Which of the following would require the most Faradays of electricity?

Question

Quizplus · Accepted Answer

The amount of Faradays required for an electrochemical reaction is directly proportional to the number of moles of electrons (or moles of charge) transferred in the reaction. This is determined by the stoichiometry of the reaction, specifically the change in oxidation state of the element being reduced or oxidized. For option C, converting 1.5 mol of Cr^+6 to Cr requires a reduction of 6 electrons per Cr atom to reach an oxidation state of 0. Therefore, for 1.5 mol of Cr, the total moles of electrons needed would be 1.5 mol * 6 e^-/mol = 9 mol of electrons. This is the highest amount of electron transfer among the given options, making it require the most Faradays of electricity.

Which of the Following Would Require the Most Faradays of Electricity