AP Chemistry: Thermodynamics
AP Chemistry Thermodynamics WS 0809.doc
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1.
The following equation represents the essential change that takes place during the fermentation of
glucose to ethanol:
C
6
H
12
O
6(s)
→
2C
2
H
5
OH
(l)
+ 2CO
2(g)
Is
Δ
S
o
positive or negative?
Explain.
2.
Calculate the change of entropy,
Δ
S
o
, at 25.0
o
C for the reaction in which urea is formed from NH
3
and
CO
2
.
2NH
3(g)
+ CO
2(g)
→
NH
2
CONH
2(aq)
+ H
2
O
(l)
The standard entropy of urea is 174 J/molK.
See the text appendices for additional values.
3.
Using values of
Δ
H
o
f
and S
o
, calculate the standard free energy change,
Δ
G
o
, for the following
reaction at 25.0
o
C.
N
2(g)
+ 3H
2(g)
→
2NH
3(g)
4.
Using standard free energies of formation, calculate
Δ
G
o
for the combustion of 1 mol of ethanol,
C
2
H
5
OH, at 25.0
o
C.
C
2
H
5
OH
(l)
+ 3O
2(g)
→
2CO
2(g)
+ 3H
2
O
(g)
5.
Calculate
Δ
H
o
and
Δ
G
o
for the reaction
KClO
3(s)
→
2KCl
(s)
+ 3O
2(g)
Interpret the signs obtained for
Δ
H
o
and
Δ
G
o
.
Values of
Δ
H
o
f
(in kJ/mol) are as following: KClO
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- Fall '10
- Feebeck
- Chemistry, Thermodynamics, AP Chemistry, kJ/mol, standard free energy, free energy change, standard free energies
-
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