Integrated Rate Law

Question

The decomposition of hydrogen peroxide in dilute sodium hydroxide at 20 °C

H₂O₂(aq)H₂O(l) + ½ O₂(g)

is first order in H₂O₂.

During one experiment it was found that when the initial concentration of H₂O₂ was 6.66×10^-2 M, the concentration of H₂O₂ dropped to 1.56×10^-2 M after 863 min had passed.

Based on this experiment, the rate constant for the reaction is _________ min^-1.

Answer 1

The integrated rate law for a 1st order reaction is..

[A] = [A]_oe^-kt

[A] = 1.56x10^-2 M

[A]_o = 6.66x10^-2 M

k = ?

t = 863 min

Plug in the values and solve for k. The units should be s^-1