+91-8076753736 support@wiredfaculty.com
logo
logo

Sponsor Area

Electrochemistry

Question
CBSEENCH12010042
Wired Faculty App

Following reactions occur at cathode during the electrolysis of aqueous silver chloride solution:


Ag+ (aq) + e-  →  Ag(s)          E° = +0.80 V

 H+ (aq) + e-   → 1/2 H2 (g)     E° = 0.00 V

 On the basis of their standard reduction electrode potential (E°) values, which reaction is feasible at the cathode and why?

Solution

We have given:

 Ag+ (aq) + e- → Ag(s)          E° = +0.80 V

 H+ (aq) + e-→ 1/2 H2 (g)      E° = 0.00 V

 

The relationship between the standard free energy change and emf of a cell reaction is given by 
∆ G = – nFE(cell)

Thus, the more positive the standard reduction potential of a reaction, the more negative is the standard free energy change associated with the process and, consequently, the higher is the feasibility of the reaction.
Since E 0 Ag+/Ag has a greater positive value than E0 H+ /H, the reaction which is feasible at the cathode is given by

 Ag+ (aq) + e- → Ag(s)         

 

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-?

Mock Test Series

Mock Test Series

NCERT Sample Papers

Entrance Exams Preparation