Question

a) Calculate the equilibrium constant at 17 K for a reaction with ΔHrxno = 10 kJ and ΔSrxno = -100 J/K. (Don't round until the end. Using the exponent enlarges any round-off error.)

b) Calculate the equilibrium constant at 146 K for the thermodynamic data in the previous question (Notice that Keq is larger at the larger temperature for an endothermic reaction)

c) Calculate the equilibrium constant at 43 K for a reaction with ΔH_rxn^o = 10 kJ and ΔS_rxn^o = 100 J/K.

d) Calculate the equilibrium constant at 145 K for the thermodynamic data in the previous question.

(Notice that K_eq is dramatically larger for a larger temperature when there is a substantial positive increase in entropy.)

e) Using data from the Appendix, calculate ΔG^o (in kJ) at 65^oC for the reaction:

N₂O(1 atm) + H₂(1 atm) ↔ N₂(1 atm) +H₂O(l) (Recall, all gases at 1 atm for standard conditions)

f)Calculate ΔG (in kJ) at 65 ^oC for the reaction:

N₂O(0.0061 atm) + H₂(0.25 atm) ↔ N₂(445.4 atm) +H₂O(l)

Answer 1