The data in the table below were obtained for the reaction:

A + B → P

3 Experiments

1 (A) (M): 0.273 (B) (M): 0.763 Initial Rate
(M/s): 2.83

2 (A) (M): 0.273 (B) (M): 1.526 Initial Rate
(M/s): 2.83

3 (A) (M): 0.819 (B) (M): 0.763 Initial Rate
(M/s): 25.47

1) The order of the reaction in A is __________.

2) The order of the reaction in B is __________.

3) The overall order of the reaction is __________.

im confused by the experiments graph how do i find the order?

rate = k[A]x[B]y

Label the experiments above 1,2, and 3.
Substitute 2 data and divide by 1 data. You should have the following.
2) 2.83 = k*[0.273]x[1.526]y
----------------------------------------
1) 2.83 = k*[0.273]x[0.763]y

So 2.83/2.83 = 1.
k cancels.
[0.273]x cancels and you are left with
1 = (2)y
So y must be zero and the reaction is zero order in B.
You do the same kind of thing to determine x, the reaction order of A. The overall order is order for A + order for B.
To find x, I would use #3 divided by #1. Post your work if you get stuck.

i divided:

1.526/0.763 and it gives me 2

2.83=2y <~ not 2.83

i did this:

2) 2.83 = k*[0.273]x[1.526]y
----------------------------------------
1) 2.83 = k*[0.273]x[0.763]y

2.83=2y

log:

0.405 = y
-------
0.301

1.5=y
2=y

is that right too?

To find the order of the reaction, you can use the method of initial rates. This involves comparing the initial rates of the reaction at different concentrations of the reactants. By examining how the initial rate changes with the concentration of each reactant, you can determine the order of the reaction.

In this case, you have three experiments with varying concentrations of reactants A and B, and their corresponding initial rates. We can use these values to calculate the orders of reaction in A and B, as well as the overall order of the reaction.

Let's go step by step:

1) To find the order of the reaction in A, we will compare the initial rates for experiments 1 and 2, where the concentration of A is kept constant and the concentration of B varies.

For experiments 1 and 2:
(A) (M): 0.273 (constant concentration)
(B) (M): 0.763 Initial Rate (M/s): 2.83
(B) (M): 1.526 Initial Rate (M/s): 2.83

Since the initial rate is the same in both experiments, it indicates that the concentration of B does not affect the rate of the reaction. Therefore, the order of the reaction in A is zero.

2) Similarly, to find the order of the reaction in B, we will compare the initial rates for experiments 1 and 3, where the concentration of B is kept constant and the concentration of A varies.

For experiments 1 and 3:
(A) (M): 0.273 Initial Rate (M/s): 2.83
(A) (M): 0.819 Initial Rate (M/s): 25.47 (increased by a factor of 9)

Here, we see that increasing the concentration of A from 0.273 M to 0.819 M increases the rate of the reaction by a factor of 9. This suggests that the rate of the reaction is directly proportional to the concentration of A. Therefore, the order of the reaction in B is 1.

3) The overall order of the reaction is the sum of the individual orders of the reactants. From the previous calculations, we found the order of reaction in A is 0 and in B is 1. Therefore, the overall order of the reaction is 0 + 1 = 1.

To summarize:

1) The order of the reaction in A is 0.
2) The order of the reaction in B is 1.
3) The overall order of the reaction is 1.

By analyzing the data from the experiments and comparing the initial rates at different reactant concentrations, you can determine the orders of the reaction in A, B, and the overall reaction.