Question

Understanding the high-temperature formation and breakdown of the nitrogen oxides is essential for controlling the pollutants generated from power plants and cars. The first-order breakdown of dinitrogen monoxide to its elements has rate constants of 0.76/s at 727°C and 0.87/s at 757°C. What is the activation energy of this reaction?

Answer 1

Understanding the high-temperature formation and breakdown of the nitrogen oxides is essential for controlling the pollutants generated from power plants and cars. The first-order breakdown of dinitrogen monoxide to its elements has rate constants of 0.76/s at 727°C and 0.87/s at 757°C. The activation energy of this reaction would be 3.82 J/mol.

Let's know how,

Given:

k1 = 0.76 s-1      t1 = 727°C = 273 +727 = 1000 K

k2 = 0.87 s-1      t2 = 757o C = 273+757 = 1030 K

E(a) = ?

Now substitute all the values in the above equation,

E(a) = 3.8 103 J/mol.

Thus the activation energy is found to be 3.8103 J/mol .

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