chem class
posted by jack ross on .
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?