Vane11
  • Vane11
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)?
Biology
  • Stacey Warren - Expert brainly.com
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SOLVED
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schrodinger
  • schrodinger
I got my questions answered at brainly.com in under 10 minutes. Go to brainly.com now for free help!
Vane11
  • Vane11
do i msg him?
aaronq
  • aaronq
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?
Vane11
  • Vane11
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?

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aaronq
  • aaronq
it wants the rate order, (the exponents in the rate law) rate=k\([dye]^n\) it wants "n"
Vane11
  • Vane11
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
aaronq
  • aaronq
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
Vane11
  • Vane11
well I was thinking it was 1, but I haven't actually done the math yet, currently multitasking and sucking at it xD
Vane11
  • Vane11
but i stole the answer from yahoo, thanks for your help!
aaronq
  • aaronq
no problem !

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