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Unit 6 Review

Total questions: 40

Worksheet time: 10hrs 0mins

Name
Class
Date
1.

The number 6.022 x 1023 is called...

a)

A dozen

b)

Bohr's number

c)

Buckley's number

d)

Avogadro's number

2.

Which has more molecules?

a)

1 mole H2O

b)

1 mole CH4

c)

1 mole Cl2

d)

They're are all the same.

3.

One mole of sulfur (S) is equal to home many atoms?

a)

32 atoms

b)

16 atoms

c)

1.20 x 1023 atoms

d)

6.022 x 1023 atoms

4.

To convert from moles to particles, you should multiply by ....

a)
b)
c)
d)
5.

To convert from particles to moles, you should multiply by ....

a)
b)
c)
d)
6.

5.11 x 1023 atoms of lithium (Li) is equal to how many moles?

a)

1.18 moles

b)

0.351 moles

c)

1.34 moles

d)

0.849 moles

7.

0.75 mole of copper (Cu) is equal to how many atoms?

a)

8.03 x 1023 atoms

b)

6.02 x 1023 atoms

c)

4.51 x 1023 atoms

d)

3.11 x 1023 atoms

8.

What is the mass of one mole of potassium (K)?

a)

19 grams

b)

39.10 grams

c)

30.97 grams

d)

38 grams

9.

To convert from moles to grams, you should multiply by ....

a)
b)
c)
d)
10.

To convert from grams to moles, you should multiply by ....

a)
b)
c)
d)
11.

Which conversion factor would you use to calculate correctly the mass of 2 moles of the element titanium?

a)

47.86 g Ti / 1 mol Ti

b)

1 mol Ti / 47.84 g Ti

c)

47.84 mol / 1 g Ti

d)

47.87 g Ti / 1 mol Ti

12.

0.50 moles of carbon (C) is equal to how many grams?

a)

6.0 grams

b)

12.0 grams

c)

8.0 grams

d)

14.0 grams

13.

36.0 g of beryllium (Be) contains how many moles?

a)

0.25 mol

b)

4.0 mol

c)

45 mol

d)

320 mol

14.

How many atoms would be contained in 454 grams of iron (Fe)?

a)

6.02 x 1023 atoms

b)

8.14 atoms

c)

4.90 x 1024 atoms

d)

55.85 x 1023 atoms

15.

Find the mass in grams of 2.25 x 1024 atoms of calcium (Ca).

a)

40.0 grams

b)

255.1 grams

c)

150 grams

d)

9.02 x 1024 grams

16.

What is the molar mass of AuCl3?

a)

96.00 g/mol

b)

130.00 g/mol

c)

232.51 g/mol

d)

303.32 g/mol

17.

What is the molar mass of (NH4)3PO4

a)

113.02 g/mol

b)

124.13 g/mol

c)

149.12 g/mol

d)

137.00 g/mol

18.

What is the mass of 2.50 mol of oxygen gas (O2)?

a)

40.0 g

b)

80.0 g

c)

16.0 g

d)

32.0 g

19.

What is the mass of 6.25 mol of Cu(NO3)2?

a)

126 g

b)

785 g

c)

625 g

d)

1172 g

20.

If I have 6.02 x 1023 molecules of CO2, what is the mass?

a)

44.0 g

b)

2.65 x1023 g

c)

1.37 x1022 g

d)

96.0 g

21.
What is the percent by mass of oxygen in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
22.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
23.
What is the percent by mass of sodium in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
24.
What is the percent by mass of chlorine in NaCl?
a)
39%
b)
61%
c)
35%
d)
65%
25.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
26.
What is the percent by mass of calcium in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
27.
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%
28.
What is the percent composition by mass of magnesium in the compound MgSO4 (gram formula mass = 120 g/mol)?
a)
20%
b)
27%
c)
46%
d)
53%
29.

Which element in the compound potassium cyanide, KCN, has a percent composition of 60.97%?

a)

K

b)

C

c)

N

d)

None of the above

30.

A compound containing 92.3 percent carbon and 7.7 percent hydrogen. What is the empirical formula?

a)

CH

b)

CH2

c)

C2H

d)

C2H2

31.

What is the empirical formula for a compound which contains 67.1% zinc and the rest is oxygen?

a)

ZnO

b)

ZnO2

c)

Zn2O4

d)

Zn2O

32.

A compound contains 18.8% Na, 29.0% Cl, and 52.5% O by mass. Determine the empirical formula.

a)

NaClO

b)

NaClO4

c)

Na2Cl2O8

d)

NaCl2O4

33.

Compound contains 42.05 g of nitrogen and 95.95 g of oxygen. What is the formula?

a)

NO

b)

NO2

c)

N2O

d)

N2O4

34.
Which pair has the same empirical formula?
a)
NaCrO4 and Na2Cr2O7
b)
C2H4O2 and C6H12O6
c)
C3H6O3 and C2H6O2
d)
CH4 and C2H6
35.
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
36.
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 
37.
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
38.

How many grams are in 1.2 x 1024 atoms of C?

a)

29.34 grams

b)

23.94 grams

c)

6.02 grams

d)

1.21 grams

39.
Calculate the number of atoms in 0.0340 g Zn.
a)
5.200 x 10-4 atoms Zn
b)
3.130 x 1023 atoms Zn
c)
3.130 x 1020 atoms Zn
d)
1 atom Zn
40.
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

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