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The Solubility Constant for AgI(s) at 25 degrees Celsius is 8.3*10^-17
how do i find [tex]\Delta[/tex]G(rxn) for [Ag+]=9.1*10^-9 & [I-]=9.1*10^-9
Using the equation:
ΔG=ΔGº+RTln(Q)
Let K=Our solubility constant:
0=ΔGº+RTlnK
ΔGº=-RTlnK
Now,
ΔG=-RTlnK+RTlnQ
ΔG=RTlnQ-RTlnK
ΔG=RT(ln(Q/K))
ΔG=-5.67KJ/mol
The answer in my practice exam claims to be 91.7kJ/mol.
Where did I go wrong?
Thanks!
how do i find [tex]\Delta[/tex]G(rxn) for [Ag+]=9.1*10^-9 & [I-]=9.1*10^-9
Using the equation:
ΔG=ΔGº+RTln(Q)
Let K=Our solubility constant:
0=ΔGº+RTlnK
ΔGº=-RTlnK
Now,
ΔG=-RTlnK+RTlnQ
ΔG=RTlnQ-RTlnK
ΔG=RT(ln(Q/K))
ΔG=-5.67KJ/mol
The answer in my practice exam claims to be 91.7kJ/mol.
Where did I go wrong?
Thanks!