Q.

For a reaction, activation energy Ea=0  and the rate constant at 200 K is 1.6×106s-1. The rate constant at 400 K will be [Given that gas constant, R = 8.314 J K–1 mol–1]

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Detailed Solution

From Arrhenius equationlog⁡k400k200=Ea2.303RT2−T1T1T2 Since, given that Ea=0 ∴log⁡k400k200=0=log 1⇒k400k200=1  So, k400=k200  So rate constant at 400K=1.6×106s−1
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