The standard reaction Gibbs energy of the isomerization of borneol (C10H17OH) to isoborneol in the gas phase at 503K is +9.4 kJ mol². 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.

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 initial concentrations or pressures of reactants and products are given for each of the following systems. Calculate the reaction quotient and determine the direction in which each system will proceed to reach equilibrium. (The system is considered in equilibrium if Kc and Qc are within 5% of each other.) (a) 2 NH3(g) equalibrium arrow N2(g) + 3 H2(g),   [NH3]i = 0.400 M, [N2]i = 0.155 M, [H2]i = 0.110 M, Kc = 16 What is the reaction quotient?   What direction will the reaction shift to?     (b) 2 NH3(g) equalibrium arrow N2(g) + 3 H2(g),  Pi(NH3) = 2.10 atm, Pi(N2) = 10.70 atm, Pi(H2) = 10.70 atm, Kp = 8.3 ✕ 104 What is the reaction quotient?   What direction will the reaction shift to?      (c) 2 SO3(g) equalibrium arrow 2 SO2(g) + O2(g),    [SO3]i = 1.90 M, [SO2]i = 1.90 M, [O2]i = 1.90 M, Kc = 0.23 What is the reaction quotient?   What direction will the reaction shift to?     (d) 2 SO3(g) equalibrium arrow 2 SO2(g) + O2(g),  Pi(SO3) = 0.100 atm, Pi(SO2) =…

7. The vapor pressure of benzene between 10 °C and 30 °C fits the expression 1780 K log()= 7.960- T where T is in K. Calculate (a) the enthalpy of vaporization (Avap H) and (b) the normal boiling point of benzene.