500 ml of a waste solution obtained from a factory contains 0.5M $C u S O_{4}$ and 0.5M $Z n {(N O_{3})}_{2}$ The solution was electrolyzed at 6v by passing a current of 10A for 60 minutes. The metal/metals electrodeposited will be:
$(E_{c u^{2 +} / c u}^{0} = 0.34 V, E_{z n^{2 +} / z n}^{0} = - 0.76 V)$

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only Zn

Zn and Cu in equal mass proportion

Zn and Cu in proportion to their atomic mass

only Cu

answer is A.

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Detailed Solution

Amount of charge used =10×60×60=36000C=0.373F
Amount of $c u^{+ 2}$ available =0.5×0.5=0.25 mole
Amount of charge required to deposit all $c u^{+ 2}$ =0.5F
only $c u^{+ 2}$ will be deposited(partially), $z n^{+ 2}$ will not discharge

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