Asked by Rebecca
The degradation of CF3CH2F (an HFC) by OH radicals in the troposphere is first order in each reactant and has a rate constant of k=1.6×108M−1s−1 at 4∘C.
If the tropospheric concentrations of OH and CF3CH2F are 8.1×105 and 6.3×108 molecules cm−3, respectively, what is the rate of reaction at this temperature in M/s?
Express your answer using two significant figures.
If you can show work please that would be fantastic!
If the tropospheric concentrations of OH and CF3CH2F are 8.1×105 and 6.3×108 molecules cm−3, respectively, what is the rate of reaction at this temperature in M/s?
Express your answer using two significant figures.
If you can show work please that would be fantastic!
Answers
Answered by
DrBob222
rate = k(CF3CH2F)(OH)
Answered by
Rebecca
Okay... I already know that. I plugged in all the numbers and I get 8.2*10^22, which is not the right answer. Can someone show the work for the problem please?
Answered by
DrBob222
molecules is not M. I would convert molecules to mol which will be mols/cc and convert that to mols/L which is M.
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