A reaction of importance in the formation of smog is that between ozone and nitr

Question

A reaction of importance in the formation of smog is that between ozone and nitrogen monoxide described by O_3(g)+NO(g) rightarrow O_2(g) + NO_2(g) The rate law for this reaction is rate of reaction = k[O_3][NO] Given that k = 2.99 times 10^6 M^-1 s^-1 at a certain temperature, calculate the initial reaction rate when [O_3] and [NO] remain essentially constant at the values [O_3]_0 = 6.87 times 10^-6 M and [NO]_0= 7.46 times 10^-5 M, owing to continuous production from separate sources. Calculate the number of moles of NO_2(g) produced per hour per liter of air.

Explanation / Answer

Initial rate = k [O3] [NO] = 2.99 * 106 * 6.87 * 10-6 * 7.46 * 10-5 = 1.53 * 10-3 M s-1

M is defined as moles / L. We need moles/L / hr = M / hr

we have M / sec.. so..

(1.53 * 10-3 M / sec) x (60 sec / hr) = 0.0918 M / hr

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