Consider the following statements regarding the synthesis of ammonia via Haber's process: Statement I: 1 mole of N₂ reacts with 3 moles of H₂ to give 2 moles of NH₃ . Statement II: 22.4 L of N₂ at STP reacts completely with 67.2 L of H₂ at STP to give 44.8 L of NH₃ . Statement III: 28 g of N₂ reacts completely with 6 g of H₂ to give 34 g of NH₃ . Statement IV: If equal masses of N₂ and H₂ are taken, N₂ will act as th

Step-by-step solution

The balanced chemical equation for Haber's process is: N₂(g) + 3H₂(g) 2NH₃(g) Statement I is correct as the stoichiometric coefficients directly give the molar ratio: 1 mole of N₂ reacts with 3 moles of H₂ to produce 2 moles of NH₃ . Statement II is correct because at STP, 1 mole of any ideal gas occupies 22.4 L. Thus, 1 22.4 L of N₂ reacts with 3 22.4 L ( 67.2 L) of H₂ to yield 2 22.4 L ( 44.8 L) of NH₃ . Statement III is correct as the molar mass of N₂ is 28 g/mol, H₂ is 2 g/mol, and NH₃ is 17 g/mol. Therefore, 2