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

To find the mass of gold formed, use the formula: mass = (current * time * molar mass) / (n * F), where n = 3 (electrons), F = 96485 C/mol, and molar mass of Au = 197 g/mol. Calculate: (2.37 A * 4260 s * 197 g/mol) / (3 * 96485 C/mol) ≈ 6.9 g.

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

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