Question
Nitrogen pentoxide decomposes according to equation: 2N2O5(g)---> 4NO2(g) + O2(g)
This first order reaction was allowed to proceed at 40° C and the data below were collected:
|
[N2O5] (M) |
Time (min) |
|
0.400 |
0.00 |
|
0.289 |
20.0 |
|
0.209 |
40.0 |
|
0.151 |
60.0 |
|
0.109 |
80.0 |
(a) Calculate the rate constant. Include units with your answer.
(b) What will be the concentration of N2O5 after 100 minutes?
(c) Calculate the initial rate of reaction.
Solution
(a) The plot of [N2O5] v/s t is as follows
|
[N2O5] (M) |
Time (min) |
log (N2O5] |
|
0.400 |
0.00 |
-0.3979 |
|
0.289 |
20.0 |
-0.5391 |
|
0.209 |
40.0 |
-0.6798 |
|
0.151 |
60.0 |
-0.8210 |
|
0.109 |
80.0 |
-0.9625 |
From the plot, log [N2O5] v/s t, we obtain by
