Galvanic / electrolytic cells, electrode potentials, Nernst equation, conductance, batteries, corrosion.
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Q1 · Electrochemistry · EASY
A galvanic cell is constructed using a zinc electrode in 1 M ZnSO₄ solution and a copper electrode in 1 M CuSO₄ solution. The standard electrode potentials are: E°(Zn²⁺/Zn) = -0.76 V and E°(Cu²⁺/Cu) = +0.34 V. What is the standard cell potential (E°cell) for this galvanic cell?
Q2 · Electrochemistry · MEDIUM
The molar conductivity of 0.01 M acetic acid solution is 16.3 S cm² mol⁻¹. If the molar conductivity at infinite dilution for acetic acid is 390.7 S cm² mol⁻¹, what is the degree of dissociation of acetic acid in this solution?
Q3 · Electrochemistry · MEDIUM
An electrochemical cell is represented as: Zn(s) | Zn²⁺(0.1 M) || Cu²⁺(0.01 M) | Cu(s). Given E°(Zn²⁺/Zn) = -0.76 V and E°(Cu²⁺/Cu) = +0.34 V. Using the Nernst equation at 298 K, what is the cell potential? (Take 2.303RT/F = 0.06 V)
Q4 · Electrochemistry · EASY
In the electrolysis of aqueous sodium chloride using inert electrodes, which of the following products are obtained at the anode and cathode respectively?
Q5 · Electrochemistry · MEDIUM
The standard electrode potential of Zn²⁺/Zn is -0.76 V and that of Cu²⁺/Cu is +0.34 V. The EMF of the cell Zn|Zn²⁺||Cu²⁺|Cu is: