An acidic solution of $C u^{2 +}$ salt containing $0.4 g$ of $C u^{2 +}$ is electrolysed until all the copper is deposited. The electrolysis is continued for seven more minutes will volume of solution kept at $100 m L$ and the current at $1.2 a m p$ . Calculate the gases evolved at NTP during the entire electrolysis.

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Solution

$0.4 g$ of $C u^{2 +} = \frac{0.4}{31.75} = 0.0126 g$ equivalent
At the same time, the oxygen deposited at anode
$- 0.0126 g - e q u i v a l e n t$
$= \frac{8}{32} \times 0.0126 = 0.00315 g - m o l e$
After the complete deposition of copper, the electrolysis will discharge hydrogen at cathode and oxygen at anode.
The amount of charge passed $= 1.2 \times 7 \times 60 = 504 c o u l o m b$
So, Oxygen liberated $= \frac{1}{96500} \times 504 = 0.00523 g - e q u i v a l e n t$
$= \frac{8}{32} \times 0.00523 = 0.001307 g - m o l e$
Hydrogen liberated $= 0.00523 g - e q u i v a l e n t$
$= \frac{1}{2} \times 0.00523 = 0.00261 g - m o l e$
Total gases evolve $= (0.00315 + 0.001307 + 0.00261) g - m o l e$
$= 0.007067 g - m o l e$
Volume of gases evolved at NTP
$= 22400 \times 0.007967 m L$
$= 158.3 m L$ .

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