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given this electrochemical cell: Tl(s) | Tl*(aq, 0.50 mol L-1) || H*(aq, x mol L-2) | H2(g, 1 atm) | Pt(s)

Concentration of H+ is unknown, Pressure of H2 is constant at 1 atm. Initial cell voltage is 0.139V, with the Pt | H2 | H+ half-cell acting as the cathode.

a) write out the oxidization and reduction half reactions, and the overall chemical reaction occurring, and find the initial pH in the H+ | H2 | Pt cell

b) What is the equilibrium constant of the reaction happening in the cell?

Half-reaction F2(g) + 2e- → 2 F-(aq) Au*(aq) + e- → Au(s) MnO4 (aq) + 8 H*(aq) + 5 e → Mn2+(aq) + 4H2O(1) BrO3-(aq) + 12 H+ (

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