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+1 vote
69.1k views
in Chemistry by (61.9k points)

Following data are obtained for the reaction:

N2O5 → 2NO2 + 1/2 O2

t/s 0 300 600
[N2O5]/mol L-1 1.6 x 10-2 0.8 x 10-2 0.4 x 10-4

(i) Show that it follows first order reaction.

(ii) Calculate the half-life.

(Given : log 2 = 0.3010 log 4 = 0.6021)

1 Answer

+1 vote
by (34.7k points)
selected by
 
Best answer

k is constant when using first order equation therefore it follows first order kinetics.

OR

In equal time interval, half of the reactant gets converted into product and the rate of reaction is independent of concentration of reactant, so it is a first order reaction.

(ii) t1/2 = 0.693/k

= 0.693/2.31 x 10-3 

= 300 s

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