Question

Predict the products of electrolysis in each of the following: (i) An aqueous solution of AgNO3 with silver electrodes. (ii) An aqueous solution of AgNO3with platinum electrodes. (iii) A dilute solution of H2SO4with platinum electrodes. (iv) An aqueous solution of CuCl2 with platinum electrodes.

Answer 1

Answer:

7/8mg magnesium

hope it helps

Answer 2

All ions are in aqueous state

(i)

Reaction in solution

AgNO3 ↔ Ag+ + NO3–

H2O ↔ H+ + OH–

Reaction at cathode

Ag+ + e-→ Ag

Reaction at anode

Ag(s) + NO3– → AgNO3(aq) + e-

Hence Ag will deposit at cathode and dissolve at anode

(ii)

Reaction in solution

AgNO3 ↔ Ag+ + NO3–

H2O ↔ H+ + OH–

Reaction at cathode

Ag+ + e-→ Ag

Reaction at anode

Due to platinum electrode self of ionization of water will take place

H2O → 2H+ + 1/2O2(g) + 2e-

Hence Ag will deposit at cathode and O2 gas will generate at anode

(iii)

Reaction in solution

H2SO4 ↔ 2H+ + SO42–

H2O ↔ H+ + OH–

Reaction at cathode

H+ + e-→ ½ H2

Reaction at anode

Due to platinum electrode self of ionization of water will take place

H2O → 2H+ + 1/2O2(g) + 2e-

Hence H2 gas will generate at cathode and O2 gas will generate at anode

(iv)

Reaction in solution

CuCl2(s) ↔ Cu2+ + 2Cl–

H2O ↔ H+ + OH–

Reaction at cathode

Cu2+ + 2e-→ Cu(S)

Reaction at anode

2Cl– → Cl2 + 2e-

Hence Cu will deposit at cathode and Cl2 gas will generate at anode