A constant current was passed through a solution of 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 solut

Question

A constant current was passed through a solution of  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 .

(Given atomic mass of Au = 197)

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Strategy:
 Determine the moles of Gold deposited and use the stoichiometry of the reduction reaction () to find the total charge passed in Faradays.

Step 1: Calculate moles of Au deposited
Mass . Atomic mass .

Step 2: Determine electrons transferred
In , Gold is in the  oxidation state.

Charge required  moles of electrons per mole of Au.

Step 3: Format the result

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