Consider the dehydrogenation of ethane to form ethene (ethylene) and hydrogen, latex: \text{c}_2\text{h}_6\rightleftharpo ons\text{c}_2\text{h}_4+\text{h}_2c 2 h 6 ⇌ c 2 h 4 + h 2 the standard enthalpies of formation and the standard entropies at 25 °c and 1 atm are given below, as pulled from oxtoby, gillis, and nachtrieb, principles of modern chemistry, fourth edition; fort worth: saunders, 1999. substance latex: \delta h^\circ_fδ h f ∘ (kj/mol) latex: s^\circs ∘ (j/mol/k) carbon (s, graphite) 5.74 hydrogen (g) 130.57 ethylene (g) 52.26 219.45 ethane (g) −84.68 229.49 assuming your goal is the production of hydrogen and/or ethylene, would it be beneficial to carry out this reaction at high pressure or low pressure, assuming kinetics are not an issue (i. e., that equilibrium is achieved reasonably quickly at any pressure)?