Question

what mass (in grams) of aspirin (c₉h₈o₄) is produced from 78.9 g of c₇h₆o₃ assuming 95.0% yield from the reaction below?c₇h₆o₃(s)+c₄h₆o₃(l)→c₉h₈o₄(s)+hc₂h₃o₂(aq).

Answer 1

To find the mass of aspirin produced from 78.9 g of C7H6O3, we calculate the moles of C7H6O3, use the molar mass of aspirin to find the theoretical yield, and then apply the 95.0% yield to get an actual yield of 97.72 grams.

Step-by-step explanation:

To calculate the mass of aspirin produced from 78.9 g of C7H6O3 with a 95.0% yield, we must first use stoichiometry to determine the theoretical yield of aspirin, based on the molecular weights of the reactant (C7H6O3) and the product (C9H8O4), and then adjust for the actual yield. The molecular mass of aspirin (C9H8O4) is 180.15 g/mol. Using the equation C7H6O3(s) + C4H6O3(l) → C9H8O4(s) + HC2H3O2(aq), we establish a 1:1 mole ratio between C7H6O3 and C9H8O4.

First, we need to determine how many moles of C7H6O3 we have:

• The molecular mass of C7H6O3 is 138.12 g/mol.
• Moles of C7H6O3 = Mass / Molecular mass = 78.9 g / 138.12 g/mol = 0.571 moles.

Next, applying the stoichiometry of the reaction, we assume that 1 mole of C7H6O3 produces 1 mole of C9H8O4:

• Theoretical yield of aspirin = Moles of C7H6O3 x Molecular mass of C9H8O4 = 0.571 moles x 180.15 g/mol = 102.86 g.
• Accounting for the 95.0% yield, the actual yield = Theoretical yield x Percentage yield = 102.86 g x 0.95 = 97.72 g.

Therefore, the mass of aspirin produced is 97.72 grams.