The first step in electroplating with gold (Au) is to use the following redox reaction. What is being oxidized and what is being reduced?

Question

2Au (s) + 6HCI (aq) > 2AuCI3 (aq)+ 3H2 (g)

Answer 1

This is the molecular equation:

2Au_(s) + 6HCI_(aq) → 2AuCI_3(aq) + 3H_2(g)

This is the completed ionic equation:

2Au_(s) + 6H⁺_(aq) + 6CI^-_(aq) → 2Au³⁺_(aq) + 6CI^-_(aq) + 3H_2(g)

This is the net ionic equation:

2Au_(s) + 6H⁺_(aq) → 2Au³⁺_(aq) + 3H_2(g)

The Au lost three electrons, the Au is being oxidized!

Au_(s) → Au³⁺_(aq) + 3e^-

The H⁺ gain two electrons, the H⁺ is being reduced?

2H⁺_(aq) → H_2(g)