In a certain electrolysis experiment, $0.650 \mathrm{~g}$ of zinc is deposited in a cell having…

In a certain electrolysis experiment, $0.650 \mathrm{~g}$ of zinc is deposited in a cell having $\mathrm{ZnSO}_4$ solution. Calculate mass of $\mathrm{Cu}$ deposited in other cell having $\mathrm{CuSO}_4$ solution arranged in series with first cell ? (molar mass of $\mathrm{Zn}=65, \mathrm{Cu}=63.5 \mathrm{~g} \mathrm{~mol}^{-1}$ )
  1. 0.635 g
  2. 6.35 g
  3. 0.317 g
  4. 3.17 g

Solution

$\frac{W_1}{E_1}=\frac{W_2}{E_2}$ $\frac{0.65}{\frac{65}{2}}=\frac{W_2}{\frac{63.5}{2}}$ $W_2=0.635 \mathrm{~g}$

Asked in: MHT CET 2022 (08 Aug Shift 2)

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