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?
1 answer:
Answer:
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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