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rate equation

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hiro:
experiment    [NO2]at start(M)    [F2]at start(M)     initial rate(molL-1s-1)
   1                     0.001                    0.005                  2x10^-4
   2                     0.002                    0.005                  4x10^-4
   3                     0.002                    0.01                    8x10^-4

the equation of this is 2NO2+F2-->2NO2F

but how to write the rate equation for this reaction?

thx

Donaldson Tan:
i give you a clue.

rate = k[NO2]a[F2]b

find the ratio of experimental rate of (1) over (2) and that for concentration of reactants.

GCT:

--- Quote from: hiro on May 13, 2005, 09:53:27 AM ---experiment    [NO2]at start(M)    [F2]at start(M)     initial rate(molL-1s-1)
   1                     0.001                    0.005                  2x10^-4
   2                     0.002                    0.005                  4x10^-4
   3                     0.002                    0.01                    8x10^-4

the equation of this is 2NO2+F2-->2NO2F

but how to write the rate equation for this reaction?

thx

--- End quote ---

how can you find the order of each reactant with respect to the rate?

what can you do to find k?

It doesn't get any simpler than this.

Donaldson Tan:
comparing experiments (1) and (2), the rate doubles when [NO2] doubles.

comparing experiments (2) and (3), the rate doubles when [F2] doubles.

This should be more than sufficient for you to arrive at your answer.

chemical:
hi,

if NO2 is increased the rate doubles this means it is a first order reaction
if F2 is increased the rate doubles also this means it is first order reaction thus the overal reaction is 2nd order

K[NO2]1[F2]1

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