The rate of a certain reaction is given by the following rate law: rate =k[N2]3[

Question

The rate of a certain reaction is given by the following rate law: rate =k[N2]3[03] Use this information to answer the questions below. What is the reaction order in N2? What is the reaction order in O3? What is overall reaction order? At a certain concentration of N2 and O3r the initial rate of reaction is 0.390 M/s. What would the initial rate of the reaction be if the concentration of N2 were doubled? Be sure your answer has the correct number of significant digits. The rate of the reaction is measured to be 23.0 M/ s when [N2] = 1.7 M and [031 = 0.48 M. Calculate the value of the rate constant. Be sure your answer has the correct number of significant digits

Explanation / Answer

Rate = k[N2]^3[O3]

Order of reaction with respect to [N2] = 3

Order of reaction with respect to [O3] = 1

Order of overall reaction = 3+1 = 4

Initial rate of the reaction = 0.39 M/s

If [N2] is doubled means,

Rate = k[2*N2]^3[O3]

Rate = k* 2^3*[N2]^3[O3]

Rate = 8*k[N2]^3[O3]

So the rate of reaction increswd by 8 times so the final rate of the reaction is = 8* 0.39 = 3.12 M/s

Rate of reaction = 23 M/s

[N2] = 1.7 M and [O3] = 0.48 M

Rate = k [N2]^3[O3]

23 = k * (1.7)^3*(0.48)

k = rate constant = 9.753 M^-3.S^-1

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