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The rate law for the reaction described by the equation
O3 (g) + NO (g) ---> O2 (g) + NO2 (g) at 310 K is

rate of reaction= (3.0 x 10^6 M ^-1 x s^-1) O3 NO (O3 and NO are inbrackets)

Given that O3 (in brackets) = 6.0 x 10^-4 M and NO (in brackets)= 4.0 x 10^-5 M at t= 0, calculate the rate of the reaction att=0

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Casey Durgan
Casey DurganLv2
16 Sep 2019

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Related questions

The reaction described by this equation: O3(g) + NO(g) ----> O2(g) + NO2(g)

has the following rate law at 310 K.

rate of reaction = k [O3][NO]

k = 3.0 x 106 M-1s-1

Given that [O3] = 7.0 x 10-4 M and [NO] = 8.0 x 10-5 M at t=0, calculate the rate of the reaction at t=0. _______M/s

What is the overall order of this reaction? 0, 1, 2, or 3?

Explain the answer.

A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by:

O3(g) + NO(g) => O2(g) + NO2(g)

The rate law for this reaction is:

rate of reaction = k[O3][NO]

Given that k = 3.66*106 /M*s at a certain temperature, calculate the initial reaction rate when [O3] and [NO] remain essentially constant at the values

[O3]0 = 2.25*10-6 M and

[NO]0 = 4.37*10-5Ā M,

owing to continuous production from separate sources.

Calculate the number of moles of NO2(g) produced per hour per liter of air.

An important reaction in the formation of photochemical smog is the reaction between ozone and NO:

NO(g)+O3(g)--> NO2(g)+O2(g)

The reaction is first order in NO and O3. The rate constant of the reaction is 80 (1/M*s) at 25 C and 3.000 x 10^3 (1/M*s) at 75 C.

(a) If this reaction were to occur in single step, would the rate law be consistent with the observed order of the reaction for NO and O3? yes/no

(b) What is the value of the activation energy of the reaction?

(c) What is the rate of the reaction at 25 X when [NO]= 2.63 x 10^-6 M and [O3]=5.96 x 10^-9 M?

(d) Predict the values of the rate constant at the following temperatures:

10 C and 35 C

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