Exactly 0.2 mole electrons are passed through two electrolytic cells in series containing `CuSO_(4)` and `ZnSO_(4)` respectively. How many grams of each metal will be deposited on the respective cathodes in the two cells ?

Exactly 0.2 mole electrons are passed through two electrolytic cells i

1.	Exactly 0.2 mole electrons are passed through two electrolytic cells in series containing `CuSO_(4)` and `ZnSO_(4)` respectively. How many grams of each metal will be deposited on the respective cathodes in the two cells ?
Answer» Gram equivalent mass of copper `=(63.5)/(2)=31.75 g` Gram equivalent mass of zinc `=(65.0)/(2)=32.50 g` Now, `" " 1.0" mole"` of electrons deposit copper=31.75 g 0.2 mole of electrons deposit copper `=((31.75 g)xx(0.2 mol))/((1.0 mol))=6.35 g` Similarly, 1.0 mole of electrons deposit zinc=32.50 g 0.2 mole of electrons deposit zinc`=((32.50g)xx(0.2 mol))/((1.0 mol))=6.50 g`

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Exactly 0.2 mole electrons are passed through two electrolytic cells in series containing `CuSO_(4)` and `ZnSO_(4)` respectively. How many grams of each metal will be deposited on the respective cathodes in the two cells ?

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