The value of G° is related to the equilibrium constant, K, by the expression: Wh
ID: 694425 • Letter: T
Question
The value of G° is related to the equilibrium constant, K, by the expression: What is G° for the following reaction at 298 K? H° = 92.4 kJ AS 198 JIK 2 NH3 (g)N2 (g) + 3 H2 (g) a) Under standard conditions (1 atm of NHs, N2 and H2) and at 298 K, what will be formed? b) Calculate the equilibrium constant for this reaction at 298 K. c) Calculate the equilibrium temperature for this standard reaction. Will product or reactant be formed above this temperature? 7. For the reaction CO (g) + 2 H2O (g) CO2 (g) + H2 (g) at 770 K, Keq-510. Calculate the AGo for the reaction at 770 K.Explanation / Answer
for the reaction 2NH3(g)--------->N2(g)+ 3H2(g) , deltaG= deltaH-T*deltaS =92.4 KJ-298*198/1000 Kj=33.4
since deltaG is +ve, the reaction is reactant favored.
Equilibrium constant (K) and deltaG are related as deltaG=-RT lnK
lnK= -deltaG/RT= -33.4*1000/(8.314*298), K= 1.39*10-6
At equilibrium, deltaG= 0 or deltaH= T*deltaS
T= deltaH/deltaS= 92.4*1000/198=467 K
above this temperature, deltaG is- ve, so product favored.
4. for the reaction given deltaG=-RT lnK= -8.314*770*ln(5.1)= -10430 J/mole= -10.430 Kj/mole
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