The standard reaction Gibbs energy of the isomerization of borneol (C10H17OH) to isoborneol in the gas phase at 503 K is +9.4 kJ mol−1. Calculate the reaction Gibbs energy in a mixture consisting of 0.15 mol of borneol and 0.30 mol of isoborneol when the total pressure is 600 Torr.

The decomposition of a generic diatomic element in its standard state is represented by the equation X,(g) – X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.60 kJ · mol- at 2000. K and -63.08 kJ - mol- at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AGf = 4.60 kJ - mol-!. What is K at that temperature? 0.718 K at 2000. K = Incorrect At 3000. K, AGf = -63.08 kJ - mol-. What is K at that temperature? 6.511 K at 3000. K = Incorrect

Suggest how the thermodynamic equilibrium constant and the equilibrium constant expressed in terms of partial pressures may respond differently to changes in pressure and temperature.

The decomposition of a generic diatomic element in its standard state is represented by the equation X₂(g) → X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.71 kJ - mol-¹ at 2000. K and −55.51 kJ · mol-¹ at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG₁ = 4.71 kJ · mol-¹. What is K at that temperature? K at 2000. K= At 3000. K, AGf = −55.51 kJ - mol-¹. What is K at that temperature? K at 3000. K =