Consider the two reactions for the production of ethanol:
i. C2H4(g) + H2O(g) → CH3CH2OH(l)
ii. C2H6(g) + H2O(g) → CH3CH2OH (l) + H2 (g)
2007-04-18 06:05:49 · 2 answers · asked by swizzbeatz905 1 in Science & Mathematics ➔ Chemistry
The difference can be worked out by looking at the Gibbs free energy of reaction of ethane and ethene. The reaction that has the lower Gibbs free energy of reaction (i.e the more negative the Gibbs Free energy is) that is less than zero will be the most feasible. The first reaction will be more feasible than the second.
2007-04-18 06:37:35 · answer #1 · answered by The exclamation mark 6 · 0⤊ 0⤋
The difference can be worked out by looking at the enthapies of formation of ethane and ethene. The one that is less negative will give a more negative enthalpy change for that reaction as a whole.
2007-04-18 13:10:55 · answer #2 · answered by Gervald F 7 · 1⤊ 1⤋