00:01
Right, so we're given the rate equation, which we see is second order in p, and then we don't have anything written for the q, so that's going to be first order.
00:09
For part a, we want the overall order with respect to p and q.
00:13
So that means we're going to take the sum of the orders of p, which is 2, and q, which is 1, to get an overall reaction order of 3.
00:20
So just add all the exponents, i mean.
00:23
All right, for part b, we want to calculate the rate constant.
00:27
We're given the rate and the concentrations at a certain point in time.
00:31
So we can rearrange this equation to solve for k and just plug in.
00:35
So k is equal to if we divide both sides by p squared and q, k is going to be the rate over the concentration of p squared, multiplied by the concentration of q.
00:48
The rate that we're given is 0 .45 times 10 to the negative fourth.
00:53
I don't know why that's not in proper scientific notation, but oh well.
00:59
And that's going to be molar.
01:01
Second.
01:02
And then we have concentration of p is 0 .012 molar and that's going to be squared.
01:13
Concentration of q is 0 .035 molar.
01:18
All right.
01:20
So now we can just do the math...