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WorksheetsMolar Mass, Mole High School Honors
Total questions: 51
Worksheet time: 3hrs 36mins
Name
Class
Date
1.
What are the units for molar mass?
a)
grams
b)
amu
c)
grams/mole
d)
liters
2.
How many grams are in 3.3 mol of Potassium Sulfide?
a)
360 g
b)
454 g
c)
238 g
d)
132 g
3.
Which compound has the smallest molar mass?
a)
CO
b)
CO2
c)
H2O
d)
H2O2
4.
Avogadro's number of representative particles is equal to one_____.
a)
kilogram
b)
gram
c)
kelvin
d)
mole
5.
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
6.
Determine the amount of moles in 1.50 x 1023 atoms of fluorine.
a)
9.03 x 1046 moles
b)
0.249 moles
c)
4.73 moles
d)
0.0131 moles
7.
How many moles of H atoms are there in 0.5 mol of H2SO4 ?
a)
0.25
b)
0.5
c)
0.75
d)
1
8.
Determine the molar mass for CCl4
a)
154 g/mol
b)
142 g/mol
c)
190 g/mol
d)
82.9 g/mol
9.
Oxygen is diatomic. What is the molar mass of oxygen gas?
a)
16 g/mol
b)
32 g/mol
c)
8 g/mol
d)
18 g/mol
10.
Determine the number of atoms in 1.50 g of carbon.
a)
0.125 atoms
b)
7.52 x 1022 atoms
c)
1.08 x 1025 atoms
d)
2.07 x 10-25 atoms
11.
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
12.
What is the molar mass of B2(CO3)3?
a)
81.6 g/mol
b)
94.8 g/mol
c)
38.8 g/mol
d)
201.6 g/mol
13.
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)
5.00 moles
14.
How many grams are there is 1.35 x 1025 atoms of K2SO4?
a)
3,909 g K2SO4
b)
174.1g K2SO4
c)
3.53 x 1021 g K2SO4
d)
423 g K2SO4
15.
How many water molecules are in 5.2 moles of water?
a)
6.02 x 1023
b)
5.2
c)
3.1304 x 1024
d)
8.638 x 10-24
16.
What is the difference between a formula unit and a molecule?
a)
formula unit - ionic bond
molecule - covalent bond
molecule - covalent bond
b)
formula unit - big
molecule - small
molecule - small
c)
formula unit - covalent bond
molecule - ionic bond
molecule - ionic bond
d)
formula unit - small
molecule - big
molecule - big
17.
What is the percentage of chromium in potassium dichromate? (dichromate is Cr2O72-)
a)
40.77%
b)
27.24%
c)
35.35%
d)
100%
18.
Find the percentage composition of Mg in Mg3(PO4)2.
a)
27.74% Mg
b)
23.57% Mg
c)
48.68% Mg
d)
13.45% Mg
19.
How many grams are in 1.2x1024 molecules of carbon monoxide?
a)
28 grams
b)
56 grams
c)
6.02 grams
d)
1.2 grams
20.
Which conversion factor should be used to solve the following, "How many moles of argon atoms are present in 11.2 L of argon gas at STP?"
a)
1 mol = 22.4 L
b)
1 mol = 39.95 g
c)
1 mol = 6.02x1023 atoms
d)
More than 1
21.
A formula with the lowest whole # ratio of elements in a compound is called
a)
empirical formula
b)
chemical formula
c)
covalent formula
d)
molecular formula
22.
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
23.
All of the following are empirical formulas EXCEPT
a)
C3H8
b)
Na2SO4
c)
N2O4
d)
Al3(SO4)2
24.
Which of the following is the correct empirical formula for C4H10
a)
C2H5
b)
CH2.5
c)
C8H20
d)
C4H10
25.
A compound is 25.9 % nitrogen and 74.1% oxygen. Find its empirical formula.
a)
N2O4
b)
NO
c)
N2O5
d)
N4O6
26.
The empirical formula of a substance is CH2O. Its molar mass is 180.0. What is the molecular formula?
a)
C6H12O6
b)
C4H8O4
c)
C8H16O8
d)
C2H4O2
27.
Epinephrine (adrenaline) is a hormone secreted into the bloodstream in times of stress. It contains 59.00% C, 6.62% H, 26.20% O, 7.65%N and has a molar mass of 183 g/mol. What is its molecular formula?
a)
C9H12NO3
b)
C5H11N3O2
c)
C8H12NO2
d)
C7H9N2O
28.
Is the empirical formula of a substance ever the same as the molecular formula for a substance?
a)
Always
b)
Sometimes
c)
Never
29.
1) How many moles of gas are in 7.6 liters of Krypton gas?
a)
a. 2.9 mol
b)
b. 0.32 mol
c)
c. 3.2 mol
d)
d. 0.34 mol
30.
1) How many molecules are in 1.5 moles of F2?
a)
a. 9.03 molecules
b)
b. 57 molecules
c)
c. 2.5x10-24 molecules
d)
d. 9.03x1023 molecules
31.
Standard temperature and pressure (STP) is defined as
a)
O .C and 1.0 atm pressure
b)
0.C and 273 mmHg pressure
c)
0K and 1.0 atm pressure
d)
0K and 760 mmHg pressure
32.
What is the volume of 5 moles of oxygen gas at STP?
a)
112 L
b)
22.4 L
c)
78.8 L
d)
114.24 L
33.
How many moles are in a 18 L tank of nitrogen gas at STP?
a)
0.9 moles
b)
1 mole
c)
0.8 moles
d)
0.75 moles
34.
A container with a volume of 893 L contains how many moles of air at STP?
a)
20003.2 L
b)
39.9 L
c)
22.4 L
d)
none of the choices
35.
Hydrogen gas that occupies 35 L has a mass of what?
a)
1.6 g
b)
2.3 g
c)
3.1 g
d)
5.2 g
36.
equal volumes of gases at the same temperature and presssure contain equal numbers of particles
a)
percent composition
b)
empirical formula
c)
molar mass
d)
Avogadro's Hypothesis
37.
How many oxygen atoms are in 10 formula units of Fe2(SO4)3?
a)
4
b)
3
c)
7
d)
12
38.
The mass of a mole of H2O is its:
a)
molar mass
b)
empirical formula
c)
atomic mass
d)
molar density
39.
6.02 ´ 1023 representative particles of a substance
a)
Avogadro's Number
b)
Avogadro's Hypothesis
c)
molar mass
d)
atomic mass
40.
Which of the following is not an empirical formula?
a)
H2O
b)
H2O2
c)
OH-
d)
NaCl
41.
Which expression represents the percent by mass of H in H2O?
a)
(1g/18g)x100
b)
(2g/18g)x100
c)
(16g/18g)x100
d)
(18g/2g)x100
42.
What is the mass, in grams, of 1023 atoms of H?
a)
0.166g
b)
6.02g
c)
0.332g
d)
1.00795g
43.
How many atoms are in 0.5 moles of H?
a)
3.01 x 1023
b)
6.02 x 1023
c)
12.04 x 1023
d)
none of these
44.
Determine the molar mass of a gas that has a density of 0.5g/L at STP. Remember 22.4L/mol.
a)
11.2L
b)
22.4L
c)
44.8L
d)
none of these
45.
What is the molecular formula of the a compound with an empirical formula of CH2 and a molar mass of 30g/mol?
a)
C2H4
b)
CH2
c)
CH3
d)
C2H
46.
How many liters are in 19.82 g Mg(OH)2?
a)
10.75 liters
b)
10.7 liters
c)
7.615 liters
d)
7.62 liters
47.
Which is the formula for a compound that contains 28.0 nitrogen and 80.0g oxygen
a)
NO2
b)
NO
c)
N2O5
d)
N2O
48.
What is the number of moles in 9.63 L of H2S gas at STP?
a)
.104 mol
b)
.430 mol
c)
3.54 mol
d)
14.7 mol
49.
How many molecules are in 32.4 grams of phosphorous pentoxide?
a)
1.76 x 1023 molecules
b)
0.29 moles
c)
1.76 x 1022 molecules
d)
0.29 molecules
50.
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
51.
What is the empirical formula for the following molecular formula: C6H14
a)
C6H14
b)
C3H7
c)
CH2
d)
CH3
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