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

The balanced chemical equation is:4 NH3(g) + 5 O2(g) → 4 NO(g) + 6 H2O(l)To calculate the volume of nitrogen monoxide gas produced, we can use the ideal gas law:PV = nRTwhere P is the pressure, V is the volume, n is the number of moles, R is the ideal gas constant, and T is the temperature.We know the pressure is 1 atm, the temperature is 25°C (298 K), and the number of moles of ammonia is:n(NH3) = 8.00 g / 17.03 g/mol = 0.470 molAccording to the balanced chemical equation, 4 moles of ammonia react to produce 4 moles of nitrogen monoxide. Therefore, the number of moles of nitrogen monoxide produced is also 0.470 mol.Substituting these values into the ideal gas law, we get:V = nRT/P = (0.470 mol)(0.0821 L·atm/(mol·K))(298 K)/(1 atm) = 11.5 LTherefore, the volume of nitrogen monoxide gas produced is 11.5 L.

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