Calculate the change in Gibbs free energy at standard conditions (TSS) an the eq

Question

Calculate the change in Gibbs free energy at standard conditions (TSS) an the equilibrium constant for each of the following reactions. CH_4(g) + H_2 O(g) Equilibrium CO(g) + 3 H_2(g); Delta H degree = +205.9 kJ, Delta S degree = +214.7 J/K Delta G degree kJ K CaCO_3(s) Equilibrium CaO(s) + CO_2(g); Delta H degree = +179.2 kJ, Delta S degree = +160.2 J/K Delta G degree kJ K A reaction has a Delta G degree value of 3.9 kJ/mol. If the reaction quotient for the reaction at 219 degree C is 9.28, what is Delta G for the reaction at 219 degree C? The equation for Delta G is Delta G = Delta G degree + RT in Q. The ideal gas constant, R, is 8.314472 J/mol-K. kJ/mol

Explanation / Answer

8)
a)
delta Go = delta Ho - T*delta So
= 205900 J - 273.15 K* 214.7 J/K
= 147255 J
= 147.3 KJ

to find K use:
delta Go = -R*T*ln K
147255 = -8.314*273.15*ln K
K = 6.91*10^-29

b)
delta Go = delta Ho - T*delta So
= 179200 J - 273.15 K* 160.2 J/K
= 135441 J
= 135.4 KJ

to find K use:
delta Go = -R*T*ln K
135441 = -8.314*273.15*ln K
K = 1.25*10^-26

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