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Chapter 3: Problem 129

Acetaminophen, an analgesic and antipyretic drug, has a molecular mass of 151.2 u and a mass percent composition of \(63.56 \%\) C \(, 6.00 \%\) H, \(9.27 \%\) N, and \(21.17 \%\) O. What is the molecular formula of acetaminophen?

Short Answer

Expert verified
The molecular formula of acetaminophen is \(C_8H_9NO_2\).

Step by step solution

01

Convert mass percentages to grams

Since percentage is a part of 100, it implies that for each 100g of the compound, there's \(63.56g\) of C, \(6.00g\) of H, \(9.27g\) of N, and \(21.17g\) of O.
02

Convert grams to moles

Use atomic masses to convert these quantities in grams to moles. These conversions are as follows: C: \(63.56g \div 12.01g/mol = 5.29mol,\) H: \(6.00g \div 1.008g/mol = 5.95mol,\) N: \(9.27g \div 14.01g/mol = 0.66mol,\) O: \(21.17g \div 16.00g/mol = 1.32mol.\)
03

Find ratio of moles

To find the molecular formula, it's necessary to find the mole ratio. To do this, divide all quantities by the smallest quantity found in the previous step. This gives: C: \(5.29 \div 0.66 = 8,\) H: \(5.95 \div 0.66 = 9,\) N: \(0.66 \div 0.66 = 1,\) O: \(1.32 \div 0.66 = 2.\) This yields the empirical formula: \(C_8H_9NO_2.\)
04

Compare empirical to molecular formula

To find the molecular formula, compare the molecular mass to the empirical formula mass. The empirical formula weighs about 151.2 g/mol. Since the empirical formula mass and the molar mass are the same, the empirical formula is therefore the molecular formula.

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Most popular questions from this chapter

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