A) Which is the limiting reactant? Given the density of acetic anhydride is 1.030 g/ml? b) What is the percent yield of this reaction?

To solve this problem, we first need to determine the molar masses of the reactants and products, then calculate the moles of each reactant to find the limiting reactant, and finally use the limiting reactant to calculate the theoretical yield and percent yield.

The balanced chemical equation is:

$$\text{C}_7\text{H}_6\text{O}_3 + \text{(CH}_3\text{CO)}_2\text{O} \rightarrow \text{C}_9\text{H}_8\text{O}_4 + \text{CH}_3\text{COOH}$$

(Salicylic acid) + (Acetic anhydride) $\rightarrow$ (Aspirin) + (Acetic acid)

Molar masses:

• Salicylic acid ($\text{C}_7\text{H}_6\text{O}_3$):

$$(7 \times 12.01) + (6 \times 1.008) + (3 \times 16.00) = 84.07 + 6.048 + 48.00 = 138.118 \text{ g/mol}$$

• Acetic anhydride ($\text{(CH}_3\text{CO)}_2\text{O}$ or $\text{C}_4\text{H}_6\text{O}_3$):

$$(4 \times 12.01) + (6 \times 1.008) + (3 \times 16.00) = 48.04 + 6.048 + 48.00 = 102.088 \text{ g/mol}$$

• Aspirin ($\text{C}_9\text{H}_8\text{O}_4$):

$$(9 \times 12.01) + (8 \times 1.008) + (4 \times 16.00) = 108.09 + 8.064 + 64.00 = 180.154 \text{ g/mol}$$