Saved Bookmarks
| 1. |
For the non-stoichiometric reaction: 2A + B to C +D, the following kinetic data were obtained in three separate experiments, all 298 K The rate law for the formation of C is: |
|
Answer» `(dC)/(dt) = K[A]` Rate of reaction, `-1/2(d[A])/(dt) = (-d[B])/(dt) = (d[C])/(dt) = (d[D])/(dt)` Now, rate of reaction, `(d[C])/(dt) = k[A]^(X)[B]^(y)` From table, `1.2 xx 10^(-3)= k(0.1)^(x)(0.1)^(y)`…………(i) `1.2 xx 10^(-3)=k(0.1)^(x)(0.2)^(y)`..........(ii) `2.4 xx 10^(-3)=k(0.2)^(x)(0.1)^(y)`............(III) On dividing equation i) by ii), we GET `(1.2xx10^(-3))/(1.2xx10^(-3)) = (k(0.1)^(x)(0.1)^(y))/(k(0.1)^(x)(0.2)^(y))` `1=(1/2)^(y)` or `(1)^(@) = (1/2)^(Y)`therefore y=0 On dividing equation (i) by (ii), we get `(1.2 xx 10^(-3))/(2.4 xx 10^(-3)) = (k(0.1)^(x)(0.1)^(y))/(k(0.2)^(x)(0.1)^(y))` `(1/2)^(1) = (1/2)^(x)` or x=1 Hence, `(d[C])/(dt) = k[A]^(1)[B]^(0)=k[A]` |
|