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Chemistry
Chemistry
Problem
Consider the following standard electrode potentials:
SO
4
2
−
(
aq
)
+
4
H
+
(
aq
)
+
2
e
−
⇌
\text{SO}_4^{2-}(\text{aq}) + 4\text{H}^+(\text{aq}) + 2\text{e}^- \rightleftharpoons
SO
4
2
−
(
aq
)
+
4
H
+
(
aq
)
+
2
e
−
⇌
E
cell
⊖
=
E^\ominus_{\text{cell}} =
E
cell
⊖
=
H
2
SO
3
(
aq
)
+
H
2
O
(
l
)
\text{H}_2\text{SO}_3(\text{aq}) + \text{H}_2\text{O}(\text{l})
H
2
SO
3
(
aq
)
+
H
2
O
(
l
)
+
0.17
V
+0.17 \text{ V}
+
0.17
V
Ag
+
(
aq
)
+
e
−
→
Ag
(
s
)
\text{Ag}^+(\text{aq}) + \text{e}^- \rightarrow \text{Ag}(\text{s})
Ag
+
(
aq
)
+
e
−
→
Ag
(
s
)
E
cell
⊖
=
E^\ominus_{\text{cell}} =
E
cell
⊖
=
+
0.80
V
+0.80 \text{ V}
+
0.80
V
What is the cell potential, in V, for the spontaneous reaction that occurs when these two half-cells are connected in a voltaic cell?
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