The mass of zinc produced by the electrolysis of zine sulphate solution with a steady current of $0.015 \mathrm{~A}$ for 15 minutes is _________ $\times 10^{-4} \mathrm{~g}$.
(Atomic mass of zinc $=65.4 \mathrm{~amu}$)
Answer (integer)
46
Solution
<p>$$\begin{aligned} & \mathrm{Zn}^{+2}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Zn} \\ & \mathrm{W}=\mathrm{Z} \times \mathrm{i} \times \mathrm{t} \\ & =\frac{65.4}{2 \times 96500} \times 0.015 \times 15 \times 60 \\ & =45.75 \times 10^{-4} \mathrm{gm}\end{aligned}$$</p>
About this question
Subject: Chemistry · Chapter: Electrochemistry · Topic: Electrochemical Cells
This question is part of PrepWiser's free JEE Main question bank. 127 more solved questions on Electrochemistry are available — start with the harder ones if your accuracy is >70%.