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  • Consider the reaction <img alt="\mathrm{A+B \rightarrow C+D+50\, \mathrm{kcal}}" src="https://entrancecorner.oncodecogs.com/gif.latex?%5Cmathrm%7BA&plus;B%20%5Crightarrow%20C&plus;D&plu

Consider the reaction \mathrm{A+B \rightarrow C+D+50\, \mathrm{kcal}},& the activation energy of the the reaction is \mathrm{80\, \mathrm{kcal}}. What will be the activation Energy for \mathrm{C+D \longrightarrow A+B} is:

Option: 1

130\, \mathrm{kcal}


Option: 2

400\, \mathrm{kcal}


Option: 3

150\, \mathrm{kcal}


Option: 4

30\, \mathrm{kcal}


Answers (1)

best_answer

\mathrm{\Delta H =E_{f}-E_{b} }

\mathrm{-50 =80-E_{b} }

\mathrm{E_{b} =80+50=130 \, \mathrm{kcal} }

Posted by

Gautam harsolia

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