You are given the following half-reactions. AgCl(s) + e Ag(s) + Cl (aq) script E

Question

You are given the following half-reactions. AgCl(s) + e Ag(s) + Cl (aq) script E° = +0.22 V Ag+(aq) + e Ag(s) script E° = +0.80 V Construct a cell with the following cell reaction. AgCl(s) Ag+(aq) + Cl (aq) Please see Adding Reactions for assistance.

(a) What is the standard cell potential? WebAssign will check your answer for the correct number of significant figures. V

(b) What is the value of G° for the reaction? WebAssign will check your answer for the correct number of significant figures. kJ/mol

(c) What is the equilibrium constant as determined from the cell potential? WebAssign will check your answer for the correct number of significant figures.

Explanation / Answer

a) AgCl(s) + e- (aq) ---> Ag(s) + Cl-(aq)        , Eo = 0.22

Ag(s) -------> Ag+(aq) + e-        ,Eo = -0.8

adding above we get   AgCl(s) ---< Ag+(aq) + Cl-(aq) , E = 0.22-0.8 = -0.58

b) dGo = -nFEo = - 1 x 96485 x (-0.58) = 55961 J/mol = 55.96 KJ/mol

where n = number of e- involved per reaction = 1

c) nFEo = RT ln K

1 x 96485 x (-0.58) = 8.314 x 298 ln K

K = 1.55 x 10^ -10

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