Question

The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C is first order in H2O2.H2O2(aq)H2O(l) + ½ O2(g)During one experiment it was found that the H2O2 concentration dropped from 2.88×10-2 M at the beginning of the experiment to 1.28×10-2 M in 839 min. What is the value of the rate constant for the reaction at this temperature? min-1

Answer 1

So, we're given the following reaction:

The reaction follows a first order, so:

Initial concentration of H2O2 = 2.88×10^-2 M

Concentration of H2O2 in 839 min = 1.28×10^-2 M

We obtain the change in concentration of H2O2 substrating: 2.88×10^-2 M - 1.28×10^-2 M, which is 1.6×10^-2 M.

Now, let's replace this value in the equation:

So the answer is k=0.00148987