So what's the rate law? I don't know the exponents but you have that you say.
Rate = k(NO)^x*(O2)^y where x and y are the exponents you have determined.
Look at any run in the experiment, substitute rate, (NO) and (O2), then calculate k.
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 × 10-1 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 × 10-1 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:
But I can't find the rate constant! Please help!
"Calculate the rate constant. (in M-2 s-1)"
3 answers
Hi DrBob, the rates are NOT given which is why I am having such an issue trying to work with rate and K both as unknowns.
Yes, the data is there to calculate that. The spacing is not good since this forum messes up the spacing; however, you are given the initial concentrations for both NO and O2. Then you are given the concentrations after certain times. That allows you to know the rate in M/s.