Problem 104P
Problem 104P
Gold is electroplated at the cathode of an electrolysis cell by this half-reaction.
Au3+(aq) + 3e‑ → Au(s)
How many moles of electrons are required to electroplate 1.40 g of Au?
Step-by-Step Solution:
Solution 104 P:
Here, we are going to calculate the moles of electrons are required to electroplate of 1.40 g of Au.
Step 1:
Molar mass of Au =196.96 g/mol
Amount of Au required to electroplate 5.8 g of Au = 1.40 g Au x
= 0.0071 mol
Step 2 of 2
