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Question: An acidic solution of \(Cu^{2 +}\) containing \(0.4g\) of \(Cu^{2 +}\)ions is electrolysed until all...

An acidic solution of Cu2+Cu^{2 +} containing 0.4g0.4g of Cu2+Cu^{2 +}ions is electrolysed until all the copper is deposited. What is the volume of oxygen evolved at NTP?

A

141cc141cc

B

31.75cc31.75cc

C

64 cc

D

32 cc

Answer

141cc141cc

Explanation

Solution

H2O→2H++12O2+2e−H_{2}O \rightarrow 2H^{+} + \frac{1}{2}O_{2} + 2e^{-} (oxidation)

Cu2++2e−→Cu(Reduction)Cu^{2 +} + 2e^{-} \rightarrow Cu ({Re}duction)

Cu2++H2O→Cu+2H++12O2Cu^{2 +} + H_{2}O \rightarrow Cu + 2H^{+} + \frac{1}{2}O_{2}

63.52=31.75gofCu2+≡12×22400=11200ccorO2\frac{63.5}{2} = 31.75gofCu^{2 +} \equiv \frac{1}{2} \times 22400 = 11200ccorO_{2}

∵31.75gCu2+\because 31.75gCu^{2 +} NTP 11200ccO211200ccO_{2}

∴0.4gCu2+1120031.75×0.4=141ccO2\therefore 0.4gCu^{2 +}\frac{11200}{31.75} \times 0.4 = 141ccO_{2}