Solution Found!
The dehydrogenation of butane to trans-but-2-ene has H = +116 kJ>mol (+27.6 kcal> mol)
Chapter 7, Problem PROBLEM 7-36(choose chapter or problem)
The dehydrogenation of butane to trans-but-2-ene has \(\Delta H^{\circ}=+116\ kJ/mol\ (+27.6\ kcal/mol)\) and \(\Delta S^{\circ}=+117\ J/kelvin-mol\ (+28.0\ cal/kelvin-mol)\).
(a) Compute the value of \(\Delta G^{\circ}\) for dehydrogenation at room temperature (\(25^{\circ}C\ \text{or}\ 298^{\circ}K\)). Is dehydrogenation favored or disfavored?
(b) Compute the value of \(\Delta G\) for dehydrogenation at \(1000^{\circ}C\), assuming that \(\Delta S\) and \(\Delta H\) are constant. Is dehydrogenation favored or disfavored?
Questions & Answers
QUESTION:
The dehydrogenation of butane to trans-but-2-ene has \(\Delta H^{\circ}=+116\ kJ/mol\ (+27.6\ kcal/mol)\) and \(\Delta S^{\circ}=+117\ J/kelvin-mol\ (+28.0\ cal/kelvin-mol)\).
(a) Compute the value of \(\Delta G^{\circ}\) for dehydrogenation at room temperature (\(25^{\circ}C\ \text{or}\ 298^{\circ}K\)). Is dehydrogenation favored or disfavored?
(b) Compute the value of \(\Delta G\) for dehydrogenation at \(1000^{\circ}C\), assuming that \(\Delta S\) and \(\Delta H\) are constant. Is dehydrogenation favored or disfavored?
ANSWER:Step 1 of 3
Given,
