Question

The reaction $\frac{1}{2}\times H_2\left(g\right)+AgCl\left(aq\right)\to H^{+}\left(aq\right)+Ag\left(s\right)$

can be represented in the galvanic cell as:

• A. Ag/AgCl(s) | KCl(sol) || AgNO${}_3$ (sol) | Ag
• B. PtH${}_2$(g) | HCl(sol) || AgNO${}_3$ (sol) | Ag
• C. Pt,H${}_2$(g) | HCl(sol) || AgCl(s) | Ag
• D. H${}_2$(g) | HCl(sol) || AgCl(s) | Ag

Answer 1

Answer: (C)

Pt,H${}_2$(g) | HCl(sol) || AgCl(s) | Ag

$H_2$ gets oxidised to $HCl$ in galvanic cell

$Pt,H_2|HCl\left(sol\right)$ forms cathode

$AgCl\left(s\right)|Ag$ forms anode

$\therefore$ The cell can be written as

$Pt,H_2\left(g\right)|HCl\left(sol\right)||AgCl\left(s\right)|Ag$

Hence, the correct option is $\text{C}$