Correct Answer: Option B

Explanation

Cu\(^{2+}\) + 2e\(^{-}\)\(_{(aq)}\) \(\rightarrow\) Cu\(_{(s)}\)

Liberating 1 mole of Cu

2 x 1F = 2 x 96,500C = 193,000C of electricity is needed

Hence, 193,000C = 1 mole

360C of electricity = \(\frac{360C \times 1 mol}{193,000C}\)

= 0.001865 mol

= 1.87 x 10\(^{-3}\) moles

There is an explanation video available below.

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