Question

Acid rain results from the reaction of nitrogen dioxide with water in the air. Unbalanced equation: NO2(g) + H2O(l) --> HNO3(aq) + NO(g) A water spray is sometimes used in exhaust stacks at coal fired power plants to help prevent acid rain. Given the following parameters, calculate the concentration of the nitric acid in 8L of wastewater (assume no evaporation ... I know this is not reality but let's make the calculation a bit easier!). 1000L/min vented through the exhaust stack assume a constant concentration of the nitrogen dioxide in the exhaust is 0.19ppm The scrubber sprays 500mL/min Assume the density of water is 1g/mL (this is an oversimplification b/c the density is temperature-dependent) Assume 100% of the nitrogen dioxide reacts with the water This is a multi-step stoichiometry problem that requires you make multiple conversions. You must first balance the equation! You must determine the limiting reactant. Use density to get from the volume of water to moles of water. Report your answer to two significant figures.

Answer 1