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Question

The kinetics of the reaction, 2N2O54NO2+O2, in liquid bromine medium was measured independently for three different initial concentrations of N2O5, which are 0.11, 0.07 and 0.05 mol L1 respectively. The half life of the reaction was found to be 4.5 hours for all these concentrations. The order of the reaction is:

A
0
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B
1
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C
2
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D
Can't be predicted
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Solution

The correct option is B 1
Given,
t12=4.5 h,Initial Concentration of N2O5a1=0.11,a2=0.07,a3=0.05
We know that,
The general formula for half life of nth order reaction is:
t12=2n11k(n1)an10 (Where n is order of reaction and n1)

Half life of zero order reaction,
t12=[a0]2k
t12a0 (a0=Initial Concentration)

Half life of first order reaction,
t12=0.693k
t12 is independent of initial concentration

Half life of second order reaction,
t12=1k[a0]
t12is inversely proportional to a0 (a0=Initial Concentration)

As it can be seen from the given information, three different initial concentration of N2O5 was taken and the half life was the same in each case. As half life is independent of the initial concentration, the reaction is a first order reaction.

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