Consider the following Gibbs energies at 25CSubstance deltaG

Consider the following Gibbs energies at 25C
Substance: deltaGf(kJ/mol-1)
Ag+(aq) 77.1
Cr-(aq) -131.2
AgCl(s) -109.8
Br-(aq) -104
AgBr(s) -96.9

(a) Calculate deltaGrxn for the dissolution for AgCl(s)
_ = kJ/mol-1
(b) Calculate the solubility product constant of AgCl.
K=
(c) Calculate deltaGrxn for the dissolution of AgBr(s).
_kJ/mol-1
(d) Calculate teh solubility product constant of AgBr.
K=

Solution

THIS WILL HELP YOU

The formula you use is deltaGrxn = deltaG °rxn + RT*lnQ

T = 298 K
deltaG °rxn = 131.1 kJ = 131100 J
Q = .033 atm
R = 8.314 J/mol*k

Plug into the equation

deltaGrxn = 131100 + 8.314*298*ln(.033)

= 122648.38 J = 122.6 kJ