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5.6 TheKinetic Molecular Theory of Gases
205
In this case, the partial pressure of the O
2
is
733 terf
=
0.964 atm
P
=
733 torr
=
760 terr/atm
0,
To find the moles of O
2
produced, we use
v
=
0.650 L
T
=
22°C
+
273
=
295 K
R
=
0.08206 L . atmlK . mol
(0.964 atm)(0.650~)
n -
-;;:-;~~~-~-.:..:...:: .... =.'~-
O
2 -
(0.08206 ~ . aHI1/K • mol)(295
K)
=
2.59 X 10-
2
mol
How many moles of KClO
3
are required to produce this amount of 02?
Use the stoichiometry problem-solving strategy:
1~ What is the balanced equation?
2KCI0
3
(s) ~ 2KCI(s)
+
30
2
(g)
2 ~ What is the mole ratio between KClO
3
and O
2
in the balanced equation?
1mol HCI 2 mol KCI0
3
1mol NaHC0
3
3mol O
2
3~ What are the moles of KClO
3
?
2mol KCI0
3
2.59
X
10- 2 meI:-02
X =
1.73
X
10- 2 mol KCI0
3
3meI:-02
4 ~ What is the mass of KClO
3
(molar mass 122.6 g/mol) in the original sample?
122.6 g KCIO
1.73
X
10- 2
~
X
3
=
2.12 g KCI0
3
1~
• Thus the original sample contained 2.12 g KCI0
3
.
SEE EXERCISES 5.87 THROUGH 5.89
5.6~
The Kinetic MoLecuLar Theory of Gases
Wehave sofar considered the behavior of gases from anexperimental point ofview. Based