The slope of the line for the graph of lo g k versus T 1 for the reaction, N 2 O 5 → 2 NO 2 + 2 1 O 2 is -5000 . Calculate the energy of activation of the reaction − ( kJ K − 1 mol − 1 )

Question

The slope of the line for the graph of lo g k versus T 1 ​ for the reaction, N 2 ​ O 5 ​ → 2 NO 2 ​ + 2 1 ​ O 2 ​ is -5000 . Calculate the energy of activation of the reaction − ( kJ K − 1 mol − 1 )

TestHub · Accepted Answer

The decomposition of dinitrogen pentoxide is given by the reaction:

$N_{2} O_{5} ⟶ 2 N O_{2} + \frac{1}{2} O_{2}$

The Arrhenius equation in logarithmic form is:

$lo g k = lo g A - \frac{E _{a}}{2.303 R} \frac{1}{T}$

Given that the plot of $lo g k$ versus $\frac{1}{T}$ has a slope of $\frac{- E _{a}}{2.303 R} = - 5000$ , we can calculate the activation energy $E_{a}$ :

$E_{a} = 2.303 \times \frac{8.314}{1000} \times 5000 K J$

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