If 0.500 g of sulfur dioxide from pollutants reacts with excess water and oxygen found in the air, what mass of sulfuric acid can be produced?
2H2O(l)+O2(g)+2SO2(g)= 2H2SO4(aq)
To determine the mass of sulfuric acid that can be produced, we first need to find the number of moles of sulfur dioxide (SO2) using the given mass.
The molar mass of sulfur dioxide (SO2) is:
Sulfur (S) = 32.06 g/mol
Oxygen (O) = 16.00 g/mol (2 oxygen atoms in sulfur dioxide)
Therefore, the molar mass of SO2 = 32.06 g/mol + 2 * 16.00 g/mol = 64.06 g/mol.
Next, we can calculate the number of moles of SO2 using the given mass:
Number of moles = Mass / Molar mass
Number of moles of SO2 = 0.500 g / 64.06 g/mol = 0.00780 mol
According to the balanced chemical equation, the stoichiometric ratio between SO2 and H2SO4 is 2 moles of SO2 to 2 moles of H2SO4. So, the number of moles of H2SO4 produced will be the same as the number of moles of SO2.
Number of moles of H2SO4 = 0.00780 mol
Finally, to determine the mass of H2SO4 produced, we can multiply the number of moles by the molar mass of sulfuric acid (98.09 g/mol):
Mass of H2SO4 = Number of moles of H2SO4 * Molar mass of H2SO4
Mass of H2SO4 = 0.00780 mol * 98.09 g/mol = 0.766 g
Therefore, approximately 0.766 grams of sulfuric acid can be produced.