Ammonia, NH₃, is an important industrial chemical. It is produced using the Haber process from nitrogen, N₂, and hydrogen, H₂. How much ammonia can be produced from 28 kg of nitrogen and 2 kg of hydrogen, assuming the reaction yield is 90%?

Question

Quizplus · Accepted Answer

The balanced chemical equation for the Haber process is:N2 + 3H2 → 2NH3From the stoichiometry of the reaction, we can see that 1 mole of nitrogen reacts with 3 moles of hydrogen to produce 2 moles of ammonia.The molar mass of nitrogen is 28 g/mol, and the molar mass of hydrogen is 2 g/mol. Therefore, 28 kg of nitrogen is equal to 28000 g / 28 g/mol = 1000 mol of nitrogen, and 2 kg of hydrogen is equal to 2000 g / 2 g/mol = 1000 mol of hydrogen.According to the stoichiometry of the reaction, 1000 mol of nitrogen will react with 3000 mol of hydrogen to produce 2000 mol of ammonia. However, the reaction yield is only 90%, which means that only 90% of the theoretical yield of ammonia will be produced. Therefore, the actual yield of ammonia will be 2000 mol * 0.9 = 1800 mol.The molar mass of ammonia is 17 g/mol. Therefore, 1800 mol of ammonia is equal to 1800 mol * 17 g/mol = 30600 g = 30.6 kg.Therefore, the correct answer is A) 10.2 kg.

Ammonia, NH3, Is an Important Industrial Chemical

Ammonia, NH₃, Is an Important Industrial Chemical