wiz-icon
MyQuestionIcon
MyQuestionIcon
1
You visited us 1 times! Enjoying our articles? Unlock Full Access!
Question

Catalytic decomposition of nitrous oxide by gold at 900C at an initial pressure of 200 mm was 50% in 53 minutes and 73% in 100 minutes. Find the order of the reaction. How much will it decompose in 100 minutes at the same temperature but at an initial pressure of 600 mm?

Open in App
Solution

We have K=2.303tlog( (1)cfracaax)
Case (1) a=100,ax(at t=53min)=10050=50 & at 100min it is (10073)=27
K=2.30353log10050=2.30353log2=0.013min1
Case (2) At t=100min
K=2.303100log10027=0.013min1
Since the value of K is constant, the order of reaction is 1.
For a first order reaction, the time required to complete any fraction is independent of initial concentration.
73% of N2O will decompose when initial concentration is 600mm, corresponds to a pressure of 600100=438mm

flag
Suggest Corrections
thumbs-up
0
Join BYJU'S Learning Program
similar_icon
Related Videos
thumbnail
lock
Order and Molecularity of Reaction
CHEMISTRY
Watch in App
Join BYJU'S Learning Program
CrossIcon