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A container of n2 03 has a pressure of .420 atm when the absolute pressure of the n2 03 is tripled the gas completely decomposes producing an o2 nno calculate the final pressure of the gas mixture assuming that the container volume does not change.
A container of n2 03 has a pressure of .420 atm when the absolute pressure of the n2 03 is tripled the gas completely decomposes producing an o2 nno calculate the final pressure of the gas mixture assuming that the container volume does not change.
Final answer:To find the final pressure of the gas mixture, we need to add up the partial pressures of the three gases: N₂O, O₂, and NO. Final pressure of the gas mixture is 0.94 atm.Explanation:In this problem, we are given the initial pressures of N₂O and O₂ gases and we need to calculate the final pressures of the three gases (N₂O, O₂, and N₂O).Since the volume of the container does not change, we can use Dalton's Law of Partial Pressures to solve the problem. According to Dalton's Law, the total pressure of the gas mixture is equal to the sum of the individual pressures of each gas.So, in this case, after reaching equilibrium, the final pressures of the three gases will be:Partial pressure of N₂O: 0.62 atmPartial pressure of O₂: 0.24 atmPartial pressure of N₂O: 0.08 atmTo find the final pressure of the gas mixture, we simply add up the partial pressures of the three gases:Final pressure of gas mixture = Partial pressure of N₂O + Partial pressure of O₂ + Partial pressure of N₂O= 0.62 atm + 0.24 atm + 0.08 atm =0.94 atm...