David Healy 2010
Unit Conversion and Dimensional Analysis
Frequently in Chemistry you will be provided with data describing a particular quantity in a
certain unit of measurement, and you will be required to convert it to a different unit which
measures the same quantity. This process is frequently described as Unit Conversion. As an
example, you may be given a measurement of length in centimeters which must be converted to
meters. This worksheet includes the rules and some guidelines to help you with converting,
density problems, stoichiometry problems, and concentration problems. This worksheet is not
intended to help you with reading comprehension of word problems regarding these types of
questions, just the mathematical application.
Rules
1.) Identify the given measurement.
2.) Identify the unit that the measurement must be converted to.
3.) Use conversion factors (relationship between two units) that link your given unit to your
final unit.
4.) Perform the mathematical calculations.
5.) Do not forget to apply significant figures to your final answer.
Guidelines
1.) When converting a single unit, such as converting from centimeters to meters, the given
should also be a single unit as well. It can become more difficult by starting with the
conversion factor: (100 cm / 1 m). Even if you know a dozen = 12, the relationship
cannot be applied if you do not know how many dozen you care about.
2.) When only a single unit given, it should be written over 1. For example, 56.93 cm should
be written as 56.93 cm / 1. Units lacking a number are assumed to be 1. If we were given
1.193 g / ml, we would write this as 1.193 g / 1 ml .
3.) Any relationship between two units can potentially be utilized as a conversion factor:
density relates mass and volume while molar mass relates moles and mass. Express these
conversion factors as a fraction in the dimensional analysis.
4.) A conversion factor can be written in two different ways. For example, converting
centimeters and meters, we can use the conversion factor (100 cm / 1 m) or (1 m / 100
cm). The unit you want to remove from the problem should be placed opposite of the
original. So, to convert from cm to m, cm is your given unit, and the cm should be in the
bottom to denominator out cm from the problem.
David Healy 2010
5.) The math should be the last thing you do. By first cancelling units, so that your final unit
is the only one, you may easily check that the conversion has been set up correctly. The
math calculation will follow this.
6.) Standardized conversion factors are never used to calculate significant figures.
Multiplying by the conversion factor (100 cm / 1 m) will not affect your significant
digits.
Example
Problem: Convert: 56.93 cm to m
Solution:
1.) The given measurement is 56.93 cm.
2.) The measurement must be converted to meters.
3.) The conversion factor(s) we need to use either has to directly relate cm and m, or chain to
cancel all units except m. Luckily, we know a direct one: 100 cm is equal to 1 m. cm
should be in the denominator to cancel with the original cm.
4.) 56.93 cm m 56.93 m
------------ X --------- = ---------- = .5693 m (significant figures applied)
1 100 cm 100
Practice Problems
Note: Unless you are confident in your ability to determine direct conversion factors, such as
cm to km, it is highly recommended to convert to the standard unit. This allows one to relate
cm to m, and then m to km.
1.
87.68 kg to g
11.
5055 mm to m
21.
2133 mL to L
31.
2.
543.7 dm to m
12.
222.9 dg to g
22.
80.66 L to dL
32.
3.
2417 m to mm
13.
794.2 km to m
23.
874.2 m to dm
33.
4.
8506 cg to g
14.
4.807 kL to L
24.
557.2 g to cg
34.
5.
3841 cL to L
15.
38.92 mg to g
25.
87.66 m to km
35.
6.
218.1 km to m
16.
89.55 m to cm
26.
20.01 L to dL
36.
7.
772.8 g to kg
17.
3.889 mL to L
27.
7022 dg to g
37.
8.
15.47 kL to L
18.
4.102 g to mg
28.
9.319 L to cL
38.
9.
67.42 dL to L
19.
6841 mL to L
29.
5.604 g to dg
39.
10.
.85 m to mm
20.
39.24 cm to m
30.
19.5 g to mg
40.
David Healy 2010
Practice Problems: Answers
1.
87680 g
11.
5.055 m
21.
2.133 L
31.
8.177 x 10
-5
kg
2.
5437. m
12.
22.29 g
22.
806.6 dL
32.
4.116 x 10
6
mm
3.
2417000 mm
13.
794200 m
23.
8742. dm
33.
6.908 x 10
-4
kL
4.
85.06 g
14.
4807 L
24.
55720 cg
34.
9.493 x 10
5
dg
5.
38.41 L
15.
0.03892 g
25.
0.08766 km
35.
2.525 x 10
-6
kg
6.
218100 m
16.
8955 cm
26.
200.1 dL
36.
1.782 x 10
7
cL
7.
0.7728 kg
17.
0.003889 L
27.
702.2 g
37.
5.359 x 10
2
mg
8.
15470 L
18.
4102 mg
28.
931.9 cL
38.
4.582 x 10
4
mL
9.
6.742 L
19.
6.841 L
29.
56.04 dg
39.
9.876 x 10
-3
km
10.
850 mm
20.
0.3924 m
30.
0.0195 mg
40.
1.511 x 10
7
dm
Density Example
Problem: Calculate the mass in grams of 14.79 ml of a substance. Its density is 1.193 g/ml.
Solution:
1.) The given measurement is 14.79 ml.
2.) It must be converted to grams.
3.) The conversion factor has to relate mass and volume. Luckily, density is supplied, and its
units are g/ml, a mass and volume unit. The number 1.193 belongs to the gram unit, and
is placed on the top so that the ml units can cancel out.
4.) 14.79 ml 1.193 g 17.64 g
----------- X --------- = --------- = 17.64 g (significant figures applied)
1 ml 1
David Healy 2010
Density Practice Problems
1.
17. g to mL, density = 3.291 g / mL
21.
854.8 cg to cL, density = 20.15 g / mL
2.
96.92 g to mL, density = 0.243 g / mL
22.
5214.000 L to kg, 4.818 g / mL
3.
62.59 mL to g, density = .5074 g / mL
23.
96.02 dL to mg, density = 7.27 g / mL
4.
4409. mL to g, density = .8449 g / mL
24.
.796 kL to dg, density = 0.9237 g / mL
5.
4155. g to mL, density = 1.291 g / mL
25.
80.03 kg to kL, density = 26.73 g / mL
6.
3.38 mL to g, density = 1.411 g / mL
26.
4.946 dL to mg, density = 7.4352 g / mL
7.
92.86 g to mL, density = 10.71 g / mL
27.
519.0 cL to dg, density = 0.8437 g / mL
8.
921.5 g to mL, density = 38.35 g / mL
28.
8830.0 mg to L, density = 4.848 g / mL
9.
53.08 mL to g, density = 60.83 g / mL
29.
76.09 dL to cg, density = 1.185 g / mL
10.
7.85 mL to g, density = 2.643 g / mL
30.
855.5 kL to kg, density = 0.695 g / mL
11.
3.23 kg to mL, density = 0.4059 g / mL
31.
980.3 dg to kL, density = 1.679 kg / L
12.
6.247 g to kL, density = 1.066 g / mL
32.
6.433 L to mg, density = 7.685 cg / dL
13.
3858. mg to mL, density = 1.492 g / mL
33.
701.4 dg to mL, density = 4.494 mg / cL
14.
5.567 mL to dg, density = 0.7086 g / mL
34.
7612.00 L to kg, density = 39.3 dg / dL
15.
9632.00 g to cL, density = 1.8020 g / mL
35.
5.423 mg to cL, density = 0.8178 Kg / dL
16.
607.3 dL to g, density = 1.2 g / mL
36.
79.72 cg to dL, density = 0.9770 dg / L
17.
3.019 cg to mL, density = 1.306 g / mL
37.
3298. cL to mg, density = 1.613 cg / mL
18.
7143.0 L to g, density = 0.438 g / mL
38.
95.57 kL to g, density = 3.445 cg / cL
19.
329.1 mg to mL, density = 2.522 g / mL
39.
8738 kg to mL, density = 0.5409 cg / kL
20.
63.47 g to L, density = 41.939 g / mL
40.
843.10 mL to kg, density = 0.7166 g / dL
Density Practice Problems: Answers
1.
5.2 mL
11.
7960 mL
21.
0.04242 cL
31.
0.00005839 kL
2.
399. mL
12.
5.860 x 10
-6
kL
22.
25120 kg
32.
4944. mg
3.
31.76 g
13.
2.586 mL
23.
698000 mg
33.
156100 mL
4.
3725. g
14.
0.3945 dg
24.
7350000 dg
34.
300. kg
5.
3218. mL
15.
534.52 cL
25.
0.002994 kL
35.
0.00006631 cL
6.
4.77 g
16.
73000 g
26.
3677000 mg
36.
81.60 dL
7.
8.670 mL
17.
0.02312 mL
27.
43790 dg
37.
5.320 x 10^5 mg
8.
24.03 mL
18.
3129000 g
28.
0.001821 L
38.
329200 g
9.
3229. g
19.
0.1305 mL
29.
901700 cg
39.
1.615 x 10^15 mL
10.
20.7 g
20.
0.001513 L
30.
595000 kg
40.
0.006042 kg
David Healy 2010
Molecule / Mole Stoichiometry Example
Problem: Based on the balanced chemical equation: C + O
2
→ CO
2
, how many
molecules of carbon dioxide could be produced from 20 atoms of carbon in the presence of
excess oxygen?
Solution:
1.) The given measurement is the 20 carbon atoms.
2.) This must be converted to molecules of carbon dioxide.
3.) The conversion factor has to relate carbon atoms and carbon dioxide molecules. Luckily,
one can use a balanced chemical equation, such as the one above, to determine a
conversion factor between the two different substances. The ratio is 1 C : 1 CO
2
, and the
carbon be in the denominator of the fraction to cancel the given carbon unit.
4.) 20 C 1 CO
2
20 CO
2
------ X -------- = --------- = 20 CO
2
molecules (significant figures applied)
1 1 C 1
David Healy 2010
Molecule / Mole Stoichiometry Practice Problems
Note: Be specific when writing conversion factors representing chemicals. You should include
not only the unit of measure, but also the identity of the chemical itself.
Note: When taking two reactants to see how much product they can produce, it is necessary to
check for the limiting reagent, the one you have less of after converting to moles and accounting
for the ratio in which it reacts.
2 N
2
O
5
→ 2 N
2
+ 5 O
2
1.
How many molecules of nitrogen gas are produced from a reaction yielding 225 molecules
of oxygen gas?
2.
How many molecules of dinitrogen pentoxide are required to produce 164 molecules of
nitrogen gas for your gas molecule collection?
3.
When 40 molecules of oxygen gas are produced, how many molecules of nitrogen gas
byproduct are produced?
4.
How many molecules of dinitrogen pentoxide are consumed in the formation of 1,870
molecules of oxygen gas?
5.
How many molecules of nitrogen gas and oxygen gas are produced in the decomposition of
643 molecules of dinitrogen pentoxide?
C
5
H
12
+ 8 O
2
→ 5 CO
2
+ 6 H
2
O
6.
From a reaction that produced 2,238 molecules of water vapor, how many carbon dioxide
molecules would you expect to be formed?
7.
Your dragon sneezes and ignites 187 molecules of pentane, how many molecules of water
vapor are produced?
8.
From the production of 170 molecules of carbon dioxide, how much oxygen gas was
required for this reaction?
9.
How much oxygen is required for the combustion of 6,914 molecules of pentane?
10.
How many molecules of carbon dioxide and water vapor were produced in question 9?
2 C
8
H
18
+ 25 O
2
→ 16 CO
2
+ 18 H
2
O
11.
From the reaction of 147.2 moles of octane with all needed oxygen, how many moles water
vapor are produced as a result?
12.
Your experiment yields 4.283 moles of carbon dioxide, how many moles water vapor are
produced as a byproduct?
13.
With excess octane, 42.05 moles of oxygen gas reacts, generating how many moles of
carbon dioxide?
14.
You want to produce 97.48 moles of carbon dioxide as a gift to your chemistry professor,
how many moles of octane should you start with?
15.
With 200. moles of octane and 164.71 moles of oxygen gas in your reaction mixture, how
many moles of carbon dioxide and water vapor can be produced?
David Healy 2010
2 Fe(NO
3
)
3
+ 3 MgO → Fe
2
O
3
+ 3 Mg(NO
3
)
2
16.
In order to obtain 132.843 moles of magnesium nitrate, how many moles of magnesium
oxide must be reacted?
17.
After a reaction runs to completion, you obtain 27.13 moles of magnesium nitrate. How
many moles of iron(III)nitrate were consumed?
18.
Determine how many moles iron(III)nitrate are required to synthesize 421.0 moles of
iron(III)oxide.
19.
You react 7.23 moles of iron(III)nitrate and 11.48 moles of magnesium oxide in the
magnesium nitrate lab you set up in your bathroom, producing how many moles of
iron(III)oxide waste?
20.
How many moles of magnesium nitrate product was formed in problem 19?
4 (NH
4
)
3
N + 3 Cr(CrO
4
)
2
→ 6 (NH
4
)
2
CrO
4
+ Cr
3
N
4
21.
What mass of ammonium chromate is produced in the complete reaction of 8.1934 moles
of ammonium nitrate?
22.
94.18 grams of chromium(IV)nitrate are collected after your experiment. How many moles
of chromium(IV)chromate reacted to produce this mass?
23.
1.0 gram of chromium(IV)chromate is reacted with excess ammonium nitrate to produce
how many moles of ammonium chromate?
24.
In an effort to resurrect your first dead pet, the Necronomicon requires 666 moles of
chromium(IV)nitrate. How many grams of each reactant are required for Fluffy to be
reborn?
25.
Determine the moles of ammonium chromate generated in the reaction of 1407 grams of
ammonium nitrate and 153.8 grams of chromium(IV)chromate.
Cu
3
(PO
4
)
2
+ 3 Na
2
SO
4
→ 2 Na
3
PO
4
+ 3 CuSO
4
26.
What mass of sodium phosphate and copper(II)sulfate is produced from the reaction of
47.002 moles of sodium sulfate?
27.
You wish to produce 131.9 grams of copper(II)sulfate. To do so, you require how many
moles of copper(II)phosphate?
28.
When 80 moles of sodium sulfate are reacted, what mass of copper(II) sulfate is produced?
29.
The lab procedure requires 45.61 grams of copper(II)phosphate and 94.65 grams of sodium
sulfate. How many moles of sodium phosphate are produced?
30.
A mole would like to make a statue of his wife out of exactly 1.00 mole of sodium
phosphate. He knows I’m good for the sodium sulfate but needs you to provide what mass
of copper(II)phosphate for the reaction?
David Healy 2010
AlCl
3
+ 3 H
2
O → Al(OH)
3
+ 3 HCl
31.
You accidently add an unknown mass of aluminum chloride into your reaction mixture
containing 47.0 grams of water. On completion, your reaction mixture yields 47.00 grams
of aluminum hydroxide. Determine the mass of aluminum chloride.
32.
You trap 6.99 grams of hydrogen chloride from a reaction. How much aluminum chloride
was required to produce this quantity?
33.
In a misguided attempt to completely remove any water from your favorite cup, you add
40.00 grams of aluminum chloride. On removal, 14.328 grams of aluminum hydroxide are
recovered. How much hydrogen chloride is produced in what is no longer your morning
coffee mug?
34.
You isolate 9.35 grams of aluminum hydroxide and 9.35 grams of hydrogen chloride from
a reaction mixture. What is the minimum mass of each reactant necessary to produce this
combination?
35.
From the remaining product in problem 34, how much water was required to produce its
mass?
4 HOCl + C → 2 H
2
O + CO
2
+ 2 Cl
2
36.
On running this experiment in the lab, your apparatus for collecting water and carbon
dioxide malfunctions. Knowing that you started with only 2.965 grams of carbon and
12.09 grams of hypochlorous acid, what should have been your mass yield for each?
37.
You are trying to find the carbon content in a 56.32 gram sample of coal, supposedly
75.41% carbon by weight. What mass of chlorine gas should be released on reaction?
38.
The chlorine gas and carbon dioxide gas from the previous problem would be a mixture.
What mass of carbon dioxide would be present?
39.
You foolishly believe if you run out of pencil graphite during your chemistry final that you
would be excused from taking it. What mass of hypochlorous acid would be required to
consume the 0.04 grams in your writing instrument?
40.
What total mass of products was formed through the reaction of 272.17 grams
hypochlorous acid and 14.41 grams of carbon?
David Healy 2010
Molecule / Mole Stoichiometry Practice Problems: Solutions
1.
90 N
2
molecules
21.
1868.1 g (NH
4
)
2
CrO
4
2.
164 N
2
O
5
molecules
22.
1.333 moles Cr(CrO
4
)
2
3.
16 N
2
molecules
23.
0.021 moles (NH
4
)
2
CrO
4
4.
374 N
2
O
5
molecules
24.
181000 grams (NH
4
)
3
N and 567000 grams
Cr(CrO
4
)
2
5.
1286 N
2
and 3215 O
2
molecules
25.
1.083 moles (NH
4
)
2
CrO
4
6.
1865 CO
2
molecules
26.
5137.0 grams Na
3
PO
4
and 7502.0 grams
CuSO
4
7.
1122 H
2
O molecules
27.
104.8 moles Cu
3
(PO
4
)
2
8.
272 O
2
molecules
28.
4000 grams CuSO
4
9.
55312 O
2
molecules
29.
39.29 moles Na
3
PO
4
10.
34570 CO
2
and 41484 H
2
O molecules
30.
190. grams Cu
3
(PO4)
2
11.
1325. moles H
2
O
31.
78.55 grams AlCl
3
12.
4.818 moles H
2
O
32.
8.33 grams HCl
13.
26.91 moles CO
2
33.
20.092 grams HCl
14.
12.19 moles C
8
H
18
34.
4.62 grams H
2
O and 11.1 grams AlCl
3
15.
105.41 moles CO
2
and 118.59 moles H
2
O
35.
1.86 grams H
2
O
16.
132.843 moles MgO
36.
0.6921 grams CO
2
and 2.075 grams H
2
O
17.
18.09 moles Fe(NO
3
)
3
37.
501.4 grams Cl
2
18.
842.0 moles Fe(NO
3
)
3
38.
169..7 grams CO
2
19.
3.62 moles Fe
2
O
3
39.
0.7 grams HOCl
20.
10.9 moles Mg(NO
3
)
2
40.
271.0 grams of products