Determine the mass of sulphur (IV) oxide obtained when 91.0g of oxygen reacts completely with sulphur according to the following equation: S(s) + O2(g) → SO...

Answer Details

The balanced chemical equation for the reaction between sulfur and oxygen to form sulfur dioxide is: S + O₂ → SO₂ This equation tells us that 1 mole of sulfur reacts with 1 mole of oxygen to produce 1 mole of sulfur dioxide. We are given the mass of oxygen that reacts completely with sulfur, which is 91.0 g. We can use this information to calculate the number of moles of oxygen: Number of moles of oxygen = Mass of oxygen / Molar mass of oxygen Number of moles of oxygen = 91.0 g / 32 g/mol Number of moles of oxygen = 2.84 mol From the balanced equation, we can see that the number of moles of sulfur dioxide produced is equal to the number of moles of oxygen that reacts. Therefore, we have: Number of moles of sulfur dioxide = 2.84 mol Now we can use the molar mass of sulfur dioxide to calculate its mass: Mass of sulfur dioxide = Number of moles of sulfur dioxide × Molar mass of sulfur dioxide Mass of sulfur dioxide = 2.84 mol × (32 g/mol + 2 × 16 g/mol) Mass of sulfur dioxide = 2.84 mol × 64 g/mol Mass of sulfur dioxide = 182 g Therefore, the mass of sulfur dioxide produced when 91.0 g of oxygen reacts completely with sulfur is 182 g. So, the correct option is (d) 182g.