Question

b. the rate constant (k) for the reaction Consider the equation for the decomposition of SO2Ch: 2. SO2CI2(8) S2(8)+ Cl2(8) Th
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Answer #1

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

Time, s in 500 1000 1500 2000 Le w In[A] = -0.00029*time - 2.30262 R? = 1.00000 Series1 in u In(SO2Cl2] Linear (Series1) u Ou

The slope of the line gives -k.

Therefore

rate constant = 2.9 x 10-4 s-1

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