Answer: 1.
![Rate=k[A]^1[B]^2](https://img.qammunity.org/2019/formulas/chemistry/middle-school/p62kppgacrxyuoudilcfxk3a2t2veytrfd.png)
2.
![Rate=k[X]^2[y]^1](https://img.qammunity.org/2019/formulas/chemistry/college/xj6pvkpcf53jdhxvys39x9n8q471tiaqzq.png)
x= 2 , y= 1 Total order= 2+1= 3
rate constant (k)=

Explanation:-
Rate law says that rate of a reaction is directly proportional to the concentration of the reactants each raised to a stoichiometric coefficient determined experimentally called as order.
![Rate=k[A]^x[B]^y](https://img.qammunity.org/2019/formulas/chemistry/middle-school/nb363n9puy7up25mzrsrec788uk0kmg0rk.png)
k= rate constant
x = order with respect to A
y = order with respect to A
On doubling the concentration of A, rate doubles thus order w.r.t A is 1.
On doubling the concentration of B, rate quadruples thus order w.r.t B is 2.
Thus
![Rate=k[A]^1[B]^2](https://img.qammunity.org/2019/formulas/chemistry/middle-school/p62kppgacrxyuoudilcfxk3a2t2veytrfd.png)
(2)

(1)
(2)
Dividing 2 by 1
![(4.8* 10^(-2))/(2.4* 10^(-2))=(k[0.20]^x[0.30]^y)/(k[0.20]^x[0.15]^y)](https://img.qammunity.org/2019/formulas/chemistry/college/2z7pxu4ogbxea22nl0u2bpkxt79oniz2bj.png)


(2)
(3)
Dividing 3 by 2
![(19.2* 10^(-2))/(4.8* 10^(-2))=(k[0.40]^x[0.30]^y)/(k[0.20]^x[0.30]^y)](https://img.qammunity.org/2019/formulas/chemistry/college/9xwgm5gwzly0xwya1k3spvu9oe5160we2n.png)


rate law:
![Rate=k[X]^2[y]^1](https://img.qammunity.org/2019/formulas/chemistry/college/xj6pvkpcf53jdhxvys39x9n8q471tiaqzq.png)
Total order = 2+1 = 3
using 1:
![2.4* 10^(-2)=k[0.20]^2[0.15]^1](https://img.qammunity.org/2019/formulas/chemistry/college/85eif6becd005uwuyhjfbca8clyvewtcoo.png)
