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Question

The catalytic decomposition of N2O(g) by gold at 900C and at an initial pressure of 200 mm is 50% complete in 53 minutes and 73% complete in 100 minutes.
(i) What is the order of the reaction?
(ii)Calculate the velocity constant.
(iii) How much of N2O(g) will decompose in 100 min. at the same temperature but at initial pressure of 600 mm?

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Solution

Let [Ao]=100
Then [At]=10050=50 at 53 min
[At]=10073=27 at 100 min
(i) & (ii)
k=2.303tlog[Ao][At]
k53=2.30353log10050=0.013min1
k100=2.303100log10027=0.013min1
k values indicate the order of reaction is 1 .
(iii) For 1st order the time required to complete any fraction is independent of [Ao]
73 % of N2O will decompose when [Ao]=600mm which corresponds to a pressure of 600100mm=438mm

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