Question

Write the cell reaction and calculate the e.m.f. of the following cell at 298 K: Sn(s)|Sn²⁺ (0.004 M)||H⁺ (0.02 M)|H₂(g) (1 Bar)|Pt (s) (Given : E°(Sn²⁺/Sn) = –0.14 V, E°(H⁺|H₂(g), Pt) = 0.00V)

Account for the following:

Write the anode and cathode reactions and the overall cell reaction occurring in a lead storage battery during its use.

Calculate the potential for half-cell containing 0.01 M K₂Cr₂O₇(aq), 0.01 M Cr³⁺(aq) and 1.0 × 10⁻⁴ M H⁺(aq). The half cell reaction is: Cr₂O₇²⁻(aq) + 14H⁺(aq) + 6e⁻ → 2Cr³⁺(aq) + 7H₂O(l) and the standard electrode potential is given as E° = 1.33 V. [Given : log 10 = 1]