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The following initial rate data are for the reaction of nitrogen dioxide with carbon monoxide:
NO2 + CO --> NO + CO2
Experiment [NO2]o, M [CO]o, M Initial Rate, Ms-1
1 0.374 0.300 8.39×10-2
2 0.374 0.600 8.39×10-2
3 0.749 0.300 0.337
4 0.749 0.600 0.337
Complete the rate law for this reaction in the box below.
Use the form k[A]m[B]n , where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n
Rate= ________________
From these data, the rate constant is _________ M-1s-1.

Respuesta :

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Answer:

7.47 × 10^-1 M-1 s-1

Explanation:

Using the form k[A]^m[B]^n we arrive at the fact that the rate constant of the reaction can be written in the form;

Rate = k[NO2] [CO] where both m and n =1

We can use data from any of the experiments to establish the rate constant hence;

From experiment 1

[NO2] = 0.374M

[CO] = 0.300 M

R= 8.39 × 10^-2

Hence k =8.39 × 10^-2 / [0.374] [0.300]

k= 7.47 × 10^-1 M-1 s-1

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