the-dehydrogenation-of-ethane-ch3-ch3-to-ethene-ch2-ch2-has-h-136-kj-mol-32-5-kc

Question

The dehydrogenation of ethane (CH₃−CH₃) to ethene (CH₂=CH₂) has ΔH° = +136 kJ/mol (+32.5 kcal/mol) and ΔS° = +120 J/kelvin-mol (+28.7 cal/kelvin-mol). Calculate the value of ΔG° for the reaction at room temperature. Is the reaction favored or disfavored?

Accepted Answer

∆Gº = +100 kJ/mol (+23.9 kcal/mol)
The reaction is disfavored.

Answer

∆Gº = +36 kJ/mol (+8.6 kcal/mol)
The reaction is favored.

Answer

∆Gº = +136 kJ/mol (+32.5 kcal/mol)
The reaction is favored.

Answer

∆Gº = +156 kJ/mol (+37.3 kcal/mol)
The reaction is disfavored.

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The dehydrogenation of ethane (CH₃−CH₃) to ethene (CH₂=CH₂) has ΔH° = +136 kJ/mol (+32.5 kcal/mol) and ΔS° = +120 J/kelvin-mol (+28.7 cal/kelvin-mol). Calculate the value of ΔG° for the reaction at room temperature. Is the reaction favored or disfavored?

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Biology

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The dehydrogenation of ethane (CH3−CH3) to ethene (CH2=CH2) has ΔH° = +136 kJ/mol (+32.5 kcal/mol) and ΔS° = +120 J/kelvin-mol (+28.7 cal/kelvin-mol). Calculate the value of ΔG° for the reaction at room temperature. Is the reaction favored or disfavored?

The dehydrogenation of ethane (CH₃−CH₃) to ethene (CH₂=CH₂) has ΔH° = +136 kJ/mol (+32.5 kcal/mol) and ΔS° = +120 J/kelvin-mol (+28.7 cal/kelvin-mol). Calculate the value of ΔG° for the reaction at room temperature. Is the reaction favored or disfavored?