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Chemistry
Chemistry
Problem
Given the following data at 298 K: (i)
S
(
s
)
+
O
2
(
g
)
→
S
O
2
(
g
)
\mathrm{S(s)+O_2(g)\rightarrow SO_2(g)}
S
(
s
)
+
O
2
(
g
)
→
S
O
2
(
g
)
Δ
S
298
∘
=
+
11.6
J
mol
−
1
K
−
1
\Delta S^{\circ}_{298}=+11.6\;\text{J\,mol}^{-1}\,\text{K}^{-1}
Δ
S
298
∘
=
+
11.6
J
mol
−
1
K
−
1
(ii)
2
S
O
3
(
g
)
→
2
S
O
2
(
g
)
+
O
2
(
g
)
\mathrm{2\,SO_3(g)\rightarrow 2\,SO_2(g)+O_2(g)}
2
S
O
3
(
g
)
→
2
S
O
2
(
g
)
+
O
2
(
g
)
Δ
S
298
∘
=
+
257
J
mol
−
1
K
−
1
\Delta S^{\circ}_{298}=+257\;\text{J\,mol}^{-1}\,\text{K}^{-1}
Δ
S
298
∘
=
+
257
J
mol
−
1
K
−
1
Calculate
Δ
S
298
∘
\Delta S^{\circ}_{298}
Δ
S
298
∘
for the reaction
2
S
(
s
)
+
3
O
2
(
g
)
→
2
S
O
3
(
g
)
\mathrm{2\,S(s)+3\,O_2(g)\rightarrow 2\,SO_3(g)}
2
S
(
s
)
+
3
O
2
(
g
)
→
2
S
O
3
(
g
)
.
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