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, ${3Sn^{2+} + 2Au^{3+} -> 3Sn^{4+} + 2Au }$ , the value of $E^{\circ}_{cell}$ is,

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

Answer 1

Answer: (A)

$+ 1.35$

Answer 2

$E_{\text {cell }}^{\circ} =E_{\text {cathode }}^{\circ}-E_{\text {anode }}^{\circ}$
$=1.5-0.15=1.35\, V$