What volumes of hydrogen and nitrogen will be required to obtain such an amount of NH3
What volumes of hydrogen and nitrogen will be required to obtain such an amount of NH3, when interacting with an excess of HNO3, 20 g of salt is obtained?
1. We write down the equation of reactions.
NH3 + HNO3 → NH4NO3.
We find the mass of ammonia according to the reaction equation.
M (NH3) = 14 + 1 × 3 = 17 g / mol.
M (NH4NO3) = 14 + 4 + 14 + 48 = 80 g / mol.
X g NH3 – 20 g NH4NO3.
17 g / mol NH3 – 80 g / mol NH4NO3.
X = 17 × 20: 80 = 4.25 g NH3.
Find the molar mass of ammonia.
n = m / M.
n = 4.25 / 17 = 0.25 mol.
2. We write down the equation of reactions.
N2 + 3H2 = 2NH3.
We find the amount of the substance nitrogen and hydrogen.
X mol N2 – 0.25 mol NH3
1 mol N2 – 2 mol NH3
X = 1 × 0.25: 2 = 0.125 mol.
V = n × Vm = 0.125 mol × 22.4 L / mol = 2.8 L N2.
X (H2) = 3 × 0.125: 2 = 0.1875 mol.
V (H2) = 0.1875 mol × 22.4 L / mol = 4.2 L.
Answer: the volume of nitrogen is 2.8 liters; the volume of hydrogen is 4.2 liters.