AP EAMCET · Chemistry · Electrochemistry
The number of Faradays required to completely deposit magnesium from \(1 \mathrm{~L}\) of \(0.1 \mathrm{M} \mathrm{MgCl}_2\) aq. solution is
- A \(0.2\)
- B \(2\)
- C \(0.1\)
- D \(0.4\)
Answer & Solution
Correct Answer
(A) \(0.2\)
Step-by-step Solution
Detailed explanation
\(\begin{aligned} & \text {} \mathrm{MgCl}_2 \rightarrow \mathrm{Mg}^{2+}+2 \mathrm{Cl}^{-} \\ & \mathrm{Mg}^{2+}+2 \mathrm{e}^{-} \rightarrow \mathrm{Mg} \text { (s) } \end{aligned}\) 2 moles of \(\mathrm{e}^{-}\)are required to deposit 1 mole of \(\mathrm{Mg}(\mathrm{s})\).…
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