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(C) According to Faraday's law of electrolysis,the mass $m$ deposited is given by $m = ZIt$,where $Z = \frac{M}{nF}$.Here,$M$ (molar mass of $Na$) $=

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$2.3$

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(C) According to Faraday's law of electrolysis,the mass $m$ deposited is given by $m = ZIt$,where $Z = \frac{M}{nF}$.Here,$M$ (molar mass of $Na$) $= 23 \, g/mol$,$n = 1$ (for $Na^+ + e^- ightarrow Na$),$I = 16 \, A$,and $t = 10 	imes 60 = 600 \, s$.Substituting the values:$m = \frac{23 	imes 16 	imes 600}{1 	imes 96500}$$m = \frac{220800}{96500} \approx 2.288 \, g \approx 2.3 \, g$.Thus,the correct option is $C$.

When a current of $16 \, A$ is passed through a $NaCl$ cell for $10 \, min$,what mass of $Na$ (in $g$) is deposited?

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