In the formation of acid rain, sulfur dioxide reacts with oxygen and water in the air to form sulfuric acid. Write the balanced chemical equation for the reaction.
2 SO2 + 1 O2 + 2 H2O --> 2 H2SO4
If 5.45 g SO2 react with excess oxygen and water, how many grams of H2SO4 are produced?
g
Convert 5.45 g SO2 to mols using mols = g/molar mass.
Convert mols SO2 to mols H2SO4 using the coefficients in the balanced equation.
Convert mol H2SO4 to grams using g = mols x molar mass.
231
if the information of acid rain sulfur dioxide reacts with oxygen and water in the air to form sulfuric acid. 2.25 g of sulfur dioxide react how many moles of sulfuric acid are produced?
To find the grams of H2SO4 produced, we need to use stoichiometry. Stoichiometry is a calculation method that uses balanced chemical equations to relate the amounts of reactants and products in a chemical reaction.
First, we need to determine the number of moles of SO2 using its molar mass. The molar mass of SO2 is 64.06 g/mol. We can calculate the number of moles of SO2 by dividing the mass (5.45 g) by the molar mass:
moles of SO2 = mass of SO2 / molar mass of SO2
moles of SO2 = 5.45 g / 64.06 g/mol
moles of SO2 ≈ 0.085 moles
The balanced chemical equation tells us that the ratio of moles of SO2 to moles of H2SO4 is 2:2 (1:1 simplified). Therefore, the number of moles of H2SO4 produced will also be 0.085 moles.
Finally, we can calculate the mass of H2SO4 produced using its molar mass. The molar mass of H2SO4 is 98.09 g/mol. We can multiply the number of moles of H2SO4 (0.085 moles) by the molar mass to find the mass:
mass of H2SO4 = moles of H2SO4 x molar mass of H2SO4
mass of H2SO4 = 0.085 moles x 98.09 g/mol
mass of H2SO4 ≈ 8.36 g
Therefore, approximately 8.36 grams of H2SO4 are produced when 5.45 grams of SO2 react with excess oxygen and water.