Temperature = T = 12°C = 273 + 12 = 285 K
Delta H° = -19.9 KJ = -19.9*1000 = -19900 J
We know that,
Delta G° = Delta H° - T * Delta S°
Delta G° = -19900 - (285)*(-55.5) = -4082.5 J
Let Kc is equilibrium constant. Then,
Delta G° = - R * T * ln Kc
-4082.5 = - 8.314 * 285 * ln Kc
ln Kc = 1.723
Kc = e^(1.723) = 5.6 ...Answer
Let me know if any doubts.
2. For a given reaction, with AH° -19.9 kJ/mol and AS = -55.5 J/K mol at...
at a temperature is 8.314 JK 2 For a given reaction, with AH = -19.9 kJ/mol and AS = -55.5 J K mol at a 12. Calculate the equilibrium constant. The Universal gas constant is 82 (25 points)
For a given reaction, Delta H = -19.9 kJ/mol and Delta S = -55.5 J/K-mol. Calculate the temperature in K where Delta G = 0. Assume that Delta H and Delta S do not vary with temperature. Also, what is the equilibrium constant at that temperature?
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