Answer:
a. Second order
b. First order
c. zero order
Explanation:
a. For a second order reaction,
![t_{1/2}=\frac{1}{k[A_0]}](https://tex.z-dn.net/?f=t_%7B1%2F2%7D%3D%5Cfrac%7B1%7D%7Bk%5BA_0%5D%7D)
As half life is inversely proportional to initial concentration, therefore, increase in intital concentration will decrease half life of the reaction.
b. First order reaction,
for first order reaction:
![k=\frac{1}{t} ln\frac{[A_0]}{[A]}](https://tex.z-dn.net/?f=k%3D%5Cfrac%7B1%7D%7Bt%7D%20ln%5Cfrac%7B%5BA_0%5D%7D%7B%5BA%5D%7D)
![kt=ln[A_0]-ln[A]\\ln[A]=ln[A_0]-kt](https://tex.z-dn.net/?f=kt%3Dln%5BA_0%5D-ln%5BA%5D%5C%5Cln%5BA%5D%3Dln%5BA_0%5D-kt)
y = C + mx
Therefore, plot between ln A and t is a straight line.
c. For a zero order reaction,
![t_{1/2}=\frac{[A_0]}{2k}](https://tex.z-dn.net/?f=t_%7B1%2F2%7D%3D%5Cfrac%7B%5BA_0%5D%7D%7B2k%7D)
Half life is proportional to initial concentration, therefore, increase in initial concentration will increase half life of the reaction.