A) 0.653 V
B) 0.889 V
C) 0.0653V
D) 2.771V
Correct Answer: A
Solution :
The Nernst?s equation, for the half-cell reaction, \[F{{e}^{3+}}+{{e}^{-}}\xrightarrow{{}}F{{e}^{2+}}\]is \[{{E}_{F{{e}^{3+}}/F{{e}^{2+}}}}=E_{F{{e}^{3+}}/F{{e}^{2+}}}^{o}-\frac{0.0591}{1}\log \frac{[F{{e}^{2+}}]}{[F{{e}^{3+}}]}\] \[=0.771-0.0591\log \frac{2.00}{0.02}\] \[=0.771-0.0591\log {{10}^{2}}\] \[=0.771-0.0591\times 2\] \[=+\,0.653\,V\]You need to login to perform this action.
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