00:01
To determine the rate constant for the overall reaction, we first need to determine the order of the reaction with respect to each reactant.
00:08
We've got 2 icl reacting with h2 to produce i2 and 2hcl.
00:18
If we look at experiments 1 and 3, we see that the concentration of the icl is constant constant at 0 .2 .2.
00:33
Molar and only the concentration of h2 is doubled.
00:44
When we double the concentration of h2 we see that the rate increases to 0 .00500 from 0 .002.
01:00
So we see a doubling of the rate if what we do to the concentration, we do to the rate, then this is representative of a first -order reaction.
01:16
So it is first order with respect to h -2.
01:24
Then if we look at experiments 1 and 2, we see that the concentration of h -2 is staying constant at 0 .1 molar, but only the concentration of icl is increased by a factor of 1 .5, it goes from 0 .1 to, i'm sorry, it goes from, well, it's actually decreased.
02:00
Okay, hold on a second.
02:02
So let's look at it in reverse.
02:04
Let's go compare 2 to 1.
02:08
If that's the case, then we see that the concentration in 2 is 0 .15, and the concentration in 1 is 0 .2, so that ratio is 1 .33.
02:28
So when we increase the concentration of icl 1 .33 times, the rate increase ends up being it goes to 0 .00 -250 -0 in experiment 1 to 0 .00.
02:58
I'm sorry, it goes to 2 .00.
02:59
To this rate at the higher concentration from 141 at the lower concentration...