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Question

In the thermal decomposition of N2O at 830 K, the time required to decompose half of the reactant was 263 sec at the initial pressure 290 mm. It takes 212 sec to decompose half of the reactant if initial pressure was 360 mm. What is the order of the reaction? Also calculate t1/2 for N2O decomposition if initial pressure of N2O is 1 atm.

A
O.R=2, Half life =100.2sec
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B
O.R=1, Half life =10.02sec
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C
O.R=4, Half life =1.002sec
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D
None of these
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Solution

The correct option is C O.R=2, Half life =100.2sec
t1/2,1t1/2,2=263212=1.24
P2P1=360290=1.24
Thus t1/2,1t1/2,2=P2P1
t1/21Pi
Thus, the half life period is inversely proportional to the initial pressure. This is characteristic of second order reaction.
t1/2,263=290760 (because 1 atm = 760 mm Hg)

t1/2=100.2sec

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