The motivational example demonstrated that the reaction: 

C₂ H₆  (g) ↔ C₂ H₄  (g) + H₂  (g) 

strongly favors the reactant ethane at equilibrium—so strongly that the amount of product is barely measurable. But this reaction was only examined at T = 25°C.

A. Plot the equilibrium constant for this reaction, as a function of temperature, from T = 25°C to T = 750°C. Use the assumption that DHT 0 is constant. 

B. Repeat part A using the rigorous approach of accounting for ΔH_T⁰ . How do the plots compare? What can you learn from this comparison? 

C. The motivational example involved a reactor that initially contained 1 mole of ethane and 0.5 moles each of ethylene and hydrogen. Find the contents of the reactor, at equilibrium, for temperatures of 250°C, 500°C, and 750°C. In each case the pressure is 1 bar.