Question

During the electrolysis of Copper (ll) chloride solution, 3.2g of Copper was deposited at the cathode, calculate the volume of chlorine gas evolved at the anode at STP at the same time. Given cu=64, 1F=96500C. Molar volume of gas at STP=22.4/dm^3

Answer 1

find the moles of Cu deposited ... 3.2 g / molar mass of Cu

there will be two moles of Cl evolved for every mole of Cu
... but because Cl is diatomic in the gaseous phase
... there will be equal moles of Cu and Cl2

Answer 2

96,500 coulombs will deposit 64/2 = 32 g Cu; therefore,
96,500 x 3.2/32 = 9,650 coulombs
2Cl^- ==> Cl2(g) + 2e so 96,500 coulombs will displace 22.4/2 = 11.2 L Cl2 gas @ STP.
Then 11.2 x (9,650/96,500) = 11.2/10 = ? L.
Check my work.

Answer 3

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