Question

This is more of a chem Q but no one in that section is helping me out =/ if anyone knows how to do this help is much appreciated :)

A reaction is begun with a reaction mixture containing the following: [dye] = 1.0 x 10-4 M [bleach] = 0.10 M When [dye] = 8.0 x 10-5 M the rate is determined to be 3.74 x 10-7 M/min. When [dye] = 4.0 x 10-5 M the rate is determined to be 1.71 10-7 M/min. What is the apparent order with respect to the dye ("a" in the rate equation)?

Answer 1

do i msg him?

Answer 2

What you wanna do here is determine how much the rate changed by changing the concentration of the species, (in this case the dye).

Trial 1:[dye] = 8.0 x 10-5 M; rate=3.74 x 10-7 M/min
Trial 2:[dye] = 4.0 x 10-5 M; rate=1.71 10-7 M/min

[dye]=decreased by half, the rate also decreased by half

can you figure it out from here?

Answer 3

ok I understand how you're halving everything, but what exactly is the question asking me to answer? I'm having trouble understanding what it wants me to put down, the whole equation?

Answer 4

it wants the rate order, (the exponents in the rate law)

rate=k\([dye]^n\)

it wants "n"

Answer 5

ohhh ok, I still don't know the answer, but now i understand what it wants, thanks! I can probably figure the rest out by googling for info haha

Answer 6

haha we'll it's easy to figure out.

assume that rate=\([dye]^1\) -> 2=\([2]^1\)

so it can be first order, because n=1

it works right?

if it was 2=/=\([2]^2\)

so it can't be 2nd order because the rate isn't consistent with the exponent

Answer 7

well I was thinking it was 1, but I haven't actually done the math yet, currently multitasking and sucking at it xD

Answer 8

but i stole the answer from yahoo, thanks for your help!

Answer 9

no problem !