Since, the reaction involves decomposition of one molecule of SO2Cl2, it would follow first order kinetics.
In first order kinetics,
ln[SO2Cl2]t = - k*t + ln[SO2Cl2]0
where
[SO2Cl2]t is the concentration of SO2Cl2 at time t
[SO2Cl2]0 is the concentration of SO2Cl2 at time 0
k is the rate constant
Using the data given, we get
Time (s) | [SO2Cl2], M | ln[SO2Cl2] |
0 | 0.1 | -2.30259 |
100 | 0.0971 | -2.33201 |
200 | 0.0944 | -2.36021 |
300 | 0.0917 | -2.38923 |
400 | 0.089 | -2.41912 |
500 | 0.0865 | -2.44761 |
600 | 0.084 | -2.47694 |
700 | 0.0816 | -2.50593 |
800 | 0.0793 | -2.53452 |
900 | 0.077 | -2.56395 |
1000 | 0.0748 | -2.59294 |
1100 | 0.0727 | -2.62141 |
1200 | 0.0706 | -2.65073 |
1300 | 0.0686 | -2.67946 |
1400 | 0.0666 | -2.70905 |
1500 | 0.0647 | -2.73799 |
Plotting this data, ln[SO2Cl2]t vs t, we get
The slope of the line gives -k.
Therefore
rate constant = 2.9 x 10-4 s-1
b. the rate constant (k) for the reaction Consider the equation for the decomposition of SO2Ch:...