Electrochemistry (Class 12)
Galvanic and electrolytic cells, Nernst equation, conductance, Kohlrausch's law, batteries.
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Take a full mock →Q1 · Electrochemistry (Class 12) · EASY
A galvanic cell is set up with electrodes of zinc and copper in solutions of their respective sulphates. Given that E°(Zn²⁺/Zn) = -0.76 V and E°(Cu²⁺/Cu) = +0.34 V. What is the standard EMF of the cell?
Q2 · Electrochemistry (Class 12) · MEDIUM
The molar conductivity of 0.05 M solution of a weak acid is 16 ohm⁻¹ cm² mol⁻¹. If the molar conductivity at infinite dilution for the weak acid is 400 ohm⁻¹ cm² mol⁻¹, what is the degree of dissociation of the acid?
Q3 · Electrochemistry (Class 12) · HARD
For the cell reaction: Zn(s) + Cu²⁺(aq) → Zn²⁺(aq) + Cu(s), the cell potential at 298 K is 1.05 V when [Zn²⁺] = 0.1 M. Given that E°(cell) = 1.10 V, what is the concentration of Cu²⁺ ions? (Take 2.303RT/F = 0.06 V at 298 K)