00:01
To determine the order of the reaction with respect to the only reactant, hydrogen peroxide, the reaction being hydrogen peroxide, decomposing into water and oxygen gas, we see that when we double the h2 concentration, h2o2 concentration, that is we go from 0 .005 to 0 .010 molar.
00:30
That's an increase by a factor of 2.
00:37
The rate goes from, the rate also doubles.
00:43
We say that the rate goes to 3 .47 times 10 to the negative 5 from 1 .73 times 10 to the negative 5, which gives us essentially 2.
01:01
So if when we double the concentration, we double the rate, that's representative of first order.
01:09
So it's first order with respect to h2o2 because that is the only reactant, then that is also the overall order is first order.
01:28
Then to determine the rate constant, we need a rate law.
01:32
The rate law is rate is equal to k, multiplied by the constant.
01:36
Concentration of h202 raised to its order of 1.
01:41
So k is simply rate divided by concentration...