1st Edition

ISBN: 9780078746376

Author: Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom

Publisher: Glencoe/McGraw-Hill School Pub Co

Concept explainers

Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,

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Gaseous State

It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed fo…

Question

Definition Definition Any of various laws that describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. At a constant temperature, the pressure of a particular amount of gas is inversely proportional with its volume (Boyle's Law) In a closed system with constant pressure, the volume of an ideal gas is in direct relation with its temperature (Charles's Law) At a constant volume, the pressure of a gas is in direct relation to its temperature (Gay-Lussac's Law) If the volume of all gases are equal and under the a similar temperature and pressure, then they contain an equal number of molecules (Avogadro's Law) The state of a particular amount of gas can be determined by its pressure, volume and temperature (Ideal Gas law)

Chapter 13, Problem 64A

Interpretation Introduction

Interpretation:

A ideal gas is to be defined and the reason why there is no true ideal gas in nature is to be justified.

Concept introduction:

The concept of ideal gas is studied by kinetic gas theory.

Expert Solution & Answer

Answer to Problem 64A

A gas is ideal if it follows all the gas laws at all temperature and pressure.

There is no ideal gas in nature because all gases follow ideal gas equation at low temperature and high pressure and deviates from ideal behavior at high temperature and low pressure.

Explanation of Solution

According to kinetic molecular theory, an ideal gas should follow:

Volume occupied by a molecule should be negligible as compared to total volume of gas.
There should be no attractive forces between the gas molecules.

So, a gas can behave ideally if above postulates are followed and these can be followed if temperature is high and pressure is low. These conditions will help the gas particles to remain at larger distance with no attractions.

And if the pressure is high and temperature is low then particles come closer and there exist a force of attraction between them.

Because a gas don't follow kinetic theory at all temperature and pressure, it is not ideal in nature.

Conclusion

All gases are real. They show ideal behavior at specific temperature and pressure range.

Chapter 13, Problem 63A

Chapter 13, Problem 65A

Chapter 13 Solutions

Chemistry: Matter and Change

Ch. 13.1 - Prob. 1PP Ch. 13.1 - Prob. 2PP Ch. 13.1 - Prob. 3PP Ch. 13.1 - Prob. 4PP Ch. 13.1 - Prob. 5PP Ch. 13.1 - Prob. 6PP Ch. 13.1 - Prob. 7PP Ch. 13.1 - Prob. 8PP Ch. 13.1 - Prob. 9PP Ch. 13.1 - Prob. 10PP

Ch. 13.1 - Prob. 11PP Ch. 13.1 - Prob. 12PP Ch. 13.1 - Prob. 13PP Ch. 13.1 - Prob. 14SSC Ch. 13.1 - Prob. 15SSC Ch. 13.1 - Prob. 16SSC Ch. 13.1 - Prob. 17SSC Ch. 13.1 - Prob. 18SSC Ch. 13.1 - Prob. 19SSC Ch. 13.2 - Prob. 20PP Ch. 13.2 - Prob. 21PP Ch. 13.2 - Prob. 22PP Ch. 13.2 - Prob. 23PP Ch. 13.2 - Prob. 24PP Ch. 13.2 - Prob. 25PP Ch. 13.2 - Prob. 26PP Ch. 13.2 - Prob. 27PP Ch. 13.2 - Prob. 28PP Ch. 13.2 - Prob. 29PP Ch. 13.2 - Prob. 30PP Ch. 13.2 - Prob. 31SSC Ch. 13.2 - Prob. 32SSC Ch. 13.2 - Prob. 33SSC Ch. 13.2 - Prob. 34SSC Ch. 13.2 - Prob. 35SSC Ch. 13.2 - Prob. 36SSC Ch. 13.2 - Prob. 37SSC Ch. 13.3 - Prob. 38PP Ch. 13.3 - Prob. 39PP Ch. 13.3 - Prob. 40PP Ch. 13.3 - Prob. 41PP Ch. 13.3 - Prob. 42PP Ch. 13.3 - Prob. 43PP Ch. 13.3 - Prob. 44PP Ch. 13.3 - Prob. 45PP Ch. 13.3 - Prob. 46SSC Ch. 13.3 - Prob. 47SSC Ch. 13.3 - Prob. 48SSC Ch. 13.3 - Prob. 49SSC Ch. 13 - Prob. 50A Ch. 13 - Prob. 51A Ch. 13 - Prob. 52A Ch. 13 - Prob. 53A Ch. 13 - Prob. 54A Ch. 13 - Prob. 55A Ch. 13 - Prob. 56A Ch. 13 - Prob. 57A Ch. 13 - Prob. 58A Ch. 13 - Prob. 59A Ch. 13 - Prob. 60A Ch. 13 - Prob. 61A Ch. 13 - Prob. 62A Ch. 13 - Prob. 63A Ch. 13 - Prob. 64A Ch. 13 - Prob. 65A Ch. 13 - Prob. 66A Ch. 13 - Prob. 67A Ch. 13 - Prob. 68A Ch. 13 - Prob. 69A Ch. 13 - Prob. 70A Ch. 13 - Prob. 71A Ch. 13 - Prob. 72A Ch. 13 - Prob. 73A Ch. 13 - Prob. 74A Ch. 13 - Prob. 75A Ch. 13 - Prob. 76A Ch. 13 - Prob. 77A Ch. 13 - Prob. 78A Ch. 13 - Prob. 79A Ch. 13 - Prob. 80A Ch. 13 - Prob. 81A Ch. 13 - Prob. 82A Ch. 13 - Prob. 83A Ch. 13 - Prob. 84A Ch. 13 - Prob. 85A Ch. 13 - Prob. 86A Ch. 13 - Prob. 87A Ch. 13 - Prob. 88A Ch. 13 - Prob. 89A Ch. 13 - Prob. 90A Ch. 13 - Prob. 91A Ch. 13 - Prob. 92A Ch. 13 - Prob. 93A Ch. 13 - Prob. 94A Ch. 13 - Oxygen Consumption If 5.00 L of hydrogen...Ch. 13 - Prob. 96A Ch. 13 - If 2.33 L of propane at 24°C and 67.2 kPa is...Ch. 13 - Prob. 98A Ch. 13 - Prob. 99A Ch. 13 - Prob. 100A Ch. 13 - Prob. 101A Ch. 13 - Apply Calculate the pressure of (4.671022)...Ch. 13 - Analyze When nitroglycerin (C3H5N3O9) explodes,...Ch. 13 - Prob. 104A Ch. 13 - Prob. 105A Ch. 13 - Prob. 106A Ch. 13 - Prob. 107A Ch. 13 - Prob. 108A Ch. 13 - Prob. 109A Ch. 13 - Prob. 110A Ch. 13 - Prob. 111A Ch. 13 - Prob. 112A Ch. 13 - Prob. 113A Ch. 13 - Prob. 114A Ch. 13 - Prob. 115A Ch. 13 - Prob. 116A Ch. 13 - Prob. 117A Ch. 13 - Prob. 118A Ch. 13 - Prob. 119A Ch. 13 - Prob. 1STP Ch. 13 - Prob. 2STP Ch. 13 - Prob. 3STP Ch. 13 - Prob. 4STP Ch. 13 - Prob. 5STP Ch. 13 - Prob. 6STP Ch. 13 - Prob. 7STP Ch. 13 - Prob. 8STP Ch. 13 - Prob. 9STP Ch. 13 - Prob. 10STP Ch. 13 - Prob. 11STP Ch. 13 - Prob. 12STP Ch. 13 - Prob. 13STP Ch. 13 - Prob. 14STP

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A ideal gas is to be defined and the reason why there is no true ideal gas in nature is to be justified. Concept introduction: The concept of ideal gas is studied by kinetic gas theory.

Solution Summary: The author explains that a gas is ideal if it follows all the gas laws at all temperature and pressure and deviates from ideal behavior at high and low pressure.