Gold can be electrochemically "plated" onto a less expensive metal by submerging the object in a solution of gold(III)and applying an electric current to drive the following half-reaction:
Au³⁺ + 3e^- $\rarr$ Au(s)
How many grams of gold will be formed if a current of 2.37 A is applied for 71 minutes?

Question

Gold can be electrochemically "plated" onto a less expensive metal by submerging the object in a solution of gold(III)and applying an electric current to drive the following half-reaction:
Au³⁺ + 3e^-

\rarr

Au(s)
How many grams of gold will be formed if a current of 2.37 A is applied for 71 minutes?

Quizplus · Accepted Answer

The Answer of Gold can be electrochemically "plated" onto a less expensive metal by submerging the object in a solution of gold(III)and applying an electric current to drive the following half-reaction: Au³⁺ + 3e^- $\rarr$ Au(s) How many grams of gold will be formed if a current of 2.37 A is applied for 71 minutes?

Gold Can Be Electrochemically "Plated" onto a Less Expensive Metal →\rarr→

Gold Can Be Electrochemically "Plated" onto a Less Expensive Metal $\rarr$