show that the decomposition of n2o gas on gold follows first order kinetics.
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Explanation:
(a) Using first order kinetic equation and substituting given values,
In firs case: k=
53
2.303
log
10
200−100
200
=0.0131min
−1
In second case: k=
100
2.303
log
10
200−146
200
=0.0131min
−1
As the values of k come out to be the same in both cases, teh reaction is of first order.
(b) As in the first order reaction, the time required for the completion of same fraction is independent of initial concentration; the percentage decomposition in 100 minutes when the initial pressure is 600 mm will also be 73%.
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