The second-order rate constant can be calculated using the integrated rate law for a second-order reaction:
[Cl]t = [Cl]0 * e^(-kt)
where k is the second-order rate constant.
Substituting the values from the table, we get:
5.6*10^-14 = 8.25*10^-11 * e^(-k*600)
Solving for k, we get:
k = -2.7*10^-3 s^-1
The reaction
Cl(g)+ O3(g) --> ClO(g)+ O2(g)
is the first-order in both reactants. Determine the pseudo-first-order and second-order rate constants for the reaction from the data in the table below if the initial ozone concentration was ..0000000000825 M or 8.25*10^-11 M.
Time [Cl](M)
0...... 5.6*10^-14
100.... 5.27*10^-14
600... 3.89*10^-14
1200... 2.69*10^-14
1850... 1.81*10^-14
The pseudo-first-order rate constant is 6*10^2. But I cant figure out the second order rate constant.
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