For the second-order reaction$ \mathrm{NO}(g)+\mathrm{F}_{2}(g) \rightarrow \mathrm{NOF}(g)+\mathrm{F}(g) $ the value of the rate constant increases from 4.72 *10⁷ M ^-1s^-1 at 298 K to 1.21* 10⁸ M^-1s^-1 at 473 K.Estimate the activation energy of the reaction.

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The Answer of For the second-order reaction$ \mathrm{NO}(g)+\mathrm{F}_{2}(g) \rightarrow \mathrm{NOF}(g)+\mathrm{F}(g) $ the value of the rate constant increases from 4.72 *10⁷ M ^-1s^-1 at 298 K to 1.21* 10⁸ M^-1s^-1 at 473 K.Estimate the activation energy of the reaction.

For the Second-Order Reaction NO(g)+F2(g)→NOF(g)+F(g) \mathrm{NO}(g)+\mathrm{F}_{2}(g) \rightarrow \mathrm{NOF}(g)+\mathrm{F}(g) NO(g)+F2​(g)→NOF(g)+F(g) The Value of the Rate Constant Increases from 4

For the Second-Order Reaction $\mathrm{NO}(g)+\mathrm{F}_{2}(g) \rightarrow \mathrm{NOF}(g)+\mathrm{F}(g)$ The Value of the Rate Constant Increases from 4