The reaction F + G = H is at equilibrium, under standard conditions. (a) Calculate âˆ†Goâ€™ if...

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The reaction F + G = H is at equilibrium, under standardconditions.
(a) Calculate âˆ†Goâ€™ if [F] = 2mM, [G] = 3 mM, and [H] = 9 mM
(b) What happens to âˆ†Goâ€™ if the solution is at equilibrium attwice this concentration of F?
(c) What happens to âˆ†Goâ€™ if the solution is at equilibrium attwice this concentration of H?
(d) Does this violate LeChatelierâ€™s Principle?

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4.4 Ratings (946 Votes)

Fo the given reaction,

(a) dGo = -RTlnK

Â Â Â Â Â Â Â Â Â Â Â = -RT ln([H]/[F][G])

Â Â Â Â Â Â Â Â Â Â Â = -8.314 x 298 ln(9/2 x 3)Â Â Â Â Â Â Â Â Â Â Â

Â Â Â Â Â Â Â Â Â Â Â = -1.003 kJ/mol

(b) when [F] = 4 mM

dGo = -RTlnK

Â Â Â Â Â Â Â Â Â Â Â = -RT ln([H]/[F][G])

Â Â Â Â Â Â Â Â Â Â Â = -8.314 x 298 ln(9/4 x 3)Â Â Â Â Â Â Â Â Â Â Â

Â Â Â Â Â Â Â Â Â Â Â = 743.27 kJ/mol

dGo = -RTlnK

Â Â Â Â Â Â Â Â Â Â Â = -RT ln([H]/[F][G])

Â Â Â Â Â Â Â Â Â Â Â = -8.314 x 298 ln(18/2 x 3)Â Â Â Â Â Â Â Â Â Â 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.

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The reaction F + G = H is at equilibrium, under standard conditions. (a) Calculate âˆ†Goâ€™ if...

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