Q. The potential of the following cell is 0.34 V at 25℃. Calculate the standard reduction potential of the copper half-cell. $Pt\ |\ H_{2}(1\ atm)\ |\ H^{+}\ (1\ M)\ ||\ {Cu}^{2 +}\ (1\ M)\ |\ Cu$
A) -3.4 V
B) +3.4 V
C) -0.34 V
D) +0.34 V
Explanation
(d)
Given, $E_{cell}^{{^\circ}}\ = \ 0.34\ V$
$E_{cell}^{{^\circ}} = E_{({Cu}^{2 +}\ /Cu)}^{{^\circ}} - \ E_{(H_{2}\ /H^{+})}^{{^\circ}}$ $\ \$
$0.34\ = \ E_{({Cu}^{2 +}\ /Cu)}^{{^\circ}} - \ 0.00$
∴ $E_{({Cu}^{2 +}\ /Cu)}^{{^\circ}}\ = \ + \ 0.34$
Reviewed by Dr. Abubacker
Physics Educator & NEET/JEE Specialist
Ph.D. in Physics with 19+ years of teaching experience.