For the concentration cell, M|M+ (aq, 0.01 mol/dm3)| |M+ (aq), 0.1 mol/dm3|M the EMF (E) of the cell at a temperature (T) equals

According to the Debye-Huckel limiting law, if the concentration of a dilute aqueous solution of KCl is increased 4-fold, the value of In γzz is the molar mean ionic activity coefficient) will

Given the standard potential for the following half-cell reaction at 298 K,
Cu+(aq) + e- → Cu(s); E° = 0.52 V
Cu2+(aq) + e- → Cu+(aq); E° = 0.16 V
Calculate the ΔG° (kJ) for the reaction, [2Cu+(aq) → Cu(s) + Cu2+]

A student recorded a polarogram of 2.0 mM Cd2+ solution and forget to add KCl solution. What type of error do you expect in his results?

For a 2 molal aqueous NaCl solution, the mean ionic activity coefficient $$\left( {{\gamma _ \pm }} \right)$$  and the Debye-Huckel Limiting Law constant (A) are related as

The standard reduction potentials at 298 K for single electrodes are given below.
Electrode Electrode potential (volt)
Mg2+ /Mg -2.34
Zn2+ /Zn -0.76
Fe2+ /Fe -0.44
From this we can infer that

For the reaction, Hg2Cl2(s) + H2(g) → 2Hg(liq) + 2HCl(aq), the correct representation of the cell and the thermodynamic properties ΔG, ΔH and ΔS at 298 K respectively, are (Given: E298 = 0.2684 V and temperature coefficient = 3 × 10-4 VK-1)

The Nernst equation for the reaction, A2+ + 2e- → B, in terms of the free energy change is