Ozone in the lower atmosphere can react with nitrogen monoxide (shown below). This is one of the steps in the formation of photochemical smog. O(g) + NO(g) O(g) + NO(g) The rate law for this reaction is rate = k[O][NO] If [O] and [NO] were to remain essentially constant at [NO] = 5.70 10 M and [O] = 2.20 10 M (because of continuous production from separate sources), and k = 3.10 10 Ms, calculate the mass in grams of NO(g) that would be produced per hour per liter of air.

Answer should be in grams