Answer to Question #281671 in Inorganic Chemistry for kahuuu

Question

When an aqueous solution containing gold (III) salt is electrolyzed, metallic

gold is deposited at the cathode and oxygen gas is generated at the anode. If

9.26 g of Au is deposited at the cathode, calculate the volume (in liters) of O2

generated at 23°C and 747 mmHg.

Answer 1

Mole ratio for discharge is:

Au : O

2 : 3.

Moles of oxygen discharged was

3/2 × 9.26 = 13.89 moles

Volume of oxygen :

At RTP, molar gas volume is 24dm³

Volume of 13.89 moles of oxygen is

13.89×24=333.36litres

P1V1/T1=P2V2/T2

296×747/V2 = 298×760/333.36

And = 325.46 litres