/*! This file is auto-generated */ .wp-block-button__link{color:#fff;background-color:#32373c;border-radius:9999px;box-shadow:none;text-decoration:none;padding:calc(.667em + 2px) calc(1.333em + 2px);font-size:1.125em}.wp-block-file__button{background:#32373c;color:#fff;text-decoration:none} Problem 9 When you let air out of a tire, ... [FREE SOLUTION] | 91影视

91影视

Log out

Learning Materials

Features

Discover

Chapter 18: Problem 9

When you let air out of a tire, the air seems cool. Why? What kind of process is occurring?

Short Answer

Expert verified
The air feels cool because it is undergoing an adiabatic process. The sudden decrease in pressure as it's released from the tire causes its temperature to drop, making it feel cool. This is characterized by the formula \( P_1/T_1 = P_2/T_2 \), signifying that the decrease in pressure leads to a corresponding decrease in temperature.

Step by step solution

01

Understand Gas Behavior

Remember that temperature and gas pressure are related. The change in temperature of a gas is directly proportional to its change in pressure, according to Guy-Lussac's law. Inside the tire, the air is under high pressure. When the air is released, it expands and the pressure drops.
02

Connect Pressure and Temperature Changes

Because the pressure and temperature of the gas are related, the decrease in pressure as the gas expands leads to a corresponding decrease in temperature. This relationship is described by the formula \( P_1/T_1 = P_2/T_2 \), where \( P_1 \) and \( T_1 \) are the initial pressure and temperature, and \( P_2 \) and \( T_2 \) are the final pressure and temperature.
03

Identify the Process

This kind of process is an adiabatic process, a type of thermodynamic process in which no heat transfer occurs between the system (in this case, the air in the tire) and its surroundings. In an adiabatic expansion, which is what happens when air is released from a tire, the gas does work on its surroundings and loses an equivalent amount of internal energy, resulting in a decrease of temperature in the gas.

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.

Over 30 million students worldwide already upgrade their learning with 91影视!

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

A gasoline engine has compression ratio 8.5 (see Example 18.3 for the meaning of this term), and the fuel-air mixture compresses adiabatically with \(\gamma=1.4 .\) If the mixture enters the engine at \(30^{\circ} \mathrm{C},\) what will its temperature be at maximum compression?

Nitrogen gas \((\gamma=1.4)\) at \(18^{\circ} \mathrm{C}\) is compressed adiabatically until its volume is reduced to one-fourth of its initial value. By how much does its temperature increase?

A gas mixture contains monatomic argon and diatomic oxygen. An adiabatic expansion that doubles its volume results in the pressure dropping to one- third of its original value. What fraction of the molecules are argon?

Monatomic argon gas is initially at a chilly \(28 \mathrm{K}\). By what factor would you have to increase its pressure, adiabatically, to bring it to room temperature \((293 \mathrm{K}) ?\)

How much of a triatomic gas with \(C_{V}=3 R\) would you have to add to 10 mol of monatomic gas to get a mixture whose thermodynamic behavior was like that of a diatomic gas?
See all solutions

Recommended explanations on Physics Textbooks

Measurements

Read Explanation

Linear Momentum

Read Explanation

Physics of Motion

Read Explanation

Modern Physics

Read Explanation

Astrophysics

Read Explanation

Conservation of Energy and Momentum

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.