Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 12: Problem 28

Ammonia, \(\mathrm{NH}_{3},\) and alcohol, \(\mathrm{C}_{2} \mathrm{H}_{6} \mathrm{O},\) are released together across a room. Which will you smell first?

Short Answer

Expert verified
The smell of ammonia will reach you first because it has a lower molar mass and thus will spread more quickly.

Step by step solution

01

Determine the Molar Masses of the Molecules

The first step is to calculate the molar masses of the molecules. This can be done using the periodic table, where you sum the molar masses of the individual atoms in each molecule. Using this method, it can be determined that the molar mass of ammonia (\(NH_{3}\)) is approx 17 g/mol and that of alcohol (\(C_{2}H_{6}O\)) is approx 46 g/mol.
02

Analyze the Relationship between Molecular Mass and Dispersion

Molecules with lower molar mass tend to move faster and disperse more quickly through a room due to the kinetic molecular theory. This theory states that lighter molecules move at higher speeds, on average, than heavier ones at the same temperature.
03

Compare the Molar Masses of Ammonia and Alcohol

Finally, by comparing the molar masses of ammonia and alcohol, it can be seen that ammonia has a lower molar mass. As such, ammonia molecules will spread faster across the room.

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

How many grams of oxygen gas must be in a 10.0 L container to exert a pressure of 97.0 kPa at a temperature of \(25^{\circ} \mathrm{C} ?\)

Explain Charles's law in terms of the kinetic-molecular theory.

A diver at a depth of \(1.0 \times 10^{2} \mathrm{m},\) where the pressure is 11.0 atm, releases a bubble with a volume of 100.0 \(\mathrm{mL}\) . What is the volume of the bubble when it reaches the surface? Assume a pressure of 1.00 atm at the surface.

A gas at \(65^{\circ} \mathrm{C}\) occupies 4.22 \(\mathrm{L} .\) At what Celsius temperature will the volume be \(3.87 \mathrm{L},\) at the same pressure?

A diver at a depth of \(1.0 \times 10^{2} \mathrm{m},\) where the pressure is 11.0 atm, releases a bubble with a volume of 100.0 \(\mathrm{mL}\) . What is the volume of the bubble when it reaches the surface? Assume a pressure of 1.00 atm at the surface.
See all solutions

Recommended explanations on Chemistry Textbooks

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Reactions

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

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