| Standard electrode potentials are: [AIPMT 2001] |
| \[F{{e}^{2+}}/Fe,\] \[{{E}^{o}}=-0.44\] |
| \[F{{e}^{3+}}/F{{e}^{2+}},\] \[{{E}^{o}}=0.77\] |
| \[F{{e}^{2+}},\,F{{e}^{3+}}\] and Fe block are kept together, then: |
A) \[F{{e}^{3+}}\] increases
B) \[F{{e}^{3+}}\] decreases
C) \[\frac{F{{e}^{2+}}}{F{{e}^{3+}}}\] remains unchanged
D) \[F{{e}^{2+}}\] decreases
Correct Answer: B
Solution :
[b] The metals have higher negative values of their electrode potential can displace metals having lower values from their salt solution. So \[F{{e}^{3+}}\] decreases.
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