What volume of H₂O gas is produced at 150 ° C and 1.00 atm of pressure from the reaction of 1.12 L of H₂ and 1.12 L of O₂, at the same pressure and temperature?

Question

Quizplus · Accepted Answer

The balanced chemical equation is:2H₂ + O₂ → 2H₂OAccording to the ideal gas law, PV = nRT, the number of moles of a gas is directly proportional to its volume at constant temperature and pressure. Therefore, the mole ratio of the reactants and products can be used to determine the volume of H₂O produced.From the balanced equation, we can see that 2 moles of H₂ react with 1 mole of O₂ to produce 2 moles of H₂O. Therefore, the mole ratio of H₂ to H₂O is 2:2, or 1:1. This means that for every 1 mole of H₂ that reacts, 1 mole of H₂O is produced.Since we have 1.12 L of H₂ and 1.12 L of O₂, we can convert these volumes to moles using the ideal gas law:n = PV/RTAt 150 °C and 1.00 atm, the value of RT is:RT = (0.0821 L atm / mol K) * (150 + 273) K = 33.6 L atm / molTherefore, the number of moles of H₂ is:n(H₂) = (1.12 L) * (1 atm) / (33.6 L atm / mol) = 0.0333 molAnd the number of moles of O₂ is:n(O₂) = (1.12 L) * (1 atm) / (33.6 L atm / mol) = 0.0333 molSince the mole ratio of H₂ to H₂O is 1:1, the number of moles of H₂O produced is also 0.0333 mol.Finally, we can convert the number of moles of H₂O to volume using the ideal gas law:V(H₂O) = n(H₂O) * RT / P = (0.0333 mol) * (33.6 L atm / mol) / (1 atm) = 1.12 LTherefore, the volume of H₂O gas produced is 1.12 L.

What Volume of H2O Gas Is Produced at 150 °

What Volume of H₂O Gas Is Produced at 150 °