Calculate the cell potential at 298 K for the cell notation: M(s) | M3+(aq, 0.01 M) || N2+(aq, 0.1 M) | N(s) Given standard reduction potentials are E°M3+/M = -0.74 V and E°N2+/N = -0.23 V. (Take 2.303 RTF = 0.06 V)

Calculate the oxidation potential (emf) of the given half-cell: Pt(s) | H2(g, 2 atm) | HCl(aq, 0.02 M) Given E°H2/H+ = 0 V, 2.303 RTF = 0.059, and log 2 = 0.3010.

A solution of copper sulphate is electrolysed for 10 minutes with a current of 1.5 amperes. The mass of copper deposited at cathode is: (Given: Molar mass of Cu = 63 g mol-1, 1 F = 96487 C mol-1)