The reaction N₂ + 3 H₂ → 2 NH₃ is used to produce ammonia.When 450.g of hydrogen was reacted with nitrogen,1575 g of ammonia were produced.What is the percent yield of this reaction?

Question

Quizplus · Accepted Answer

The percent yield is calculated using the formula: (actual yield/theoretical yield) * 100. First, we need to find the molar mass of hydrogen (H2) and ammonia (NH3). The molar mass of H2 is approximately 2.02 g/mol, and for NH3, it is approximately 17.03 g/mol. Given 450 g of hydrogen, we have 450 g / 2.02 g/mol = 222.77 mol of hydrogen. According to the balanced chemical equation, 3 moles of hydrogen produce 2 moles of ammonia. Therefore, the theoretical yield of ammonia is (222.77 mol H2 * 2 mol NH3 / 3 mol H2) = 148.51 mol NH3. Converting moles of NH3 to grams gives us 148.51 mol * 17.03 g/mol = 2528.5 g of NH3 as the theoretical yield. The actual yield is 1575 g. Thus, the percent yield = (1575 g / 2528.5 g) * 100 = 62.3%. The closest answer is 62.1%.

The Reaction N2 + 3 H2 → 2 NH3 Is

The Reaction N₂ + 3 H₂ → 2 NH₃ Is