The oxidation of hso3- by o2 in aqueous solution is a, Ask an Expert

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The oxidation of HSO3(-) by O2 in aqueous solution is a reaction of importance to the processes of acid rain formation and flue gas desulfurization. The reaction 2 HSO3(-) + O2 --> 2 SO4(-2) + 2 H(+) follows the rate law v = k[HSO3(-)]^2[H(+)]^2. Given a pH of 5.6 and an oxygen molar concentration of 2.4 * 10^-4 mol dm^-3 (both presumed constant), an initial HSO3(-) molar concentration of 5 * 10^-5 mol dm^-3, and a rate constant of 3.6 * 10^6 dm^9 mol^-3 s^-1, what is the initial rate of reaction? How long would it take for HSO3(-) to reach half its initial concentration?

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