole of copper
b)
mole of lithium
c)
they have the same mass
13.
A scientist shows you a 2.25-mol sample of carbon and a 2.25-mol sample of selenium.  Which of the following is true?
a)
they have the same mass
b)
they have the same volume
c)
they have the name number of atoms
d)
they have the same density
14.
How many atoms are there in 3.2 grams of sulfur?
a)
6.022 x 1023 atoms S
b)
6.022 x 1022 atoms S
c)
0.031 atoms S
d)
1.66 x 10-24 atoms S
15.
A weather balloon containing helium gas is 1000 grams. How many atoms of He are in the balloon?
a)
4 atoms
b)
250 atoms
c)
1.5 x 1026 atoms
16.

How many grams are in 1.204 x 1024 molecules of H2O? (molar mass = 18g/mol)

a)

36 g

b)

18 g

c)

9 g

d)

54 g

17.

How many molecules are in 36 grams of H2O? (molar mass = 18g/mol)

a)

1.204 x 1024 molecules

b)

1.806 x 1024 molecules

c)

9.01 x 1023 molecules

d)

6.02 x 1023 molecules

18.

How many atoms are in 128 grams of Cu? (molar mass = 64 g/mol)

a)

1.204 x 1024 molecules

b)

1.806 x 1024 molecules

c)

9.01 x 1023 molecules

d)

6.02 x 1023 molecules

19.

How many grams are in 3.01 x 1023 atoms of Kr? (molar mass = 84 g/mol)

a)

42 g

b)

84 g

c)

168 g

d)

200 g

20.
What can be determined from a balanced chemical equation?
a)
Mole ratio of any two substances in the reaction
b)
Energy released in the reaction.
c)
Electron configuration of all elements in the reaction. 
d)
Mechanism involved in the reaction. 
21.
N2 +  3H2 → 2NH3 
What is the mole ratio between Nitrogen and Ammonium 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 
22.
4NH3 + 5O2-->4NO + 6H2O
What is the total number of moles of H2O produced when 12 mole of NH3 is completely consumed?
a)
15
b)
18
c)
20
d)
24
23.
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
24.
3 Mg + 1 Fe2O3 → 3 MgO + 2 Fe
What is the Ratio of moles of Mg 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
25.
H2+Cl2-->2HCl
How many moles of Cl2 are needed to react with 3 moles of H2?
a)
5
b)
2
c)
3
d)
6
26.
2Na + S -->Na2S
What is the total number of moles of Na2S produced when 8.0 moles of Na were completely consumed?
a)
1
b)
2
c)
0.5
d)
4
27.
Mole ratios are obtained from the
a)
balanced chemical equation
b)
periodic table
c)
molar mass
28.
Which of the following represent a mole ratio between silver nitrate and copper(II) nitrate in the following reaction:
2AgNO3 + Cu --> Cu(NO3)2 + 2Ag
a)
2 mol AgNO3 / 2 mol Ag
b)
2 mol Ag / 2 mol AgNO3 
c)
2 mol AgNO3 / 2 mol Cu(NO3)2
d)
2 mol AgNO3 / 1 mol Cu(NO3)2
29.

Where are the numbers for a mole ratio found?

a)

They are part of the chemical formulas for the reactants / products.

b)

They are given in the problem.

c)

They are found on the periodic table for those elements.

d)

They are found as coefficients in the reaction's balanced chemical equation.

30.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

Ethane (C2H6) combusts in the above reaction. What is the mole ratio of ethane to oxygen gas?

a)
b)
c)
d)
31.

2 C2H6 + 7 O2 → 4 CO2 + 6 H2O

New problem: If 16 moles of carbon dioxide are formed by this reaction, how many moles of water were also produced?

a)

4 mol H2O

b)

6 mol H2O

c)

24 mol H2O

d)

96 mol H2O

e)

384 mol H2O

32.
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
33.
What is the mass of 0.89 mol of CaCl2?
a)
111 grams
b)
0.008 grams
c)
98.9 grams
d)
none of the choices
34.

What is the percent composition by mass of magnesium in the compound MgSO4

a)

20%

b)

27%

c)

46%

d)

53%

35.
What is the empirical formula if you have 88.80% copper and 11.20% oxygen?
a)
Cu3O8
b)
CuO4
c)
Cu2O
d)
Cu4O10
36.
What is the empirical formula for the following molecular formula: C6H14
a)
C6H14
b)
C3H7
c)
CH2
d)
CH3
37.
What is the molecular formula if the empirical formula is C2H5 and the molecular molar mass is 58.14 g/mol?
a)
C2H5
b)
C4H10
c)
C1H2.5
d)
C4H8
38.

A compound with the following composition has a molar mass of 60.10g/mol: 39.97% carbon; 13.41% hydrogen; 46.62% nitrogen. Find the molecular formula.

a)

C2H3N2

b)

CH2N

c)

CH4N

d)

C2H8N2

39.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
40.
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
41.
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
42.
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
43.
Find the percent composition of Cu2S?
a)
%Cu= 67.987 %S= 32.013
b)
%Cu= 79.854   %S= 20.145
c)
%Cu= 35.946   %S= 64.054
44.
How many molecules are in 2.5 mol of NaCl?
a)
1.51x1023
b)
146
c)
4.15
d)
1.51x1024
45.

Phosphorus combines with oxygen to form an oxide that reacts with water to produce phosphoric acid, which is an important industrial compound used to produce fertilizers. A balanced equation for the production of phosphoric acid is shown here:

P4O10(s) + 6H2O(L) → 4H3PO4(aq) + energy

Write the empirical formula of the solid reactant in the equation.



(a)  

46.

Phosphorus combines with oxygen to form an oxide that reacts with water to produce phosphoric acid, which is an important industrial compound used to produce fertilizers. A balanced equation for the production of phosphoric acid is shown here:

P4O10(s) + 6H2O(L) → 4H3PO4(aq) + energy

Show a numerical setup for calculating the percent composition by mass of phosphorus in P4O10 (formula mass is 283.89 u).

(a)  

47.

Given the balanced equation for the reaction of butane and oxygen:

2C4H10 + 13O2 → 8CO2 + 10H2O + energy

How many moles of carbon dioxide are produced when 5.0 moles of butane react completely?

a)

5.0 mol

b)

20.0 mol

c)

10.0 mol

d)

40.0 mol

48.

What is the percent composition by mass of nitrogen in the compound N2H4 (gram-formula mass 32 g/mol)?

a)

13%

b)

88%

c)

44%

d)

93%

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