00:01
To determine the rate law, we need to know the order of the reaction with respect to each reactant.
00:07
If we look at runs 1 and 2, we see that the concentration of rx is constant, but the concentration of hydroxide is being doubled.
00:21
The hydroxide concentration in run 2 is 0 .02, and then it goes to 0 .02, 0 .04 in run 1.
00:36
When that happens, we see that the rate goes from 4 times 10 to the negative 6 to 8 times 10 to the negative 6.
00:47
So when we double the concentration, we double the rate.
00:51
That is representative of first order.
00:55
If we double the concentration and nothing happens, it's zero order.
00:59
If we double the concentration and the rate quadruples, it's second order.
01:04
So now if we look at runs 1 and 3, we see that we're keeping the hydroxide concentration constant, but we have doubled the rx concentration.
01:23
So the concentration of rx goes from 0 .005 molar in run 3 to 0 .01 molar in run 1.
01:38
And when that happens, the rate goes from 4 times 10 to the negative 6 to 8 times 10 to the negative 6...