Balance the chemical equation given below,and calculate the volume of nitrogen monoxide gas produced when 8.00 g of ammonia is reacted with 9.00 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

First, balance the chemical equation: 4NH3(g) + 5O2(g) → 4NO(g) + 6H2O(l). Then, calculate moles of NH3 (8.00 g / 17.03 g/mol = 0.47 mol) and O2 (9.00 g / 32.00 g/mol = 0.28 mol). The limiting reactant is O2, which produces 0.28 mol * (4 mol NO / 5 mol O2) = 0.224 mol NO. The volume of NO at 25°C is 0.224 mol * 24.45 L/mol (using ideal gas law at room temperature) = 5.48 L, which rounds to 5.49 L when considering the density of NO is 1.23 g/L for conversion if needed.

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