Question

The decomposition of H2O2 is first order in H2O2 and the rate constant for this reaction is 1.63 x 10-4 s-1. How long will it take for [H2O2] to fall from 0.95 M to 0.33 M?

Answer 1

Answer:

It will take 6486.92 minutes  for [H2O2] to fall from 0.95 M to 0.33 M

Explanation:

The order of reaction is defined as the sum of the powers of the concentration terms in the equation. Order of a reaction is given by the number of atoms or molecule whose concentration change during the reaction and determine the rate of reaction.

In first order reaction;

$In \dfrac{a}{a_o-x}= k_1 t$

where;

a = concentration at time t

$a_o$ = initial concentration

and k = constant.

$In (\dfrac{0.33}{0.95})= -1.63 \times 10^{-4} \times t$

$-1.05736933 = -1.63 \times 10^{-4} \times t$

$t = \dfrac{-1.05736933}{ -1.63 \times 10^{-4} }$

t = 6486.92 minutes