Exactly 0.4 faraday electric charge is passed through three electrolytic cells in series, first containing `AgNO_(3)`, second `CuSO_(4)` and third `Fe
Exactly 0.4 faraday electric charge is passed through three electrolytic cells in series, first containing `AgNO_(3)`, second `CuSO_(4)` and third `FeCl_(3)` solution. How many grams of each metal will be deposited assuming only cathodic reaction in each cell ?
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The cathodic reaction in the cells are respectively.
`underset(("1 mole"),(108 g))(Ag^(+))+underset(("1 mole"),("1 F"))(e^(-)) rarr Ag`
`underset(("1 mole"),(63.5 g))(Cu^(2+))+underset(("2 mole"),("2 F"))(2e^(-)) rarr Cu`
and `underset(("1 mole"),(56 g))(Fe^(3+))+underset(("3 mole"),("3 F"))(3e^(-)) rarr Fe`
Hence, Ag deposited `=108xx0.4=43.3 g`
Cu deposited `=63.5/2xx0.4=12.7 g`
and Fe deposited `=56/3 xx0.4 =7.47 g`
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