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Chemistry
Chemistry
Problem
The enthalpy and entropy changes for the reaction
A
(
s
)
+
B
(
aq
)
→
C
(
aq
)
+
D
(
g
)
\text{A}(\text{s}) + \text{B}(\text{aq}) \rightarrow \text{C}(\text{aq}) + \text{D}(\text{g})
A
(
s
)
+
B
(
aq
)
→
C
(
aq
)
+
D
(
g
)
are
Δ
H
⊖
=
100
kJ mol
−
1
\Delta H^\ominus = 100 \text{ kJ mol}^{-1}
Δ
H
⊖
=
100
kJ mol
−
1
and
Δ
S
⊖
=
100
J K
−
1
mol
−
1
\Delta S^\ominus = 100 \text{ J K}^{-1} \text{ mol}^{-1}
Δ
S
⊖
=
100
J K
−
1
mol
−
1
What does this tell you about the reaction?
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