Question

Aspirin is a common analgesic. If you want to produce 500. mg of aspirin (C9H8O4, m.w. = 180.16 g/mol) from the reaction of C7H6O3 (m.w. = 130.12 g/mol) and C4H6O3 (m.w. = 102.09 g/mol), what is the minimum amount of C4H6O3 that is needed?2C7H6O3(s) + C4H6O3(l) → 2C9H8O4(s) + H2O(l)

Answer 1

1) First, let's rewrite the chemical equation here:

2 C7H6O3(s) + C4H6O3(l) → 2 C9H8O4(s) + H2O(l)

2) Let's find out how many moles of C9H8O4 have into 500 mg of it. For this, use ese the following equation:

mole = mass/ molar mass

mass = 500 mg = 0.5 g

molar mass of C9H8O4 = 180.16 g/mol (the question give it to us)

mole = 0.5/180.16

mole = 0.0028 moles of C9H8O4

3) Using the chemical equation proportion, we can discover the amount in moles of C4H6O3 needed to form 0.0028 moles of C9H8O4. So:

1 mol of C4H6O3 forms 2 moles of C9H8O4

x mol of C4H6O3 forms 0.0028 moles of C9H8O4

2x = 0.0028

x = 0.0014 moles of C4H6O3

4) We need to find the answer in grams. Let's transform 0.0014 moles of C4H6O3 into grams. For this, use ese the following equation:

mass = mole × molar mas

mass = 0.0014 moles × 102.09

mass = 0.142 grams or 1.42x10⁻¹

Answer: The amount of C4H6O3 that is needed is 1.42x10⁻¹ g.