∆G° = ∆H° - T∆S° = -19.9×103J/mol - 285.15K×(-55.5J/K.mol) = -4074.175 J/mol
∆G = ∆G° + RT ln K = 0
∆G° = - RT ln K
-4074.175J/mol = - 8.314J/K.mol × 285.15K × ln K
ln K = 1.7185
K = e1.7185 = 5.576
K = 5.58 (Answer)
at a temperature is 8.314 JK 2 For a given reaction, with AH = -19.9 kJ/mol...
2. For a given reaction, with AH° -19.9 kJ/mol and AS = -55.5 J/K mol at a temperature of 12 °C. Calculate the equilibrium constant. The Universal gas constant is 8.314 J.K'mol (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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