Question

The emf of the cell involving the following reaction
$2A{g}^{+}+H_2\to 2Ag+2H^{+}$
is $0.80Volt$ . The standard oxidation potential of silver electrode is

• A. -0.80 V
• B. 0.80 V
• C. 0.40 V
• D. -0.40 V

Answer 1

Answer: (B)

$2A{g}^{+}+H_2\to 2Ag+2H^{+}$
By convention, the cell may be represented as.
$H_2|H^{+}|A{g}^{+}|Ag$
$\therefore E_{\text{cell}}^{\circ }=E_{A{g}^{+}/Ag}^{\circ }-E_{H^{+}/H_2}^{\circ }$
or $E_{A{g}^{+}/Ag}^{\circ }=E_{\text{cell}}^{\circ }+E_{H^{+}/H_2}^{\circ }$
$=0.80+0=0.80v$
Thus, standard reduction potential of $Ag$ electrode as,
$E_{A{g}^{+}/Ag}^{\circ }=0.80V$
and standard oxidation potential of $Ag$ electrode as,
$E_{Ag/A{g}^{+}}^{\circ }=-0.80V$