Answer :
The order of reaction is, 0 (zero order reaction).
The value of rate constant is, ![0.00388Ms^{-1}](https://tex.z-dn.net/?f=0.00388Ms%5E%7B-1%7D)
Explanation :
Half life : It is defined as the time in which the concentration of a reactant is reduced to half of its original value.
The general expression of half-life for nth order is:
![t_{1/2}\propto \frac{1}{[A_o]^{n-1}}](https://tex.z-dn.net/?f=t_%7B1%2F2%7D%5Cpropto%20%5Cfrac%7B1%7D%7B%5BA_o%5D%5E%7Bn-1%7D%7D)
or,
![\frac{t_{1/2}_1}{t_{1/2}_2}=\frac{[A_2]^{n-1}}{[A_1]^{n-1}}](https://tex.z-dn.net/?f=%5Cfrac%7Bt_%7B1%2F2%7D_1%7D%7Bt_%7B1%2F2%7D_2%7D%3D%5Cfrac%7B%5BA_2%5D%5E%7Bn-1%7D%7D%7B%5BA_1%5D%5E%7Bn-1%7D%7D)
or,
.............(1)
where,
= half-life of the reaction
n = order of reaction
[A] = concentration
As we are given:
Initial concentration of A = 0.229 M
Final concentration of A = 0.639 M
Initial half-life of the reaction = 29.5 s
Final half-life of the reaction = 82.3 s
Now put all the given values in the above formula 1, we get:
![n=\left (\frac{\log \frac{29.5}{82.3}}{\log\frac{0.639}{0.229}}\right )+1](https://tex.z-dn.net/?f=n%3D%5Cleft%20%28%5Cfrac%7B%5Clog%20%5Cfrac%7B29.5%7D%7B82.3%7D%7D%7B%5Clog%5Cfrac%7B0.639%7D%7B0.229%7D%7D%5Cright%20%29%2B1)
![n=0.000196\approx 0](https://tex.z-dn.net/?f=n%3D0.000196%5Capprox%200)
Thus, the order of reaction is, 0 (zero order reaction).
Now we have to determine the rate constant.
To calculate the rate constant for zero order the expression will be:
![t_{1/2}=\frac{[A_o]}{2k}](https://tex.z-dn.net/?f=t_%7B1%2F2%7D%3D%5Cfrac%7B%5BA_o%5D%7D%7B2k%7D)
When,
= 29.5 s
= 0.229 M
![29.5s=\frac{0.229M}{2k}](https://tex.z-dn.net/?f=29.5s%3D%5Cfrac%7B0.229M%7D%7B2k%7D)
![k=0.00388Ms^{-1}](https://tex.z-dn.net/?f=k%3D0.00388Ms%5E%7B-1%7D)
Thus, the value of rate constant is, ![0.00388Ms^{-1}](https://tex.z-dn.net/?f=0.00388Ms%5E%7B-1%7D)