Nitrogen gas and hydrogen gas are reacted to form ammonia via the Haber process. If 140.0 g of N ₂ is allowed to react with 24.0 g of H ₂ and the percentage yield of the reaction is 75 % , the actual mass of ammonia produced in grams is _______. (Given molar masses: N = 14.0 g mol ⁻¹ , H = 1.0 g mol ⁻¹ )

Step-by-step solution

The balanced chemical equation for the Haber process is: N ₂ + 3 H ₂ 2 NH ₃ Molar mass of N ₂ = 28.0 g mol ⁻¹ Molar mass of H ₂ = 2.0 g mol ⁻¹ Molar mass of NH ₃ = 17.0 g mol ⁻¹ Initial moles of N ₂ = 140.0 28.0 = 5 moles Initial moles of H ₂ = 24.0 2.0 = 12 moles To find the limiting reagent, divide the moles by their stoichiometric coefficients: For N ₂ : 5 1 = 5 For H ₂ : 12 3 = 4 Since 4 Theoretical moles of NH ₃ produced = 2 3 ( moles of H ₂) = 2 3 12 = 8 moles Theoretical mass of NH ₃ = 8 17.0 = 136 g Given t