Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 5: Problem 70

The molecular formula of acetylsalicylic acid (aspirin), one of the most commonly used pain relievers, is \(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\) a. Calculate the molar mass of aspirin. b. A typical aspirin tablet contains \(500 . \mathrm{mg} \mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4} .\) What amount (moles) of \(\mathrm{C}_{9} \mathrm{H}_{8} \mathrm{O}_{4}\) molecules and what number of molecules of acetylsalicylic acid are in a 500.-mg tablet?

Short Answer

Expert verified
a. The molar mass of aspirin (C9H8O4) is 180.17 g/mol. b. A 500 mg tablet has approximately 0.00277 mol of C9H8O4 molecules, which corresponds to \(1.67 \times 10^{21}\) acetylsalicylic acid molecules.

Step by step solution

01

Calculate the molar mass of aspirin (C9H8O4)

First, we need to find the molar mass of each element in acetylsalicylic acid and then add them together to determine the molar mass of the compound. The molar mass of carbon (C) is 12.01 g/mol, hydrogen (H) is 1.01 g/mol, and oxygen (O) is 16.00 g/mol. So, Molar mass of C9H8O4 = (9 * 12.01) + (8 * 1.01) + (4 * 16.00)
02

Calculate the total molar mass

Calculate the total molar mass of C9H8O4: Molar mass = (9 * 12.01) + (8 * 1.01) + (4 * 16.00) Molar mass = 108.09 + 8.08 + 64.00 Molar mass = 180.17 g/mol The molar mass of aspirin (C9H8O4) is 180.17 g/mol. a. Answer: The molar mass of aspirin is 180.17 g/mol.
03

Convert tablet mass to moles

Now, we have to find out the amount (moles) of C9H8O4 molecules in a 500 mg tablet. First, convert the mass from mg to g: 500 mg = 0.5 g Now, use the molar mass to convert the mass of the tablet into moles: moles = mass (g) / molar mass (g/mol) moles = 0.5 g / 180.17 g/mol
04

Calculate the number of moles

Calculating the number of moles of C9H8O4 in a 500 mg tablet: moles = 0.5 g / 180.17 g/mol moles ≈ 0.00277 mol b. Answer (1): The amount of C9H8O4 molecules in a 500 mg tablet is approximately 0.00277 mol.
05

Find the number of acetylsalicylic acid molecules

Now, we need to find the number of acetylsalicylic acid molecules in a 500 mg tablet. To do this, we must multiply the number of moles by Avogadro's number (6.022 x 10^23). Number of molecules = moles * Avogadro's number Number of molecules ≈ 0.00277 mol * 6.022 x 10^23
06

Calculate the total number of molecules

Calculate the total number of acetylsalicylic acid molecules in a 500 mg tablet: Number of molecules ≈ 0.00277 mol * 6.022 x 10^23 Number of molecules ≈ 1.67 x 10^21 b. Answer (2): There are approximately \(1.67 \times 10^{21}\) molecules of acetylsalicylic acid (aspirin) in a 500 mg tablet.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Some bismuth tablets, a medication used to treat upset stomachs, contain \(262 \mathrm{mg}\) of bismuth subsalicylate, \(\mathrm{C}_{7} \mathrm{H}_{5} \mathrm{BiO}_{4},\) per tablet. Assuming two tablets are digested, calculate the mass of bismuth consumed.

Determine the molecular formula of a compound that contains \(26.7 \% \mathrm{P}, 12.1 \% \mathrm{N},\) and \(61.2 \% \mathrm{Cl},\) and has a molar mass of \(580 \mathrm{g} / \mathrm{mol}.\)

A sample of urea contains \(1.121 \mathrm{g} \mathrm{N}, 0.161 \mathrm{g} \mathrm{H}, 0.480 \mathrm{g} \mathrm{C}\) and \(0.640 \mathrm{g}\) O. What is the empirical formula of urea?

Ammonia is produced from the reaction of nitrogen and hydrogen according to the following balanced equation: $$\mathrm{N}_{2}(g)+3 \mathrm{H}_{2}(g) \longrightarrow 2 \mathrm{NH}_{3}(g)$$ a. What is the maximum mass of ammonia that can be produced from a mixture of \(1.00 \times 10^{3} \mathrm{g} \mathrm{N}_{2}\) and \(5.00 \times 10^{2} \mathrm{g} \mathrm{H}_{2} ?\) b. What mass of which starting material would remain unreacted?

The reaction of ethane gas \(\left(\mathrm{C}_{2} \mathrm{H}_{6}\right)\) with chlorine gas produces \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}\) as its main product (along with HCl). In addition, the reaction invariably produces a variety of other minor products, including \(\mathrm{C}_{2} \mathrm{H}_{4} \mathrm{Cl}_{2}, \mathrm{C}_{2} \mathrm{H}_{3} \mathrm{Cl}_{3},\) and others. Naturally, the production of these minor products reduces the yield of the main product. Calculate the percent yield of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}\) if the reaction of \(300 .\) g of ethane with \(650 .\) g of chlorine produced \(490 .\) g of \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{Cl}.\)
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Kinetics

Read Explanation

Chemistry Branches

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Nuclear Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free