Answer to Question #142013 in Chemistry for Kosalu

Question

Calculate the time it will take to deposit 1 mole of silver if a current of 6A is passed through a solution of silver trioxonitrate (v) (F=96500)

Answer 1

Silver trioxonitrate, or silver nitrate AgNO₃ solution electrolysis reaction at cathode is the following:

Ag⁺ + e^- $\rightarrow$ Ag.

According to the Faraday's laws of electrolysis, the number of the moles of the deposited silver is proportional to the charge passed through the solution:

$n(Ag) = \frac{It}{F}$ .

Therefore, the time needed to deposit 1 moles of silver with a current of 6 A is:

$t = \frac{n(Ag)·F}{I} = \frac{1 \text{ mol}·96500\text{ C/mol}}{6\text{ A}} = 16083$ seconds, or 268 minutes, or 4 hours 28 minutes.

Answer: it will take 4 hours 28 minutes to deposit 1 mole of silver if a current of 6 A is passed through a solution of silver trioxonitrate.