Consider the following electrochemical cell :

Chemistry Electrochemistry General Single Correct MCQ

Published by: CGP EDU Academic Team

Published on: August 12, 2026

Write a balanced net ionic equation for the spontaneous reaction that take place in the cell.

Calculte the standard cell potential Eº for the cell reaction.

If the cell emf is 1.6 V, what is the concentration of Zn 2+ ?

How will the cell potential be affected if KI is added to Ag + half-cell ?

Text Solution

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The correct answer is:

CHECK THE SOLUTION.

The spontaneous cell reaction : Zn + 2Ag + (aq) Zn 2+ (aq) + 2Ag (s)

1.56 V [Zn 2+ ] = 4 × 10 –4 M

As we add KI to cathode chamber, some Ag + will precipitate out as :

Ag + + I – ⎯→ AgI

The above reaction reducing [Ag + ] from cathode chamber. This will reduce E cell according to Nernst’s equation.

Sol. Zn + 2Ag + (aq) Zn 2+ (aq) + 2Ag(s)

Eº = 0.8 – (– 0.76) = 1.56 V

1.6 = 1.56– log or ( ;k ) 1.356 = log

or ( ;k ) log = 1.356 or ( ;k ) = 22.7 or ( ;k ) [Zn 2+ ] = = 4.4 × 10 –4 M

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