Need help with determining rate law!!!! Part A and B (3 and 4) included in the p

Question

Need help with determining rate law!!!! Part A and B (3 and 4) included in the pic! Questions Consider the reaction between nitrogen dioxide and carbon monoxide: NO2(g) + CO(g)-- NO(g) + CO2(g) The initial rate of the reaction is measured at several IN21 (M) ICO] (M) Initial Rate (M/s) 0.10 0.10 0.20 0.10 0.0021 0.0082 0.0083 0.033 0.10 different concentrations of the reactants with the accompanied results. From the data, determine: 3. the rate law for the reaction 4. the rate constant (k) for the reaction 020 0.20 0.40

Explanation / Answer

3. let the rate law be,

rate = k[NO2]^x[CO]^y

with, k being the rate constant and, x and y be the order with respect to NO2 and CO

from first two readings from the table,

rate1/rate2 = 0.0021/0.0082 = [0.1]^x[0.1]/[0.2]^x[0.1]

x = 2

so the reaction is second order with respect to NO2

Now, from second and third readings from table,

rate2/rate3 = 0.0082/0.0083 = [0.2]^x[0.1]^y/[0.2]^x[0.2]^y

y = 0

so the rate of reaction does not depend upon CO

rate law thus would be,

rate = k[NO2]^2

4. rate constant k = rate/[NO2]^2 = 0.0082/(0.2)^2 = 0.205 M-1.s-1

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