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Chapter 3: Problem 23

Determine the mass percent of each of the elements in the antimalarial drug quinine, \(\mathrm{C}_{20} \mathrm{H}_{24} \mathrm{N}_{2} \mathrm{O}_{2}\)

Short Answer

Expert verified
The percentage composition by mass of each element in quinine, \(\mathrm{C}_{20} \mathrm{H}_{24} \mathrm{N}_{2} \mathrm{O}_{2}\), is computed by the formulas given. The exact values will require calculator usage to complete these calculations.

Step by step solution

01

Compute the Molar Mass of Quinine

The molar mass of quinine is calculated by adding the molar masses of all the atoms in one molecule. Given that Carbon (C) has an atomic weight of approximately 12.01 g/mol, Hydrogen (H) has an approximate atomic weight of 1.008 g/mol, Nitrogen (N) has an atomic weight of approximately 14.01 g/mol, and Oxygen (O) weighs about 16 g/mol yields: \( \text{Molar mass of quinine} = (20 \times 12.01 \, \text{g/mol}) + (24 \times 1.008 \, \text{g/mol}) + (2 \times 14.01 \, \text{g/mol}) + (2 \times 16 \, \text{g/mol}) \)
02

Determine the Molar Mass of Each Element in Quinine

Calculate the molar mass contributed by each element by multiplying the atomic weight of each element by the number of atoms of that element in the molecule. For example, for Carbon: \( \text{Molar mass of C in quinine} = 20 \times 12.01 \, g/mol \). Repeat this for Hydrogen, Nitrogen, and Oxygen.
03

Use the Formula to Calculate Percent Composition

To find the percent composition, divide the molar mass of each element by the molar mass of quinine, and then multiply the result by 100%. For example, for Carbon: \( \text{Percent composition of C} = \left(\frac{\text{Molar mass of C in quinine}}{\text{Molar mass of quinine}}\right) \times 100\% \). Compute this for every element.

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Most popular questions from this chapter

A \(1.013 \mathrm{g}\) sample of \(\mathrm{ZnSO}_{4} \cdot x \mathrm{H}_{2} \mathrm{O}\) is dissolved in water and the sulfate ion precipitated as \(\mathrm{BaSO}_{4}\). The mass of pure, dry \(\mathrm{BaSO}_{4}\) obtained is \(0.8223 \mathrm{g}\). What is the formula of the zinc sulfate hydrate?

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A hydrocarbon mixture consists of \(60.0 \%\) by mass of \(\mathrm{C}_{3} \mathrm{H}_{8}\) and \(40.0 \%\) of \(\mathrm{C}_{x} \mathrm{H}_{y} .\) When \(10.0 \mathrm{g}\) of this mixture is burned, \(29.0 \mathrm{g} \mathrm{CO}_{2}\) and \(18.8 \mathrm{g} \mathrm{H}_{2} \mathrm{O}\) are the only products. What is the formula of the unknown hydrocarbon?

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