Equimolar amounts of the gases N₂ and H₂ are mixed in a closed container fitted with a piston (allowing the volume of the container to change, thus keeping the pressure constant). Calculate the ratio of the final volume of the container to the initial volume of the container when the reaction N₂ + 3H₂ → 2NH₃ goes to completion.

Question

Quizplus · Accepted Answer

According to the balanced chemical equation, for every mole of N₂ that reacts, 3 moles of H₂ are consumed and 2 moles of NH₃ are produced. Therefore, the number of moles of gas in the container does not change during the reaction. Since the pressure is constant, the ideal gas law (PV = nRT) can be used to relate the initial and final volumes of the container: (PV)initial = nRT (PV)final = nRT Dividing the second equation by the first: PV/PV = (nRT)/(nRT) Vfinal/Vinitial = 1 Therefore, the ratio of the final volume to the initial volume is 1, or equivalently, the final volume is equal to the initial volume.

Equimolar Amounts of the Gases N2 and H2 Are Mixed

Equimolar Amounts of the Gases N₂ and H₂ Are Mixed