The following reaction was carried out in water :
`Cl_(2) + 2I^(ɵ) rarr I_(2) + 2Cl^(ɵ)`
The initial concentration of `I^(ɵ)` was `0.25 mol L^(-1)` and the concentration after `10 min` was `0.23 mol L^(-1)`. Calculate the rate of disappearance of `I^(ɵ)` and rate of appearance of `I_(2)`.

Explanation

`Delta[I^(ɵ)] = 0.25 - 0.23 = 0.02 mol L^(-1)`
`Delta t = 10 - 0 = 10 min`
`(-Delta[I^(ɵ)])/(Delta t) = ((0.02))/(10) = 0.002 mol L^(-1) min^(-1)`
`= (Delta[I_(2)])/(d t) = -(1)/(2)(Delta[I^(ɵ)])/(d t) = (0.002)/(2) = 0.001 mol L^(-1) min^(-1)`
`= 1 xx 10^(-3) mol L^(-1) min^(-1)`