Consider the cell Pt | H2(g) | HCl(aq) | AgCl(s) | Ag for which the cell reaction is 2 AgCl(s) + H2(g) ā 2 Ag(s) + 2 HCl(aq). At 25Ā°C and a molality of HCl of 0.010 mol kg^-1, E = +0.4658 V.
(a) Write the Nernst equation for the cell reaction.
(b) Calculate ĪrG for the cell reaction.
(c) Assuming that the Debye-HĆ¼ckel limiting law holds at this concentration, calculate EĀ°(AgCl, Ag).
Calculate the equilibrium constants for the following reactions at 25Ā°C from standard potential data:
(a) Sn(s) + CuSO4(aq) ā Cu(s) + SnSO4(aq)
(b) Cu2+(aq) + Cu(s) ā 2 Cu+(aq)
The emf of the cell Bi | Bi2S3(s) | Bi2S3(aq) | Bi is +0.96 V at 25Ā°C. Calculate:
(a) the solubility product of Bi2S3 and
(b) its solubility.