The Haber process is used to synthesize ammonia from hydrogen and nitrogen. How much hydrogen is required to produce 42.8 kg of ammonia?

Question

Quizplus · Accepted Answer

The balanced chemical equation for the Haber process is N2 + 3H2 → 2NH3. The molar mass of NH3 is 17 g/mol, and for H2, it is 2 g/mol. To produce 42.8 kg (42800 g) of NH3, we need (42800 g / 17 g/mol) = 2517.65 mol of NH3. According to the stoichiometry, 3 moles of H2 are needed for every 2 moles of NH3, so we need (2517.65 mol * 3/2) = 3776.48 mol of H2. The mass of H2 required is (3776.48 mol * 2 g/mol) = 7552.96 g, which is approximately 7.60 kg.

The Haber Process Is Used to Synthesize Ammonia from Hydrogen