For the non-stoichiometric reaction:
`A + B to C +D`, the following kinetic data were obtained in three separate experiments, all at 298K.

The order of the reaction is.

Answer

B

Explanation

The rate law expression is `k [A]^x [B]^y = k[A]^x [b]^y`
`therefore (d|C|)/(dt) = k[A]^(x)[B]^(y)`.
Substituting the given values in above equation for three separate experiments we get,
`0.12 = k[0.2]^x [0.2]^y` ....(i)
` 0.24 = k[0.2]^x [0.4]^y` ....(ii)
`0.24 = k[0.4]^x [0.2]^y` .....(iii)
Dividing equation (i) by (iii),
`0.12/0.24 = (k[0.2]^(x)[0.2]^(y))/(k[0.2]^(x)[0.4]^(y))`
`[1/2]^(1) = [1/2]^(y), therefore y =1`
Now Dividing equation ( i) by ( iii),
`0.12/0.24 = (k[0.2]^(x)[0.2]^(y))/(k[0.4]^(x)[0.2]^(y))`
`[1/2]^(1) = [1/2]^(x), therefore x =1`
Hence, the rate law expression is Rate = `k[A]^1 [B]^1`

Hence, the order of the reaction is = `1 + 1 = 2`.