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Ch. 2 Chemistry Comes Alive
Hoehn - Marieb Human Anatomy & Physiology, 12th edition
Hoehn, Haynes, Abbott12th EditionMarieb Human Anatomy & PhysiologyISBN: 9780138242732Not the one you use?Change textbook
All textbooksHoehn, Haynes, Abbott 12th EditionCh. 2 Chemistry Comes AliveProblem 17
Chapter 2, Problem 17

How many moles of aspirin, C₉H₈O₄, are in a bottle containing 450 g by weight? (Note: The approximate atomic weights of its atoms are C = 12, H = 1, and O = 16.)

Verified step by step guidance
1
Identify the molecular formula of aspirin, which is C\_9H\_8O\_4, and note the atomic weights: C = 12, H = 1, O = 16.
Calculate the molar mass of aspirin by multiplying the number of each type of atom by its atomic weight and summing the results: \(\text{Molar mass} = (9 \times 12) + (8 \times 1) + (4 \times 16)\).
Sum the values from the previous step to find the total molar mass of one mole of aspirin in grams per mole (g/mol).
Use the formula to find the number of moles: \(\text{moles} = \frac{\text{mass of sample (g)}}{\text{molar mass (g/mol)}}\).
Substitute the given mass of aspirin (450 g) and the calculated molar mass into the formula to determine the number of moles in the bottle.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molar Mass

Molar mass is the mass of one mole of a substance, calculated by summing the atomic masses of all atoms in its molecular formula. For aspirin (C₉H₈O₄), multiply the number of each atom by its atomic weight and add them to find the molar mass in grams per mole.
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Mole Concept

A mole represents 6.022 × 10²³ particles (atoms, molecules, etc.) of a substance. It links the microscopic scale of atoms to the macroscopic scale of grams, allowing conversion between mass and number of molecules using the molar mass.
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Mass to Moles Conversion

To find the number of moles from a given mass, divide the mass of the substance by its molar mass. This calculation converts the weight of aspirin in grams to the amount in moles, which is essential for stoichiometric and quantitative chemical analysis.
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Related Practice
Textbook Question

Which of the following covalently bonded molecules are polar?

(a)

(b)

(c)

(d)

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Textbook Question

Identify each reaction as one of the following:

a. A synthesis reaction

b. A decomposition reaction

c. An exchange reaction

(1) 2Hg + O₂ → 2HgO

(2) HCl + NaOH → NaCl + H₂O

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Textbook Question

A chemist, during the course of an analysis, runs across a chemical composed of carbon, hydrogen, and oxygen in the proportion 1:2:1 and having a six-sided molecular shape. It is probably:

a. A pentose

b. An amino acid

c. A fatty acid

d. A monosaccharide

e. A nucleic acid

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Textbook Question

What are hydrogen bonds and how are they important in the body?

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Textbook Question

Differentiate clearly between primary, secondary, and tertiary protein structure.

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Textbook Question

Consider the following information about three atoms: 12/6 C 13/6 C 14/6 C

a. How are they similar to one another?

b. How do they differ from one another?

c. What are the members of such a group of atoms called?

d. Using the planetary model, draw the atomic configuration of 12/6 C, showing the relative position and numbers of its subatomic particles

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