B.Sc Chemistry Electrochemistry — practice questions
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In the Daniell cell shown, which metal acts asFor a galvanic cell, the standard cell EMF is given by:Given standard reduction potentials $E^{\circ}(\mathrm{Cu^{2+}/Cu}) = +0.34$ V and $E^{\circ}(\mathrm{Zn^{2+}/The Nernst equation for a half-cell reaction at 298 K is:How many coulombs of charge are required to deposit $108$ g of silver from a $\mathrm{AgNO_3}$ solution? (AtomWhen a current of $5$ A is passed through a $\mathrm{CuSO_4}$ solution for $193$ seconds, the mass of Cu deposA device converting CHEMICAL energy to electrical energy via spontaneous redox is a:In the Daniell cell, the cathode reaction is:EMF of standard Daniell cell at 25°C is approximately:Faraday's first law of electrolysis states mass deposited is proportional to:The value of Faraday's constant F is approximately:In a galvanic cell, electrons flow externally from:The Nernst equation gives cell EMF at non-standard conditions. For a half-cell Mⁿ⁺ + ne⁻ → M, it is:Relation between standard cell potential E°, ΔG°, and equilibrium constant K:For ΔG° < 0 (spontaneous), E° must be:The molar conductivity Λ_m of an electrolyte:Kohlrausch's law states the limiting molar conductivity of an electrolyte is:For the cell Zn | Zn²⁺ (1 M) || Cu²⁺ (1 M) | Cu, with E°(Zn) = -0.76 V, E°(Cu) = +0.34 V, E_cell:Standard electrode potential of SHE (Standard Hydrogen Electrode) is taken as:For Cu²⁺ + 2e⁻ → Cu, how much charge to deposit 0.5 mol Cu? (F = 96500 C/mol)Conductivity κ of pure water is approximately:At 25°C, ratio of Nernst factor 0.0591/n to RT/(nF) ln 10 in SI units:A current of 2 A flows for 30 min through a CuSO4 solution. Mass of Cu deposited (M_Cu = 63.5):For the cell: Zn|Zn²⁺(0.1 M)||Cu²⁺(0.01 M)|Cu, at 25°C, E_cell is:Equilibrium constant K of the Daniell cell at 25°C (E° = 1.10 V, n = 2):A 0.1 M weak acid HA has Λ_m = 10 S·cm²/mol; at infinite dilution Λ_m^0 = 400. Degree of dissociation α:In electrolysis of CuSO4 with Pt electrodes, the cathode product is:Standard electrode potentials: E°(Fe³⁺/Fe²⁺) = +0.77 V, E°(I2/I⁻) = +0.54 V. For the reaction 2Fe³⁺ + 2I⁻ → 2FWhy is the cell potential temperature-dependent?For Hg²⁺/Hg (E° = +0.79 V) and Cu²⁺/Cu (E° = +0.34 V), the spontaneous reaction is:Conductivity of a 0.01 M NaCl solution is 0.0014 S/cm. Molar conductivity Λ_m:Lead-acid battery during DISCHARGE: PbO2 + Pb + 2H2SO4 → 2PbSO4 + 2H2O. The role of PbO2 is:Corrosion of iron involves which type of reaction?In electroplating silver onto a spoon, the cathode is: