Question

A steady current passing through a solution of $AgN{O}_3$ deposits $0.50g$ of $Ag$ in $1h$ . What volume of hydrogen in $mL$ at $27^{\circ }C$ and $750mm$ pressure would the same current liberate in one hour?
Express your answer by rounding off up to two significant figures

Answer 1

Answer: 58

$W=0.5g,t=1hrW=Z.Q=\frac{\text{ Gram equivalent weight }\times Q}{96500}$
Number of coulombs $=\frac{0.5\times 96500}{108}C=446.7C$
Gram equivalents of $H_2$ produced $=\frac{Q}{96500}=\frac{446.7}{96500}$
$\frac{v_{H_2}}{\frac{\text{ molar volume }}{2}}=\frac{446.7}{96500}$
(For $H_2$, equivalent volume $=\frac{\text{ molar volume }}{2}$ )
$V_{H_2}=4.6296\times 10^{-3}\times \frac{\text{ molar volume }}{2}$
$=4.6296\times 10^{-3}\times \frac{0.0821\times 300}{750/760\times 2}=0.0577L=57.7mL$