Fo the given reaction,
(a) dGo = -RTlnK
          Â
= -RT ln([H]/[F][G])
          Â
= -8.314 x 298 ln(9/2 x
3)Â Â Â Â Â Â Â Â Â Â Â
          Â
= -1.003 kJ/mol
(b) when [F] = 4 mM
dGo = -RTlnK
          Â
= -RT ln([H]/[F][G])
          Â
= -8.314 x 298 ln(9/4 x
3)Â Â Â Â Â Â Â Â Â Â Â
          Â
= 743.27 kJ/mol
(c) when [H] = 18 mM
dGo = -RTlnK
          Â
= -RT ln([H]/[F][G])
          Â
= -8.314 x 298 ln(18/2 x
3)Â Â Â Â Â Â Â Â Â Â Â
          Â
= -2.72 kJ/mol
(d) Yes, this violates the LeChatellier's principle, according
to which when the concentration at one end increase the
concentration at other end would increase accordingly.
