Ozone in the lower atmosphere can react with nitrogen monoxide (shown below). this is one of the steps in the formation of photochemical smog. o₃(g) no(g) → o₂(g) no₂(g) the rate law for this reaction is rate = k[o₃][no] if [o₃] and [no] were to remain essentially constant at [no] = 5.70 × 10⁻⁵ m and [o₃] = 2.20 × 10⁻⁶ m (because of continuous production from separate sources), and k = 3.10 × 10⁶ m⁻¹s⁻¹, calculate the mass in grams of no₂(g) that would be produced per hour per liter of air.