Rate of reaction, `A+B rarr` products is given below as a function of different initial concentration of

Determine the order of the reaction with respect to A and B. What is the half-life of A in the reaction?

Explanation

(i) A=1, B=0 (ii) `t_(1//2) =1.386` min
Looking at the rate data of experiment number 1 and 2 indicates that rate is doubled on doubling concentration of A while concentration of B is constant. Therefore, order with respect to A is 1. Similarly, comparing data of experiment number 1 and 3, doubling concentration of B, while concentration of A is constant, has no effect on rate. Therefore, order with respect to B is zero.
`rArr " Rate "=k[A] rArr k=(0.005)/(0.010)=0.5" m in"^(-1)=(0.693)/(t_(1//2)) rArr t_(1//2) =(0.693)/(0.5) =1.386` m in