4. Consider the following reaction: NO2(g) à NO(g) + O(g)
The concentration of NO2 was monitored at a fixed temperature as a function of time during the decomposition reaction and the data is tabulated below:
Time (s) |
[NO2] (M) |
Time (s) |
[NO2] (M) |
Time (s) |
[NO2] (M) |
Time (s) |
[NO2] (M) |
0 |
0.0100 |
250 |
0.00611 |
550 |
0.00416 |
800 |
0.00329 |
50 |
0.00887 |
300 |
0.00567 |
600 |
0.00395 |
850 |
0.00316 |
100 |
0.00797 |
350 |
0.00528 |
650 |
0.00376 |
900 |
0.00303 |
150 |
0.00723 |
400 |
0.00495 |
700 |
0.00359 |
950 |
0.00292 |
200 |
0.00662 |
450 |
0.00466 |
750 |
0.00343 |
1000 |
0.00282 |
Part a.
The plot of ln[NO2] versus time can be drawn as follows.
Part b.
Equation of the line: ln[NO2] = -0.00121*t + (-4.75302)
Compare the above equation with ln[NO2] = -kt + ln[NO2]0
i.e. The rate constant (k) = 0.00121 s-1 = 1.21*10-3 s-1
Part c.
If t = 2000 s, ln[NO2] = -0.00121*2000 + (-4.75302)
ln[NO2] = -2.42 + (-4.75302) = -7.17302
i.e. [NO2] = 0.000767 M
Part d.
At t = 0, [NO2]0 remains as such.
For a first-order reaction, the half-life period (t1/2) is independent of the initial concentration.
i.e. t1/2 = ln(2)/k = 0.693/0.00121 = 572.85 s ~ 573 s
4. Consider the following reaction: NO2(g) à NO(g) + O(g) The concentration of NO2 was monitored...
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