In a certain polluted atmosphere containing O3 at a steady-state concentration of 2 × 10^-8 M, the hourly production of O3 by all sources was estimated as 7.2 × 10^-15 M. If only mechanism for the des

Question

In a certain polluted atmosphere containing O3 at a steady-state concentration of 2 × 10^-8 M, the hourly production of O3 by all sources was estimated as 7.2 × 10^-15 M. If only mechanism for the destruction of O3 is second-order reaction, the rate constant (in ml mol^-1 s^-1) for the destruction reaction is

Prashant Kotian · Accepted Answer

Correct answer: 5. At steady state, rate of production = rate of destruction. Rate of production = 7.2 × 10^-15 M/h = (7.2 × 10^-15) / 3600 M/s = 2.0 × 10^-18 M/s. Rate of destruction = k[O3]^2 = k(2 × 10^-8)^2 = k(4 × 10^-16). Equating them: k(4 × 10^-16) = 2.0 × 10^-18, so k = 0.5 × 10^-2 M^-1 s^-1 = 5 × 10^-3 L mol^-1 s^-1. Converting to ml, k = 5 × 10^-3 × 1000 = 5 ml mol^-1 s^-1. Therefore, correct answer is 5.

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