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1.
Suppose someone gave you a container with 1 mole of N
2
. Estimate the number of
N
atoms in the container at (a) P=1 atm, T=298K, (b)
P = 0.1 atm, T = 298K, and (c) P=1
atm, T = 1000K.
Use Table C.3 in your textbook, assume that nitrogen is an ideal gas
and that its heat capacity is temperature independent
.
We have solved this problem in the class (except that we were doing it for O
2
). Here are
the answers:
a) the number of atoms is N ~ 2.97
×
10
56
< 1 (i.e., zero)
b) N = 0
c) N = 178
Note: You could solve this by either using the van’t Hoff eq., in which case you would
have to take the temperature dependence of
∆
H into account (assuming that the heat
capacities are constant) or you could simply look up the
∆
G
f
for each component at
T=1000K
2.
For the reaction
CH
4
(g) + H
2
O(g) = CO(g) + 3H
2
(g)
A
. Calculate the equilibrium constant K at T=500K, P=1 atm, using the following data:
∆
G
f
(CH
4
) = 32741 J/mol,
∆
G
f
(H
2
O) = 219051 J/mol,
∆
G
f
(CO) = 155414 J/mol,
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 Spring '08
 LIM
 Physical chemistry, Atom, Mole, pH

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