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Chapter 11 Test Review

Total questions: 43

Worksheet time: 2hrs 10mins

Name
Class
Date
1.
What is the molar mass of PbSO4
a)
303.3 g/mol
b)
294.7g/mol
c)
163.8g/mol
d)
372g/mol
2.
What is the molar mass of NaBr
a)
381.9g/mol
b)
102.9 g/mol
c)
213.6g/mol
d)
93.0g/mol
3.
What is the molar mass of Ca(OH)2
a)
74.1 g/mol
b)
210.0g/mol
c)
98.9g/mol
d)
219.9g/mol
4.
What is the percent by mass of magnesium in MgO?
a)
20%
b)
40%
c)
50%
d)
60%
5.

What is the percent by mass of calcium in CaF2

a)
24%
b)
49%
c)
51%
d)
65%
6.
What is the percent by mass of fluorine in CaF2 (gram-formula mass = 78 g/mol)?
a)
24%
b)
49%
c)
51%
d)
65%
7.

What are the units for atomic mass?

a)

grams

b)

amu

c)

molecules

d)

grams/mole

8.

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

9.

How many moles are in 450.0g Potassium chloride (KCl)?

a)

6.0 g

b)

6.0 mol

c)

74.6 g/mol

d)

33.570 mol

10.

How many mole are there in 51 grams of NH3?

a)

1 mole

b)

2 moles

c)

3 moles

11.

How many grams are there in 2.0 moles of CH4

a)

12 grams

b)

16 grams

c)

24 grams

d)

32 grams

12.

The number 6.02 x 1023 is called...(definition for mole)

a)

Obama's number

b)

Bohr's number

c)

Trump's number

d)

Avogadro's number

13.

How can you figure out how many particles there are in 2 moles?

a)
2
b)
2 x (6.02 x 1023)
c)
2 x (atomic mass)
d)
2 ÷ (6.02 x 1023)
14.

How many moles are 2.85 x 1018 atoms of iron?

a)

4.73 x 10-6 moles

b)

1.72 x 1042 moles

c)

4.73 x 106 moles

d)

1.72 x 10-6 moles

15.

5.11x1023 atoms of lithium is equal to how many moles?

(to find moles, you must divide atoms by Avogadro's number)

a)

1.18

b)

0.351

c)

1.34

d)

0.849

16.

How many atoms of iodine are in a mole of iodine?

a)

53

b)

63.55g

c)

126.9

d)

6.02 x 1023

17.

What is the representative particle for NaCl?

a)

formula units

b)

atoms

c)

molecules

d)

ions

18.

What is the representative particle for H2?

a)

formula units

b)

atoms

c)

molecules

d)

ions

19.

What is the representative particle for H2O?

a)

formula units

b)

atoms

c)

molecules

d)

ions

20.

What is the representative particle for CO32-?

a)

formula units

b)

atoms

c)

molecules

d)

ions

21.

What is the representative particle for C?

a)

formula units

b)

atoms

c)

molecules

d)

ions

22.

What is the representative particle for potassium nitrate?

a)

formula units

b)

atoms

c)

molecules

d)

ions

23.
What is the following Br2
a)
Atom
b)
Molecule
c)
Formula Unit
24.

What is the molar mass of one mole of HCl?

a)

79.92 grams per mole of HCl

b)

36.46 grams per mole of HCl

c)

35.45 grams per mole of HCl

d)

1.01 grams per mole of HCl

25.

Which of the following has more molecules or formula units?

a)
1 mole H2O
b)
1 mole Al(OH)3
c)
1 mole NaCl
d)
There are all the same
26.
How many moles are in 15 grams of lithium?
a)
0.5 moles
b)
104.1 moles
c)
2.2 moles
d)
50 moles
27.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
28.
How many moles are in 3.01 x 1022 atoms of magnesium?
a)
0.050 moles
b)
1.81 x 1046 moles
c)
5.00 x 1021 moles
d)
5.00 moles
29.
How many grams are in 1.2 x 1024 atoms of C?
a)
28 grams
b)
24 grams
c)
6.02 grams
d)
1.2 grams
30.
Which of the following dimensional analysis setups will correctly convert 27.76g of Li to atoms of Li?
a)
A
b)
B
c)
C
d)
D
31.
What is the empirical formula if you have 36.84% nitrogen and 63.16% oxygen?
a)
NO
b)
N2O3
c)
N2O4
d)
N2O5
32.
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.
33.

When calculating empirical or molecular formula, what do you do when you get a half in the ratio?

a)
add 2 to each element
add two to only the one with the half
b)
multiply the one with the half only by two
c)
multiply all of them by two
d)
add two to all of the ratios
34.
What is the empirical formula of the following molecular formula:  C3H6
a)
C3H6
b)
CH2
c)
C2H4
d)
CH3
35.
Which one is empirical?
a)
H2O2
b)
C2H6O12
c)
CaCl2
d)
N2O8
36.
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
37.

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 empirical and molecular formula.

a)

CHN, CH2N4

b)

CH4N, C2H4N

c)

CH4N, C2H8N2

d)

none of the above are correct

38.
Name the following ionic compound: MgSO4*7H2O
a)
magnesium sulfate * hexahydarte
b)
magnesium sulfate hexahydarte
c)
magnesium sulfate heptahydrate
d)
magnesium sulfate* heptahydrate
39.
Na2CO3 · 10H2O is known as sodium sulfate ______
a)
Hydroxide
b)
Hydrate
c)
Decahydrate
d)
None of the above
40.
A 15.67 g sample of a hydrate of magnesium carbonate was heated to drive off the water. The mass was reduced to 7.58 g. What is the formula of the hydrate?
a)
MgCO3 · 5H2O
b)
MgCO3 · 4H2O
c)
MgCO3 · 6H2O
d)
MgCO3 · 1H2O
41.

A 4.175 gram sample of a certain hydrate of copper (II) sulfate, CuSO4•xH2O, is heated until all the water is driven off. The resulting anhydrous compound weighs 3.120 grams. What is the formula of the hydrate?

a)

CuSO4•H2O

b)

CuSO4•3H2O

c)

CuSO4•6H2O

d)

CuSO4•4H2O

42.

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%

d)

Cu= 39.925%; S= 20.151%

43.

A sample with a molar mass of 34.00 g/mol is found to consist of 0.44 g H and 6.92 g O. Find its molecular formula.

a)

HO

b)

H2O2

c)

H2O

d)

H1/2O1/2

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