Balance the chemical equation given below,and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 12.0 g of oxygen at 25°C? The density of nitrogen monoxide at 25°C is 1.23 g/L.
_____ NH₃(g) + _____ O₂(g) → _____ NO(g) + _____ H₂O(l)

Question

Quizplus · Accepted Answer

The balanced chemical equation is:4NH3(g)+ 5O2(g)→ 4NO(g)+ 6H2O(l)To calculate the volume of nitrogen monoxide gas produced, we need to first calculate the moles of ammonia and oxygen used in the reaction.Moles of ammonia = 8.00 g / 17.03 g/mol = 0.470 molMoles of oxygen = 12.0 g / 32.00 g/mol = 0.375 molAccording to the balanced chemical equation, 4 moles of ammonia react with 5 moles of oxygen. Therefore, oxygen is the limiting reactant in this reaction.Moles of nitrogen monoxide produced = 0.375 mol * (4 mol NO / 5 mol O2) = 0.300 molVolume of nitrogen monoxide produced = 0.300 mol * 22.4 L/mol = 6.72 LHowever, the density of nitrogen monoxide at 25°C is 1.23 g/L. Therefore, the volume of nitrogen monoxide gas produced at 25°C is:Volume = Mass / Density = (0.300 mol * 30.01 g/mol) / 1.23 g/L = 7.32 LTherefore, the correct answer is A) 7.32 L.

Balance the Chemical Equation Given Below,and Calculate the Volume of Nitrogen