00:01
To determine the order of the reaction with respect to each reactant, we need to find two experiments where one concentration is stained constant and the other one is changing.
00:10
If we look at experiments 1 and 2, we'll see that the, i'm sorry, 1 and 3, we'll see that the concentration of permanganate is stained constant, but the concentration of h2c204 is changing.
00:26
The ratio of the change is 2 .31.
00:30
I'll take the concentration in experiment 3, which is larger, divided by that in experiment 1, and i get 2 .31.
00:41
I'll do a similar ratio of the rates, experiment 3 to experiment 1, and i get a 2 .31 ratio also.
00:51
So if what i do to the concentration, i do to the rate, then this is indicative of first order.
00:58
I 2 .31 times the concentration, i 2 .31 times the rate, its first order with respect to h2c204 oxalic acid.
01:11
Now if i look at experiments 2 and 3, i see that the concentration of oxalic acid is staying constant, but the concentration of permanganate is changing.
01:24
It goes from .0033 to .0089.
01:30
That's an increase of 2 .70 .70.
01:33
The rate then goes from 2 .179 times 10 to negative 5 to 8 .08 times 10 to negative 6...
