Question

What is the theoretical yield of C9H8O4 when 3.03 g of C₇H₆O₃reacts with 4.01 g of C₇H₆O₃?

C₇H₆O₃=138.1 g/mol, C4H6O3= 102.1 g/mol, C9H8O4= 180.2 g/mol
C₇H₆O₃(s)+C₄H₆O₃(l) → C₉H₈O₄(S) + C₂H₄O₂(l)

Answer 1

To calculate the theoretical yield of C9H8O4, you need to determine the limiting reactant. Convert the given masses of C7H6O3 and C4H6O3 to moles, compare the moles to find the limiting reactant, and then use the mole ratio from the balanced equation to calculate the moles of C9H8O4.

Step-by-step explanation:

To calculate the theoretical yield of C9H8O4, we need to determine the limiting reactant. First, we convert the given masses of C7H6O3 to moles by dividing by its molar mass, which is 138.1 g/mol. We do the same for C4H6O3, which has a molar mass of 102.1 g/mol.

Next, we compare the moles of C7H6O3 and C4H6O3 to find the limiting reactant. The reactant that produces fewer moles of C9H8O4 is the limiting reactant. Finally, we use the mole ratio from the balanced equation to calculate the moles of C9H8O4 that can be produced. We then convert moles to grams using the molar mass of C9H8O4, which is 180.2 g/mol.

The balanced equation given is: C7H6O3(s) + C4H6O3(l) → C9H8O4(s) + C2H4O2(l)

Let's follow the steps to calculate the theoretical yield:

1. Convert the mass of C7H6O3 to moles: 3.03 g ÷ 138.1 g/mol = 0.02197 mol.
2. Convert the mass of C4H6O3 to moles: 4.01 g ÷ 102.1 g/mol = 0.03931 mol.
3. Compare the moles of C7H6O3 and C4H6O3 to find the limiting reactant. Since C7H6O3 produces fewer moles of C9H8O4, it is the limiting reactant.
4. Use the mole ratio from the balanced equation to calculate the moles of C9H8O4 produced. From the equation, we see that 1 mole of C7H6O3 produces 1 mole of C9H8O4, so we have 0.02197 mol of C9H8O4.
5. Finally, convert moles to grams using the molar mass of C9H8O4: 0.02197 mol × 180.2 g/mol ≈ 3.96 g.