Question

At 25^oC rate constant for the reaction I^-_(aq) + ClO^-_(aq) IO^-_(aq) + Cl^-_(aq) is 0.0606 M^-1s^-1. If a solution is initially 3.50 × 10^-3 M with respect to each reactant, what will be the concentration of each species present after 300s?

Results must be reported to the correct number of significant figures.

Answer 1

Answer – Given, rate constant k = 0.0606 M^-1.s^-1 , [I^-]o = 3.50*10^-3 M ,

[ClO^-]o = 3.50*10^-3 M , time t = 300 s

From the unit of the rate constant we are getting that this is second order reaction

So the formula for the second order reaction –

First reactant –

1/[I^-] = -k*t + 1/[I^-]o

So, 1/[I^-] = 0.0606 M^-1.s^-1 *300 s + 1/3.50*10^-3 M

              = 303.89 M

So, [I^-] = 3.29*10^-3 M

Now for second reactant –

1/[ClO^-]= -k*t + 1/[ClO^-]o

So, 1/[ClO^-] = 0.0606 M^-1.s^-1 *300 s + 1/3.50*10^-3 M

                   = 303.89 M

So, [ClO^-]= 3.29*10^-3 M