Chemistry 3411 Solutions Worksheet - Georgia Institute Of Technology - 2010 Page 2
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12CHEM 3411, Fall 2010
Solution Set 2
1
⊖
⊖
⊖
⊖
∆
H
(C
H
) = 3∆
H
(H
O(l)) + 3∆
H
(CO
(g))
∆
H
f
3
6
f
2
f
2
r
2
1
= 3 × 285.83 kJ mol
+ 3 × 393.51 kJ mol
× 2 × 2091 kJ mol
1
1
1
2
1
= 52.98 kJ mol
With this information we can now calculate the enthalpy of isomerization of cyclopropane to propene. The balanced
equation for this process is
⊖
(cyclopropane) → C
C
H
H
(propene)
∆
H
=?
3
6
3
6
r
The enthalpy of this reaction is simply given by
⊖
⊖
⊖
∆
H
= ∆
H
(propene)
∆
H
(cyclopropane)
r
f
f
1
= 20.42 kJ mol
52.98
=
32.56
Solution
⊖
• The enthalpy of formation of cyclopropane is ∆
1
H
(C
H
) = 53 kJ mol
.
f
3
6
⊖
• The isomerization enthalpy of cyclopropane to propene is ∆
1
H
=
33 kJ mol
.
r
2
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