JEE Main · 2024 · 29 Jan 2024 · Shift 2 · Redox Reactions and Electrochemistry

A constant current was passed through a solution of

AuCl X_{4} X^{-}

ion between gold electrodes. After a period of 10.0 minutes, the increase in mass of cathode was 1.314 g. The total charge passed through the solution is _____

\times 1 0^{- 2} F

.
(Given atomic mass of

Au = 197

)

Answer: 2

Solution

Gold is deposited from

AuC l_{4}^{-}

, in which gold is in the +3 state, so

n = 3

and the equivalent mass of Au is

197/3

.

By Faraday's law, the charge passed (in Faradays) equals mass deposited divided by equivalent mass:

Q (F) = \frac{W}{E} = \frac{1.314}{197/3} = \frac{1.314 \times 3}{197} = \frac{3.942}{197} = 0.02 F

The charge passed through the solution is

2 \times 1 0^{- 2} F

JEE Main · 2024 · 29 Jan 2024 · Shift 2 · Integer answer

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