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Sulfur dioxide gas reacts with oxygen gas and water according to the chemical reaction below. When 4.5g of SO2 are mixed with excess o2 and H2O how many grams of H2SO4 are produced? 2so2(g) + o2(g) + 2h2o(l) -> 2h2so4(l)
Accepted Answer
2SO2(g) + O2(g) + 2H2O(l) → 2H2SO4(l)
To solve this problem, we need to determine the limiting reactant. To do this, we will convert the mass of SO2 to moles using its molar mass (64.06 g/mol):
moles of SO2 = 4.5 g / 64.06 g/mol = 0.0702 mol
Now, we will convert the moles of SO2 to moles of H2SO4 using the stoichiometry of the balanced chemical equation:
moles of H2SO4 = 0.0702 mol SO2 × 2 mol H2SO4 / 2 mol SO2 = 0.0702 mol H2SO4
Finally, we will convert the moles of H2SO4 to grams using its molar mass (98.08 g/mol):
grams of H2SO4 = 0.0702 mol H2SO4 × 98.08 g/mol = 6.88 g
Therefore, 4.5 g of SO2 will produce 6.88 g of H2SO4.
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