Sulfur dioxide gas (SO2) and oxygen gas (O2) react to form the liquid product of sulfur trioxide (SO3). How much sulfur dioxide would you need to completely react with 6.00 g O2 such that all reactants could be consumed?
1 answer:
1) Balanced chemical equation: 2SO2 (g) + O2 (g) -> 2SO3 (l) 2) Molar ratios 2 mol SO2 : 1 mol O2 : 2 mol SO3 3) Convert 6.00 g O2 to moles number of moles = mass in grams / molar mass number of moles = 6.00 g / 32 g/mol = 0.1875 mol O2. 4) Use proportions with the molar ratios => 2 moles SO2 / 1 mol O2 = x / 0.1875 mol O2 => x = 0.1875 mol O2 * 2 mol SO2 / 1 mol O2 = 0.375 mol SO2. 5) Convert 0.375 mol SO2 to grams mass in grams = number of moles * molar mass molar mass SO2 = 32 g/mol + 2*16 g/mol = 64 g/mol => mass SO2 = 0.375 mol * 64 g / mol = 24.0 gAnswer: 24.0 g of SO2 are needed to react completely with 6.00 g O2.
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