Aspirin can be prepared in the chemistry laboratory by the reaction of salicylic acid with acetic anhydride. What volume of acetic anhydride is required to produce one killogram of aspirin assuming 100%yield

To determine the volume of acetic anhydride required to produce one kilogram of aspirin, we need to use the molar masses and stoichiometry of the reaction.

1. First, let's find the molar mass of salicylic acid (C7H6O3) and acetic anhydride (C4H6O3).
- Molar mass of salicylic acid (C7H6O3) = (12.01 g/mol x 7) + (1.01 g/mol x 6) + (16.00 g/mol x 3) = 138.12 g/mol
- Molar mass of acetic anhydride (C4H6O3) = (12.01 g/mol x 4) + (1.01 g/mol x 6) + (16.00 g/mol x 3) = 102.09 g/mol

2. Next, determine the molar mass of aspirin (C9H8O4) and calculate the number of moles needed to produce one kilogram of aspirin.
- Molar mass of aspirin (C9H8O4) = (12.01 g/mol x 9) + (1.01 g/mol x 8) + (16.00 g/mol x 4) = 180.16 g/mol
- Number of moles of aspirin = mass of aspirin (in grams) / molar mass of aspirin = 1000 g / 180.16 g/mol = 5.55 mol

3. Now, let's write the balanced chemical equation for the reaction between salicylic acid and acetic anhydride to produce aspirin:
C7H6O3 + C4H6O3 → C9H8O4

4. By examining the stoichiometry of the balanced equation, we can determine the mole ratio between acetic anhydride and aspirin. From the equation, we see that 1 mol of acetic anhydride reacts with 1 mol of aspirin.

5. Since we know the number of moles of aspirin needed (5.55 mol), the same number of moles of acetic anhydride is required.

6. Finally, we need to determine the volume of acetic anhydride using its concentration (expressed in mol/L). Suppose we have a solution with a concentration of X mol/L, to calculate the volume, we can use the equation:
Volume (in L) = Number of moles / Concentration (in mol/L)

Therefore, to determine the volume of acetic anhydride, we need to know its concentration in the laboratory.