JEE Mains · Chemistry · STD 12 - 3. Chemical kinetics
Consider the following plots of rate constant versus \(\frac{1}{\mathrm{T}}\) for four different reactions. Which of the following orders is correct for the activation energies of these reactions?
- A \(E_{\mathrm{b}}>E_{\mathrm{d}}>E_{\mathrm{c}}>E_{\mathrm{a}}\)
- B \(E_{\mathrm{a}}>E_{\mathrm{c}}>E_{\mathrm{d}}>E_{\mathrm{b}}\)
- C \(E_{\mathrm{c}}>E_{\mathrm{a}}>E_{\mathrm{d}}>E_{\mathrm{b}}\)
- D \(E_{\mathrm{b}}>E_{\mathrm{a}}>E_{\mathrm{d}}>E_{\mathrm{c}}\)
Answer & Solution
Correct Answer
(C) \(E_{\mathrm{c}}>E_{\mathrm{a}}>E_{\mathrm{d}}>E_{\mathrm{b}}\)
Step-by-step Solution
Detailed explanation
\(\log \mathrm{K}=\frac{-\mathrm{Ea}}{2.303 \mathrm{RT}}+\log \mathrm{A}\) Acrroding to Arrhenius equation plot of \(\operatorname{log } \mathrm { K }\) Vs. \(\frac{1}{\mathrm{T}}\) is linear with. slope \(=\frac{-\mathrm{Ea}}{2.303 \mathrm{R}}\) From plot we conclude: \(|\)…
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