correct answer is suppose to be about 0.023. How do you get this?

During production, transport, and use of natural gas (primarily methane), some inevitably leaks into the atmosphere where it acts as a greenhouse gas. The principal removal mechanism for methane is via reaction with hydroxyl radical (page 90 of the text). Assuming the second-order rate constant for the reaction is k=9.2x 1015cm3molec1s1, the methane concentration is 2.207ppmv (similar to the concentration given in Table 8.3 ), and the hydroxyl radical concentration is 1.2106moleccm3 (a reasonable estimate for a clean atmosphere), calculate a pseudo-first-order rate constant for the reaction. Use the pseudo-first-order rate jnstant to calculate the first-order half-life for methane in the atmosphere. Report the half-life to three decimal places in units of minutes. Do not include units in your answer. Assume 25C and 1.00atm pressure for unit conversion