Question

Given, for $ Sn^{4+}/Sn^{2+} $ , standard reduction potential is $ 0.15 \,V $ and for $ Au^{3+}/Au $ , standard reduction potential is $ 1.5\, V $ .
For the reaction,
$ \ce{3Sn^{2+} + 2Au^{3+} -> 3Sn^{4+} + 2Au } $ ,
the value of $ E^{\circ}_{cell} $ is,

• A. $ + 1.35 $
• B. $ + 2.55 $
• C. $ - 1.35 $
• D. $ - 2.55 $

Answer 1

Answer: (A)

$ E_{\text {cell }}^{\circ} =E_{\text {cathode }}^{\circ}-E_{\text {anode }}^{\circ} $

$=1.5-0.15=1.35\, V$