The dehydrogenation of butane to trans-but-2-ene has (H( = +116 kJmol (+27.6 kcal/mol) and (S( = +117

Question:

The dehydrogenation of butane to trans-but-2-ene has (H( = +116 kJmol (+27.6 kcal/mol) and (S( = +117 J/kelvin-mol (+28.0 cal/kelvin-mol).
(a) Compute the value of (G( for dehydrogenation at room temperature (25 (C or 298 (K). Is dehydrogenation favored or disfavored?
(b) Compute the value of (G for dehydrogenation at 1000 (C, assuming (S and (H are constant. Is dehydrogenation favored or disfavored?