A 6.00-L sample of C₂H₄(g)at 2.00 atm and 293 K is burned in 6.00 L of oxygen gas at the same temperature and pressure to form carbon dioxide and water.If the reaction goes to completion,what is the final volume of all gases at 2.00 atm and 293 K?

Question

Quizplus · Accepted Answer

The balanced chemical equation for the combustion of C₂H₄ is:C₂H₄(g) + 3O₂(g) → 2CO₂(g) + 2H₂O(g)According to the stoichiometry of the balanced equation, 1 mole of C₂H₄ reacts with 3 moles of O₂ to produce 2 moles of CO₂ and 2 moles of H₂O. Therefore, the total number of moles of gas in the final mixture is:1 mol C₂H₄ + 3 mol O₂ → 2 mol CO₂ + 2 mol H₂O= 1 mol + 3 mol + 2 mol + 2 mol = 8 molThe final volume of all gases at 2.00 atm and 293 K can be calculated using the ideal gas law:PV = nRTwhere P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.Substituting the given values into the ideal gas law, we get:2.00 atm * V = 8 mol * 0.0821 L·atm/(mol·K) * 293 KSolving for V, we get:V = 2.66 LTherefore, the final volume of all gases at 2.00 atm and 293 K is 2.66 L.

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