The decomposition of hydrogen peroxide was studied, and the following data were obtained at a particular temperature. Time (s)[H2O2] (mol/L)0 1.00120 ± 10.91300 ± 10.78600 ± 10.591200 ± 10.371800 ± 10.222400 ± 10.133000 ± 10.0823600 ± 10.050Assuming that the rate= -delta [H2O2]/delta t determine the rate law, integrated rate law, and the value of the rate constant. Calculate [H2O2] at 4000. s after the start of the reaction.

Explanation:

From the graphical diagram attached below; we can see the relationship between the concentration of which declines exponentially in relation to the time and it obeys the equation:

This relates to the 1st order reaction rate, whereby:

The integrated rate law

here:

[A] = reactant concentration at time (t)

[A]_o = initial concentration for the reactant

k = rate constant

As such, the order of the reaction is the first order

Rate constant

Rate law

The integrated rate law

From the given table:

the initial concentration of = 1.00 M

∴

We can determine the concentration of the reactant at 4000s by using the formula:

Finally, at 4000s: the average rate is:

the correct answer is:

a. formation of precipitation

the ratio of the conjugate base to the acid required to attain the desired ph.