Question

A cell using Zn/Zn⁺² (aq, 1M) and H2 / H+1 (aq, 1M) generates a cell potential of + 0.67 V under standard conditions.

A. Write the half-cell reaction at the anode.

B. Write the half-cell reaction at the cathode.

C. Write the electrochemical cell notation.

D. Calculate the standard reduction potential at the anode.

Answer 1

(A): $Zn^0 (s) = Zn^{2+} (aq)+ 2e^-$

(C): $2H^+(aq) + 2e^- = H_2(g)$

$$Zn (s) + 2H^+ (aq) = Zn^{2+} + H_2(g)$$

$E_{cell} = E^0(2H^+/H_2) - Е^0(Zn^0/Zn^{2+}) = 0.763 V$