2
Question
The reaction, 2N2O5→4NO2+O2, was studied and the following data were collected:
Expt.
No. [N2O5]
(molL−1) Rate of disappearance of
N2O5
(molL−1min−1) 1. 1.13×10−2 34×10−5 2. 0.84×10−2 25×10−5 3. 0.62×10−2 18×10−5
Determine (i) order the reaction, (ii) the rate law, and (iii) rate constant for the reaction.
| Expt. No. | [N2O5] (molL−1) | Rate of disappearance of N2O5 (molL−1min−1) |
| 1. | 1.13×10−2 | 34×10−5 |
| 2. | 0.84×10−2 | 25×10−5 |
| 3. | 0.62×10−2 | 18×10−5 |
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Solution
Let the rate law for the reaction be
Rate =k[N2O5]x
34×10−5=k[1.13×10−2]x
25×10−5=k[0.84×10−2]x
or 34×10−525×10−5=[1.13×10−2]x[0.84×10−2]x
1.36=[1.345]x
x=1
Order of the reaction is 1. Rate law =k[N2O5]
k=Rate[N2O5]=34×10−51.13×10−2=30.08×10−3min−1
Rate =k[N2O5]x
34×10−5=k[1.13×10−2]x
25×10−5=k[0.84×10−2]x
or 34×10−525×10−5=[1.13×10−2]x[0.84×10−2]x
1.36=[1.345]x
x=1
Order of the reaction is 1. Rate law =k[N2O5]
k=Rate[N2O5]=34×10−51.13×10−2=30.08×10−3min−1
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