Electrochemistry
Electrochemical cells and cell reactions; standard electrode potentials; Nernst equation; electrochemical series; emf; Faraday's laws of electrolysis; electrolytic conductance — specific, equivalent and molar conductivity; Kohlrausch's law; primary and secondary batteries; fuel cells; corrosion.
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Take a full mock →Q1 · Electrochemistry · HARD
A current of 2.5 A is passed through an aqueous solution of CuSO₄ for 40 minutes. The mass of copper deposited at the cathode is approximately: (Atomic mass of Cu = 63.5, Faraday constant F = 96500 C/mol)
Q2 · Electrochemistry · MEDIUM
The standard electrode potentials are: Zn²⁺/Zn = –0.76 V and Cu²⁺/Cu = +0.34 V. What is the standard cell potential (in V) for the Daniell cell?
Q3 · Electrochemistry · HARD
A galvanic cell is constructed using Ag⁺/Ag (E° = +0.80 V) and Cu²⁺/Cu (E° = +0.34 V) half-cells. If the [Ag⁺] = 0.01 M and [Cu²⁺] = 1.0 M at 298 K, calculate the cell potential (in V) using the Nernst equation. (Take 2.303RT/F = 0.059 V)