Section 12.1
Counting Particles of Matter
Practice Test
1.
A direct measurement on a sample of pure substance can be converted to a count of the number of particles through ________________.
a.
geometry
b.
stoichiometry
c.
telemetry
d.
theory
Hint
2.
The number of things in one mole is the ________________.
a.
Avogadro constant
b.
gram
c.
atomic mass unit
d.
kilogram
Hint
3.
How many hydrogen atoms are in one mole of hydrogen molecules?
a.
12.04 × 10
23
b.
6.02 × 10
23
c.
2.02
d.
1.01
Hint
4.
What is the molar mass of arsenic?
a.
74.9 g/mol
b.
74.9 u/mol
c.
33 lb/mol
d.
33 kg/mol
Hint
5.
What is the molar mass of carbon dioxide?
a.
6.02 × 10
23
g/mol
b.
12.0 g/mol
c.
32.0 g/mol
d.
44.0 g/mol
Hint
6.
How many moles of sucrose, C
12
H
22
O
11
, are in 1222 g of sucrose?
a.
0.258
b.
1.22
c.
3.57
d.
10.8
Hint
7.
How many moles of calcium are in 0.544 g of calcium?
a.
0.0136
b.
0.0773
c.
0.554
d.
3.11
Hint
8.
What is the mass of 2.40 mol of copper?
a.
152 g
b.
26.5 kg
c.
3.78 mg
d.
5.65 g
Hint
9.
How many atoms are in 34.6 g of carbon?
a.
1.73 × 10
24
b.
12.1 × 10
23
c.
2.88
d.
0.00554
Hint
10.
Determine the number of atoms in 3.54 mol S.
a.
1.70 x 10 23
b.
1.70 x 10 24
c.
2.13 x 10 23
d.
2.13 x 10 24
Hint
11.
Calculate the mass in grams of 0.0790 moles of aluminum.
a.
1.0 g
b.
2.1 g
c.
21 g
d.
34 g
Hint
12.
How many moles of chlorine are in 100 g chlorine (Cl)?
a.
0.355
b.
2.82
c.
64.6
d.
100
Hint
13.
How many atoms of carbon are in a pure sample of carbon having a mass of 72.0 g?
a.
3.6 x 10 24
b.
36 x 10 24
c.
3.6 x 10 23
d.
4.33 x 10 25
Hint
14.
Calculate the number of moles of hydrogen atoms in 4.75 mol sulfuric acid.
a.
2.38 mol
b.
4.75 mol
c.
9.50 mol
d.
33.2 mol
Hint
