2 you obtain the below data for a reaction between a and b...

2) You obtain the below data for a reaction between A and B to give P (concentrations are M) [A] [B] Initial Rate (M/hr) 0.10 0.10 3.0x10$^{-3}$ 0.10 0.30 3.0x10$^{-3}$ 0.30 0.30 2.7x10$^{-2}$ 0.30 0.60 2.7x10$^{-2}$ a) What is the order of the reaction with respect to each reagent (A and B). (10 points) b) Write the rate law for this reaction (5 points) c) Calculate k when [A] and [B] are 0.1 M (5 points) d) What would you expect the rate of the reaction to be if [A] is increased to 1.0 M (5 points)

Transcript

00:01 For the generic reaction a plus b plus c goes to d, given the initial rates and the initial concentrations, we should be able to determine the order of the reaction with respect to each reactant.

00:13 When only c is doubled, so i'm looking at experiments, let's see, a, 1, and 4, where the a concentration stays constant at 0 .05, and the b concentration stays constant at 0 .05, 0 .05, but the concentration of c is doubled from 0 .01 to 0 .02.

00:43 We see that the rate stays constant for experiments 1 and 4.

00:47 Therefore, if you change the concentration of just one reactant, and the rate does not change when changing the concentration of that reactant, this would be zero order.

01:00 So it's zero order with respect to c.

01:04 Now when only b is doubled, so i'm looking at experiments 2 and 3 where a stays constant at 0 .1 molar and c stays constant at 0 .01 molar, and b goes from 0 .05 to 0 .1 molar.

01:23 When we double the concentration of b, we'll notice that we quadruple the rate of the reaction from 1 .25 times 10 to the negative 2 to 5 .00 times 10 to the negative 2, doubling a concentration resulting in a and a quadrupling of a reaction is indicative, the rate of the reaction is indicative of a second order reaction.

01:48 So this reaction is second order with respect to b.

01:52 Now when only a is doubled, so i'm looking at experiments one and two, where c stays constant at 0 .01, b stays constant at 0 .05 molar, and a is doubled from 0 .05 to point one.

02:08 We see that the rate of the reaction is also doubled from 6 .25 times 10 to negative 3 to 1 .25 times 10 to the negative 2.

02:17 So when we double the concentration, we double the rate.

02:23 This is indicative of a first order reaction, so it's first order with respect to a.

02:30 So we can then write the differential rate law for the reaction as rate is equal to k, multiplied by a concentration of a, raised to the first power, multiplied by concentration of b raised to the second power...

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