☰
✕

Electrochemistry
Question
Wired Faculty App

Predict the products of electrolysis obtained at the electrodes in each case when the electrodes used are of platinum.
(i) An aqueous solution of AgNO3.
(ii) An aqueous solution of H2SO4.

Answer

(i)
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

(ii)
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

Sponsor Area

Some More Questions From Electrochemistry Chapter

Why does the conductivity of a solution decrease with dilution?

Suggest a way to determine the Λ°m value of water.

The molar conductivity of 0.025 mol L–1 methanoic acid is 46.1 S cm2 mol–1. Calculate its degree of dissociation and dissociation constant. Give λ°(H+) = 349.6 S cm2 mol–1 and λ° (HCOO– ) = 54.6 s cm2 mol–1.

If the current of 0.5 ampere flows through a metallic wire for 2 hours, then how many electrons flow through the wire?

Suggest a list of metals that are extracted electrolytically.

Consider the reaction: Cr2O72– + 14H+ + 6e- → 2Cr3+ + 8H2O
What is the quantity of electricity in coulombs needed to reduce 1 mol of Cr2O72-?

Write the chemistry of recharging the lead storage battery, highlighting all the materials that are involved during recharging.