At T(K), the following data were obtained for a general reaction, A + B + C `to` products

`The rate constant for the above reaction is

Options

A. `8.0xx10^(-4)s^(-1)`
B. `8.0xx10^(-4)Lmol^(-1)s^(-1)`
C. `8.0xx10^(4)Lmol^(-1)s^(-1)`
D. `8.0xx10^(-4)L^(2)mol^(-2)s^(-1)`

Answer

B

Explanation

Comparing expt. (1) and expt. (2). When [B] is doubled rate of reaction doubles.
`therefore` Reaction is first order is B.
Comparing expt. (2) and expt (3).
When [C] is doubled rate of reaction doubles.
`therefore` Reaction is first order in C.
Comparing expt. [3] and expt [4]. When [A] is doubled rate of reaction remains unchanged.
`therefore` Reaction is zero order in A.
Rate law = `K[A]^(0)[B][C].`
Using data of expt. (1) we get
`2.4xx10^(-6)=K[0.02]^(0)[0.1]^(1)[0.03]^(1)`
`2.4xx10^(-6)=Kxx1xx0.1xx0.03`
`K=(2.4xx10^(-6))/(3xx10^(-3))=0.8xx10^(-3)=8.0xx10^(-4)Lmol^(-1)s^(-1)`