10.0 g of gaseous ammonia and 6.50 g of oxygen gas are introduced into a previously evacuated 5.50 l vessel. if the ammonia and oxygen then react to yield no gas and water vapor, what is the final gas pressure inside the vessel at 23? c

3.54 × 10⁵ Pa.

Explanation

Ammonia NH₃ and oxygen gas O₂ reacts at a one-to-one molar ratio to produce NO and H₂O.

NH₃ + O₂ → NO + H₂O (Balanced)

NH₃ has a molar mass of 17.03 g/mol. 10.0 g of NH₃ contains 0.5872 mol molecules.O₂ has a molar mass of 32.00 g/mol. 6.50 g of H₂O contains 0.2031 mol molecules.H₂O is the limiting reactant. All 0.2031 mol of O₂ will be consumed. Only 0.2031 mol of NH₃ will be consumed. 0.5872 - 0.2031 = 0.3841 mol of NH₃ will be in excess. The reaction will produce 0.2031 mol of NO and 0.2031 mol of H₂O.

The vessel will contain

0.3841 mol NH₃,0 mol O₂,0.2031 mol NO, and0.2031 mol H₂O.

It will contain 0.3841 + 0.2031 + 0.2031 = 0.7903 mol gas particles by the end of the reaction.

Assuming that the final mixture is an ideal gas, it will exert a pressure of 3.54 × 10⁵ Pa on the container.

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