The activation energy (E*) for 2N2O ---> 2N2 + O2 is 250 KJ. If the k for this reaction is 0.380/M at 1001oK, what will k be at 298oK? What will the half-life be at both temperatures?

Explanation:

GIven that:

The activation energy = 250 kJ

k₁ = 0.380 /M

k₂ = ???

Initial temperature 1001 K

Final temperature 298 K

Applying the equation of Arrhenius theory.

where ;

R gas constant = 8.314  J/K/mol

 /M .sec

Half life:

At 1001 K.

1.82368 secc

At 298 K:

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