Sulfur burns in oxygen with a deep blue flame to produce sulfur dioxide.If 5.85 g S₈ and 1.00 atm of O₂ completely react in a 5.00 L flask (at 25°C),determine the partial pressure of SO₂ (at 25°C)and the total pressure in the flask. S₈(s)+ 8O₂(g)→ 8SO₂(g)

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Quizplus · Accepted Answer

The balanced chemical equation is:S8(s) + 8O2(g) → 8SO2(g)The molar mass of S8 is 256.56 g/mol. Therefore, 5.85 g of S8 is equal to 5.85 g / 256.56 g/mol = 0.0228 mol.The initial partial pressure of O2 is 1.00 atm. According to the balanced chemical equation, 8 moles of O2 react with 1 mole of S8. Therefore, the initial number of moles of O2 is 8 * 0.0228 mol = 0.1824 mol.The total number of moles of gas in the flask after the reaction is 0.0228 mol + 0.1824 mol = 0.2052 mol.The partial pressure of SO2 is equal to the number of moles of SO2 divided by the total number of moles of gas in the flask multiplied by the total pressure. Therefore, the partial pressure of SO2 is 8 * 0.0228 mol / 0.2052 mol * 1.00 atm = 0.893 atm.The total pressure in the flask is equal to the sum of the partial pressures of all the gases in the flask. Therefore, the total pressure in the flask is 0.893 atm + 0.107 atm = 1.00 atm.

Sulfur Burns in Oxygen with a Deep Blue Flame to Produce