3 Formula 1 point In the preparation of sulfuric acid (H_(2)SO_(4)) sulfur dioxide must be oxidized to the less harmful sulfur trioxide. How much oxygen in liters must be available to convert 66.9 grams of sulfur dioxide according to this process? Type your answer.

Question

3 Formula 1 point In the preparation of sulfuric acid (H_(2)SO_(4)) sulfur dioxide must be oxidized to the less harmful sulfur trioxide. How much oxygen in liters must be available to convert 66.9 grams of sulfur dioxide according to this process? Type your answer.

Answer 1

To solve this problem, we need to use the balanced chemical equation for the reaction between sulfur dioxide (SO2) and oxygen (O2) to produce sulfur trioxide (SO3).The balanced chemical equation is:2 SO2 + O2 → 2 SO3Given information:- Mass of sulfur dioxide (SO2) = 66.9 gramsStep 1: Calculate the number of moles of sulfur dioxide (SO2).Moles of SO2 = Mass of SO2 / Molar mass of SO2Molar mass of SO2 = 64.06 g/molMoles of SO2 = 66.9 g / 64.06 g/mol = 1.045 molStep 2: Use the stoichiometry of the balanced equation to find the number of moles of oxygen (O2) required.According to the balanced equation, 2 moles of SO2 react with 1 mole of O2.Moles of O2 required = 1.045 mol SO2 × (1 mol O2 / 2 mol SO2) = 0.5225 mol O2Step 3: Calculate the volume of oxygen (O2) required.At standard temperature and pressure (STP), 1 mole of any gas occupies 22.4 liters.Volume of O2 required = 0.5225 mol O2 × 22.4 L/mol = 11.66 LTherefore, 11.66 liters of oxygen must be available to convert 66.9 grams of sulfur dioxide to sulfur trioxide.

Problemas

3 Formula 1 point In the preparation of sulfuric acid (H_(2)SO_(4)) sulfur dioxide must be oxidized to the less harmful sulfur trioxide. How much oxygen in liters must be available to convert 66.9 grams of sulfur dioxide according to this process? Type your answer.

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