For a reaction, the rate constant is expressed as, k = A ⋅ e − 40000/ T . The energy of the activation is :

k = Ae RT − 4000 By comparing with Arrhenius equation k = Ae R − E a ⇒ R E a = 40000 ⇒ E a = 2 cal × 40000 = 80000 cal

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For a reaction, the rate constant is expressed as, $k = A \cdot e^{- 40000/ T}$ . The energy of the activation is :

Answer:

Solution:

$k = Ae^{\frac{- 4000}{RT}}$

By comparing with Arrhenius equation

$k = Ae^{\frac{- E _{a}}{R}} \Rightarrow \frac{E _{a}}{R} = 40000 \Rightarrow E_{a} = 2 cal \times 40000 = 80000 cal$

Stream:JEESubject:ChemistryTopic:Chemical KineticsSubtopic:Arrhenius Equation

⏱ 2mℹ️ Source: QB

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