Nernst Equation and Effect of Concentration
Apply the Nernst equation to calculate cell and electrode potentials under non-standard conditions and understand the effect of concentration and pH.
Why this shows up in the exam
NEET/JEE frequently test calculations involving the Nernst equation and the impact of changing concentrations on cell potential.
How NEET tests this
Practise it
These are real questions from past NEET papers that test this exact idea.
In the electrochemical cell : Zn|ZnSO₄(0.01 M)||CuSO₄(1.0 M)|Cu, the emf of this Daniell cell is E₁. When the concentration of ZnSO₄ is changed to 1.0 M and that of CuSO₄ changed to 0.01 M, the emf changes to E₂. From the followings, which one is the relationship between E₁ and E₂? (Given, RT/F = 0.059)
Push further
More challenging1 harder question built from the past papers above — a step up in difficulty, with distractors designed so you can't get there by elimination. Written and checked by our reviewers, not from a real paper.
A copper electrode is immersed in a 0.01 M solution of copper(II) sulfate. Given the standard electrode potential E°(Cu²⁺/Cu) = +0.34 V, calculate the electrode potential at 25°C. (Assume 2.303 RT/F = 0.059 V)
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