Answer :
Final answer:
The amount of salicylic acid needed to produce a specific amount of aspirin can be calculated using molar masses and stoichiometry principles. Adjustments need to be made for efficiency percentages, and theoretical and actual yields can also be determined following the same steps.
Explanation:
This is a stoichiometry problem, and it requires finding the molar mass of both aspirin (C₉H₈O₄) and salicylic acid (C₇H₆O₃). The molar mass of aspirin is approximately 180.16 g/mol, and the molar mass of salicylic acid is approximately 138.12 g/mol. We know that the reaction uses one mole of salicylic acid to produce one mole of aspirin.
(a) The amount of salicylic acid needed to produce 2.4x10² kg of aspirin is determined by first converting kg to grams then using the molar masses to convert grams to moles and finally using stoichiometry to determine the moles of salicylic acid. (b) If only 51% of the salicylic acid gets converted to aspirin, the initial required amount should be almost doubled. (c) The theoretical yield of aspirin depends on the initial amounts of the reactants, in this case, salicylic acid and acetic anhydride. Given the initial masses, we first convert the mass to moles, then using stoichiometry, we determine the limiting reactant and use it to calculate the theoretical yield. If 191 kg of aspirin were produced, then the percentage yield is actually the ratio of actual yield to theoretical yield multiplied by 100.
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