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Mole Conversions, % Composition, & Emp/Molec Formulas

Total questions: 24

Worksheet time: 2hrs 0mins

Name
Class
Date
1.
How many molecules of sugar (C6H12O6) are in a mole?
a)
24 molecules
b)
180 molecules
c)
180 g
d)
6.02 x 1023 molecules
2.
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
3.
How many steps are in a gram to mole conversion?
a)
1
b)
2
c)
3
d)
4
4.
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
5.
If an atom of Fluorine has an atomic mass of 19 amu, it has a Molar mass of ____
a)
19 lbs.
b)
19 kg
c)
How am I supposed to know?
d)
19 g/mol
6.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
7.
What is the molar mass of table salt (NaCl)?
a)
116.886 g/mol
b)
35.453 g/mol
c)
22.990 g/mol
d)
58.443 g/mol
8.
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
9.
How many steps are in a gram to molecule conversion?
a)
1
b)
2
c)
3
d)
4
10.

(0901) Avogadro’s number is:

a)

6.02 x 1022

b)

6

c)

6.02 x 1023

d)

3.01 x 1023

11.

(0901) How many water molecules are in 5.2 moles of water?

a)

6.0 x 1023 molecules

b)

5.2 molecules

c)

3.1 x 1024 molecules

d)

8.6 x 10-24 molecules

12.

(0901) Determine the number of moles in 5.2 x 1022 atoms of gold.

a)

0.086 mole

b)

0.52 mole

c)

8.63 x 1044 moles

d)

3.1 x 1046 moles

13.

(0901) How many moles of methane (CH4) are in 1.24 x 1023 molecules of methane?

a)

6.02 x 1023 moles

b)

7.46 x 1046 moles

c)

978 moles

d)

0.206 moles

14.

(0902) The mass of one mole of substance is called...

a)

molecular mass

b)

mole constant

c)

molar mass

d)

atomic weight

15.

(0902) What is the molar mass of Ca(NO3)2?

a)

148.096 g

b)

164.086 g

c)

102.055 g

d)

70.084 g

16.

(0903) How many moles are in 74 g of KCl

a)

0.99 mole

b)

0.014 mole

c)

11 moles

d)

0.14 mole

17.

(0903) Determine how many grams are in 0.36 moles of CCl4.

a)

150 g

b)

55 g

c)

0.0023 g

d)

2.2 g

18.
Fill in the blank....
Percent to Mass, Mass to Mole, ____________, Multiply till whole. 
a)
Multiply by Small
b)
Divide by Small
c)
Divide till Whole
d)
Divide by the number off the PT
19.
What is the equation for calculating percent composition?
a)
mass of element/mass of compound = x 100
b)
mass of compound/mass of element = x 100 
c)
total mass/molar mass = x 100 
d)
molar mass/molar mass = x 100 
20.

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

a)

20%

b)

27%

c)

46%

d)

53%

21.
What is the empirical formula if you have 88.80% copper and 11.20% oxygen?
a)
Cu3O8
b)
CuO4
c)
Cu2O
d)
Cu4O10
22.
What is the empirical formula for the following molecular formula: C6H14
a)
C6H14
b)
C3H7
c)
CH2
d)
CH3
23.
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
24.

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