An exothermic reaction X- Y has an activation energy 30 kJ-mol- If energy change - E during the reaction is -20 kJ-mol- the activation energy for the reverse reaction in kJ-mol is -

Δ H = E_a,f E_a,b nbsp;= 20 20=30 – E_a,b E_a,b nbsp; = 50 kJ/mol ...

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Standard XII

Chemistry

Collision Theory

An exothermic...

Question

An exothermic reaction $X \to Y$ has an activation energy $30 k J / m o l$ . If energy change $Δ E$ during the reaction is $- 20 k J / m o l,$ the activation energy for the reverse reaction in $k J / m o l$ is ______.

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Solution

$Δ H = E_{a, f} - E_{a, b} = - 20 - 20 = 30 - E_{a, b} E_{a, b} = 50 k J / m o l$

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An exothermic reaction X→Y has an activation energy 30 kJ/mol. If energy change ΔE during the reaction is −20 kJ/mol, the activation energy for the reverse reaction in kJ/mol is ______.

ΔH=Ea,f−Ea,b=−20−20=30–Ea,bEa,b=50 kJ/mol

An exothermic reaction $X \to Y$ has an activation energy $30 k J / m o l$ . If energy change $Δ E$ during the reaction is $- 20 k J / m o l,$ the activation energy for the reverse reaction in $k J / m o l$ is ______.

$Δ H = E_{a, f} - E_{a, b} = - 20 - 20 = 30 - E_{a, b} E_{a, b} = 50 k J / m o l$