3. Write the reaction quotient, Qc, for each of the following reactions:  (a) CH4(g) + CO2(g) ↔ CO(g) + H2(g)  (b) H2S(g) + SO2(g) ↔ S(s) + H2O(g)  (c) HCN(aq) +NaOH(aq) ↔ NaCN(aq) + H2O(l)

A reaction has a standard free-energy change of -13.10 kJ mol-¹(-3.131 kcal mol-¹). Calculate the equilibrium constant for the reaction at 25 °C. Keq =

What is the standard enthalpy (in kJ/mol) of a reaction for which the equilibrium constant increased by a factor of 4.0 when the temperature is increased by 34 K starting from 333 K.

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 5.51 kJ · mol-! at 2000. K and –57.84 kJ · mol- at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AGf = 5.51 kJ · mol-. What is K at that temperature? K at 2000. K = At 3000. K, AGf = -57.84 kJ · mol-1. What is K at that temperature? K at 3000. K =