A constant current was passed through a solution of $\mathrm{AuCl}_4^{-}$ ion between gold electrodes. After a period of 10.0 minutes, the increase in mass of cathode was $1.314 \mathrm{~g}$. The total charge passed through the solution is _______ $\times 10^{-2} \mathrm{~F}$.
(Given atomic mass of $\mathrm{Au}=197$)
Answer (integer)
2
Solution
<p>$$\begin{aligned}
& \frac{\mathrm{W}}{\mathrm{E}}=\frac{\text { charge }}{1 \mathrm{~F}} \\
& \frac{1.314}{\frac{197}{3}}=\frac{\mathrm{Q}}{1 \mathrm{F}} \\
& \mathrm{Q}=2 \times 10^{-2} \mathrm{~F}
\end{aligned}$$</p>
About this question
Subject: Chemistry · Chapter: Electrochemistry · Topic: Electrochemical Cells
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