# Chemistry

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An atmospheric scientist interested in how NO is converted into NO2 in urban atmospheres carries out two experiments to measure the rate of this reaction. The data are tabulated below.

A: [NO]0 = 9.63 × 10-3 M, [O2]0 = 4.1 × 10-4 M
t(s) 0/3.0/6.0/9.0/12.0
[O2] 4.1/2.05/1.02/0.51/0.25
*[O2] is in(10-4 M)

B: [NO]0 = 4.1 × 10-4 M, [O2]0 = 9.75 × 10-3 M
t(s) 0/1.00/2.00/3.00/4.00
[NO] 4.1/2.05/1.43/1.02/0.82
*[NO] is in(10-4 M)

I figured out the rate law:
Rate=k[O2][NO]2

"Calculate the rate constant. (in M-2 s-1)"

• Chemistry -

Use the rate law expression you have and substitute EITHER set of data into that equation. That is, substitute the number for (O2), the number for (NO) and the number for rate, then solve for k.

• Chemistry -

I got it, thanks!

• Chemistry -

What was the value?

• Chemistry -

how do you get the rate?

• Chemistry -

Did anyone end up getting this. if you plug in the numbers above you still need the retain rate to find k. How do you do that??!!

• Chemistry -

to get rate you need to get the slope of the graph

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