The progress of the reaction `AhArrnB` with time, is presented in figure. Determine

the value of n.

Explanation

Step 1: Calculation of the value of n, from the curves Decreases in concentration of A in 4 hours
(1 to 5) `=0.5 -0.3 =0.2` mol
Increase in concentration of A in 4 hours (1 to 5)
`=0.6 - 0.2 = 0.4` mol
`(d[A])/(dt) =0.2 /4` and `(d[B])/(dt) = 0.4/4`
the reaction rate (r) may be given as:
`-(d[A])/(dt) =1/n (d[B])/(dt)` or `-(0.2)/4 = 1/n (0.4/4)`
`n = -0.4/0.2 = -2(2)`
Step II. Calculation of Equilibrium constant The equation may now be written as:
`A `therefore` Equilibrium constant (K) `=[B]^(2)/[A] = (0.6)^(2)/(0.3) =1.2`
Step III: Calculation of initial rate of conversion of A.
`A= (0.2 M)/(2 hr) = 0.1 M hr^(-1)`