Question

6. A power plant emits SO2 at a concentration of 1.00 g/m3 as S. In the atmosphere, SO2 reacts with water vapors to form H2SO3 and H;SO4. Assuming that a 40.0% of the emitted SO2 reacts to form H2SO3 and the rest of it reacts to form H2SO. a. Calculate the concentration of H2SO3 and of H2SO4. Express your answer in mol/m3 and g/m3 as S. b. Calculate the sum of the concentrations of H2SO; and H2SO4 Express your answer in &m2 as S. c. Knowing that H2SO4 is an acid (causing acid rain) calculate its concentration in units of eq/m2

Answer 1

It is given that Iglm² of son is liberated out of which 40% (0.4 alma is tesog & 60% (0.6 glm²) he so is formed. Molecular mass of the so, z82 g/mol Molecular mass of ty so as a8 g/mol a) - Concentration of ty 50 = 0.4g/m3 - 004 g/m3 =0.005 mol 82 glmol Concentration of thy so 4 = obglms - - 6.6 glm3 = 0.006 mol 98 g/mol m3 Sum of Concentration of tys og & ty sa is = 0.4 +0.6 = 10 g b) c) Concentration of the sopa oooo6 mol = 0.006 mood x 2m