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Answer :
Final answer:
To produce 1.3 x 10^2 kg of aspirin, one would require approximately 100 kg of salicylic acid, given the stoichiometry of the reaction. Thus, none of the provided options are correct.
Explanation:
This question involves stoichiometry in chemistry. If we look at the provided equation : C7H6O3 + C4H6O3 → C9H8O4 + HC2H3O2, we can see that one mole of salicylic acid, C7H6O3 reacts to form one mole of aspirin, C9H8O4; they are in a 1:1 ratio. To find how much salicylic acid is required to produce 1.3 x 102 kg of aspirin, we need to convert the mass of aspirin to moles using its molar mass, and then use the stoichiometric ratio to find the moles (and then mass) of salicylic acid.
First, convert mass of aspirin to moles: 1.3 x 102 kg aspirin * 1000 g/kg / 180.157 g/mol = C9H8O4 = ~721 moles of aspirin. Given the 1:1 ratio of reactant to product, we need 721 moles of C7H6O3 (salicylic acid).
Convert this to mass: 721 moles of C7H6O3 * 138.121 g/mol = C7H6O3 = ~99590 g, or ~99.59 kg of salicylic acid, which is approximately 100 kg. Thus, none of the given options are correct if the stoichiometry of the reaction is respected.
Learn more about Chemical Stoichiometry here:
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