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Exactly 0.2 mole electrons are passed th...

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 ?

Text Solution

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Gram equivalent mass of copper `= (63.5)2) = 31.75g`
Gram equivalent mass of zinc `=(65.0)/(2) = 32.50g`
Now 1.0 mole of electrons deposit copper = 31.75g
0.2 mole of electrons deposit copper `= (31.75 xx 0.2)/(1.0)= 6.35g`
Similarly, 1.0 mole of electrons deposit zinc = 32.50g
0.2 mole of electrons deposit zinc `= (32.5 xx 0.2)/(1.0) = 6.50g`
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