The following data were collected for the rate of disappearance of NO in the rea

ID: 862877 • Letter: T

Question

The following data were collected for the rate of disappearance of NO in the reaction 2 NO(g) + O2(g) ? 2 NO2(g).

(a) What is the rate law for the reaction? (Rate equations take the general form 'rate = k . [A] . [B]'.)

(b) What is the average value of the rate constant calculated from the three data sets?

(d) What is the rate of disappearance of O2 at the concentrations given in part (d)?

Experiment [NO] (M) [O2] (M) Initial Rate
(M/s) 1 0.0126 0.0125 1.41 10-2 2 0.0252 0.0125 5.64 10-2 3 0.0252 0.0250 1.13 10-1

(a) What is the rate law for the reaction? (Rate equations take the general form 'rate = k . [A] . [B]'.)

rate = k . [NO]^a* [O2]^b

When NO is doubled rate is increased 4times

Rate1/rate2= (1.41/5.64) = (.0126/.0252)^a

So a = 2

Similarly

Rate2/rate3 = (.0564/.113) = (.0125/.0250)^b

So b=1

rate = k . [NO]^2* [O2]

(b) What is the average value of the rate constant calculated from the three data sets?

k = rate/([NO]^2* [O2])

k1 = 0.0141/(.0126^2*.0125)=7105.1 s-1 M-1

k2 = 0.0564/(.0252^2*.0125)=7105.1 s-1 M-1

k3 = 0.113/(.0252^2*.0250)=7117.7 s-1 M-1

Average k = 1/3*(k1+k2+k3) = 7109.3 s-1 M-1

when [NO] = 0.0750 M and [O2] = 0.0100 M?

Rate of reaction = k . [NO]^2* [O2] = 7109.3*(.075)^2*(.01)=0.4 M/s

Rate of disappearance of NO =2*rate of reaction = 2*.4=0.8M/s

(d) What is the rate of disappearance of O2 at the concentrations given in part (d)?

Rate of disappearance of O2 = 1*.4 = 0.4M/s

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