Electronic concepts of oxidation and reduction; redox reactions; oxidation number; balancing redox reactions; electrolytic and metallic conduction; conductance — specific, equivalent and molar; Kohlrausch's law; electrochemical cells; EMF; standard electrode potential; Nernst equation; relation between Gibbs energy change and EMF; electrochemical series; fuel cells; corrosion; batteries; Faraday's laws of electrolysis.
Study notes are still being prepared.
Don't wait — Shishya can teach you this topic right now, on demand.
Ask Shishya to teach this →Shishya is your personal tutor for this topic. Pick a starter or open a free chat.
Q1 · Redox Reactions and Electrochemistry · EASY
In the reaction: 2MnO4^- + 5H2O2 + 6H+ → 2Mn^2+ + 5O2 + 8H2O, the oxidation state of manganese changes from +7 to +2. What is the equivalent weight of KMnO4 in this reaction? (Molar mass of KMnO4 = 158 g/mol)
Q2 · Redox Reactions and Electrochemistry · MEDIUM
The standard electrode potentials are: E°(Zn^2+/Zn) = -0.76 V and E°(Cu^2+/Cu) = +0.34 V. A galvanic cell is constructed using these two half-cells with 1 M concentrations. What is the standard EMF of the cell and which electrode acts as the anode?
Q3 · Redox Reactions and Electrochemistry · MEDIUM
The molar conductivity of 0.01 M solution of a weak acid HA is 20 S cm^2 mol^-1. The molar conductivity at infinite dilution for HA is 400 S cm^2 mol^-1. What is the degree of dissociation and the dissociation constant Ka of the acid?
Q4 · Redox Reactions and Electrochemistry · MEDIUM
A current of 0.5 A is passed through an aqueous solution of CuSO4 for 30 minutes. How much copper will be deposited at the cathode? (Atomic mass of Cu = 63.5 g/mol, Faraday constant = 96500 C/mol)
Q5 · Redox Reactions and Electrochemistry · HARD
For the electrochemical cell: Pt(s) | H2(1 atm) | H+(aq, pH = x) || Cu^2+(0.01 M) | Cu(s), the cell EMF is found to be 0.34 V at 298 K. Given E°(Cu^2+/Cu) = +0.34 V and 2.303RT/F = 0.059 V, what is the pH of the solution in the anode compartment?