00:01
In the first mechanism, we have two steps where we've got r, vr going to r plus, plus br minus, and this is slow, and then we have r plus oh minus, going to r -o -h, and this one's fast.
00:29
So the rate law for this reaction comes from the slow step, where rate is equal to k, by the concentration of the only reactant, rbr, raised to its coefficient, which is one.
00:46
For mechanism two, we just have a single step of rbr plus oh minus, going to r -o -h -b -r -m minus, and its rate loss, since this is the only step, can be written from its stoichiometry or molecularity, rate, will be equal to k, multiplied by the concentration of r, br raised to the one, multiplied by the concentration of hydroxide raised to the one.
01:22
So now to answer the questions, which mechanism has a reactive intermediate? that's going to be mechanism one.
01:34
The intermediate being r plus that was created and then later consumed.
01:44
What is the reactive intermediate? as i mentioned, r plus, which mechanism is consistent with the rate law, rate equals k, rb, multiplied by hydroxide...