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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 $\mathrm{Zn}=65, \mathrm{Cu}=63.5 \mathrm{~g} \mathrm{~mol}^{-1}$ )
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The correct answer is:
0.635 g
$\frac{W_1}{E_1}=\frac{W_2}{E_2}$
$\frac{0.65}{\frac{65}{2}}=\frac{W_2}{\frac{63.5}{2}}$
$W_2=0.635 \mathrm{~g}$
$\frac{0.65}{\frac{65}{2}}=\frac{W_2}{\frac{63.5}{2}}$
$W_2=0.635 \mathrm{~g}$
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