Consider the reaction `2A + B to 2C`. Suppose that at a particular moment during the reaction , rate of disappearance of A is 0.076 `m//s`
(a) What is the rate of formation of C ?
( b ) What is the rate of consumption of B ?
(c) What is the rate of the reaction ?

Answer

(a) Rate of formation of C= 0.076 `Ms^(-1)`
( b) Rate of consumption of B= 0.038 `Ms^(-1)`
( c) Rate of reaction = 0 .038 `Ms^(-1)`

Explanation

Given : `2A + B to 2C`
Rate of disappearance of A= 0.076 `Ms^(-1)`
(a) Rate of formation of C= ?
( b) Rate of consumption of B = ?
(c ) Rate of reaction = ?
Rate of disappearance of `A = (d[A])/(dt) = 0.076 Ms^(-1)`
(a) Rate of formation of `C= (d[C ])/(dt) = (d[A])/(dt)`
`=0.076 Ms^(-1)`
( b) Rate disappearance of `B= (d[B])/(dt) = - (1)/(2) (d[A])/(dt)`
`= (1)/(2) xx 0.076 =0. 038 Ms^(-1)`
( c) Rate of reaction `=- (1)/(2) .(d[A])/(dt) = (-d[B])/(dt) = (1)/(2) (d[C])/(dt)`
`= (1)/(2) (0.076) = 0.038 = (1)/(2) xx 0.076`
`= 0.038 Ms^(-1)`