Chemistry - Chemical Kinetics Question with Solution | TestHub

If rate $=\mathrm{k}[\mathrm{A}{]}^{\mathrm{x}}[\mathrm{B}{]}^{\mathrm{y}}[\mathrm{C}{]}^{\mathrm{z}}$ From first two given data $8.08\times 10^{-3}=\mathrm{k}[0.2{]}^{\mathrm{x}}[0.1{]}^{\mathrm{y}}[0.02{]}^{\mathrm{z}}\dots (1)$ $2.01\times 10^{-3}=\mathrm{k}[0.1{]}^{\mathrm{x}}[0.2{]}^{\mathrm{y}}[0.02{]}^{\mathrm{z}}\dots .(2)$ Divide $(1)$ by $(2)$ we get, $4=2^x(1/2{)}^y$ Similarly, from second and third data $(9{)}^{\mathrm{y}}(9{)}^{\mathrm{z}}=3$ $2y+2z=1$ From first and fourth data $4^{\mathrm{z}}=8=2^3$ $2z=3.$ So $z=3/2,y=-1,x=1$