Answer: A
Step-by-step explanation:
To determine the percentage yield of ammonia in this reaction, we need to know the theoretical work of ammonia, which is the maximum amount of ammonia that could be produced based on the reaction's stoichiometry. The balanced chemical equation for the reaction tells us that for every 2 moles of ammonia produced, 3 moles of hydrogen are consumed. Suppose we know the mass of hydrogen that is used in the reaction. In that case, we can use the molar mass of hydrogen to determine the number of moles of hydrogen consumed and then use the balanced chemical equation to determine the theoretical yield of ammonia. In this case, we are given that 60 kg of hydrogen is used in the reaction. The molar mass of hydrogen is 1.008 g/mol, so the number of hydrogen used in the response is 60 kg / 1.008 g/mol = 59.5 moles. The balanced chemical equation tells us that for every 3 moles of hydrogen consumed, 2 moles of ammonia are produced, so the theoretical yield of ammonia in this reaction is 2 moles NH3/3 moles H2 * 59.5 moles H2 = 39.7 moles NH3. The molar mass of ammonia is 17.031 g/mol, so the theoretical yield of ammonia in this reaction is 39.7 moles * 17.031 g/mol = 675.9 kg. To determine the percentage yield, we divide the actual yield (60 kg) by the theoretical work (675.9 kg) and multiply by 100%. This gives us a percentage yield of 60 kg / 675.9 kg * 100% = 8.85%. Therefore, the correct answer is A) 5.9%.