Given,
temperature =200 K
Gibbs free energy change (G) = 27.8 kJ/mol = 27800 J/mol
ideal gas constant = 8.314 J/mol
relation between gibbs free energy change and equillibrium(K) constant is given as
G = -RT ln K
27800 = - 8.314x200 lnK
ln K = - 16.71
taking antiln both sides
K= 5.62 x 10-8
Determine K for a reaction at 200 Kif AG° = 27.8 kJ/mol. (R = 8.314 J/mol...
Determine K for a reaction at 200 K if AG° = 12.9 kJ/mol. (R = 8.314 J/mol · K)
AG°= AH-TAS AG=AGº+RTinQ where R=8.314 J/mol K 1. Calculate AGº for the following reaction at 25 °C if AH°= -1854 kJ/mol; AS°= -236 J/mol K CH-COCH3(g) + 402(g) → 3C02(g) + 3H2O(1) 2. NH.NO, dissolving in water is a spontaneous process. As it dissolves, the temperature of the solution decreases. Based on this, what must the signs (positive or negative) of AG, AH, and AS be?
Determine AGⓇ for a reaction when AG = -184.7 kJ/mol and Q = 0.043 at 298 K. (R = 8.314 J/mol K)
Determine Gº for a reaction when AG = -119.1 kJ/mol and Q = 0.043 at 298 K. (R = 8.314 J/mol · K)
For a particular reaction at 212.3 °C, AG = -889.99 kJ/mol, and AS = 385.90 J/(mol · K). Calculate AG for this reaction at -2.8 °C. AG= 193.97 kJ/mol
For a particular reaction, AH = -14.20 kJ/mol and AS = -198.5 J/(mol.K). Calculate AG for this reaction at 298 K. AG = 73.35 kJ/mol
For a particular reaction at 203.3 °C, AG = 424.99 kJ/mol, and AS - 551.38 J/mol K). Calculate AG for this reaction at -66.6 °C. AG = kJ/mol What is the value of K for this aqueous reaction at 298 K? A + B =C+D AG° = 11.80 kJ/mol
What is the value of Keq if ∆Gº=15.6 kJ (R=8.314 J/mol-K)? 1.84x10-3 0.994 1.01 5.05x10-7
For a particular reaction at 239.1 °C, AG = 363.40 kJ/mol, and AS = 739.34 J/mol. K). Calculate AG for this reaction at -19.0 °C. AGE 554.22 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)