Ideal & real gases Physical Chemistry Report

1. Koya University
Faculty of Engineering
Chemical Engineering Department
Instructor
Mr. Soran Delawar
Physical Chemistry
Physical Chemistry Report
Ideal & Real Gases
Submitted Date
24 Apr 2021
Prepared by
Safeen Yaseen Ja’far
Ibrahim Ali
Rekan Kazm Jamel
Rekar Hamza
Rivan Dler Ali
Rokan Mohammed Omer
Ramazan Shkur Kakl
Ahmed Mamand Aziz

2. TABLE OF CONTENTS
ABSTRACT/SUMMARY ............................................................................................... 1
1. INTRODUCTION........................................................................................................ 2
2. BODY........................................................................................................................4-11
2.1 WHAT ARE THE GASES .............................................................................................. 4
2.2 THE TWO TYPES OF GASES......................................................................................... 4
2.2.1 Ideal Gases ........................................................................................................ 5
2.2.2 Real Gases........................................................................................................... 6
2.3 DIFFERENCES BETWEEN THE IDEAL AND REAL GASES .............................................. 8
2.4 APPLICATIONS OF THE IDEAL AND REAL GASES........................................................ 9
2.5 DEVIATIONS FROM IDEAL GAS LAW BEHAVIOR ....................................................... 10
3. CONCLUSION .......................................................................................................... 12
4. LIST OF REFERENCES ......................................................................................... 13

3. LIST OF FIGURES
Figure 1 ............................................................................................................................. 2
Figure 2 ............................................................................................................................. 3
Figure 3 ............................................................................................................................. 4
Figure 4 ............................................................................................................................. 5
Figure 5 ............................................................................................................................. 6
Figure 6 ............................................................................................................................. 6
Figure 7 ............................................................................................................................. 7

4. 1
Abstract
All matters have specific phase and have general and special properties. In this report we
discuss about one of the phases of matter which include gases. However, gas phase is the most
contributed substance with us and with around of us. Typically, gases have benefits and can be
used for different thing, such as, Heating and cooling. water heating, and cooking, Power plants
can use gas to generate electricity, also, transport. Some of the gases exist naturally in the planet.
Natural Gas (NG) Which an integral part of our everyday lives

5. 2
1. Introduction
Physical chemistry is now one of the most important fields of chemistry research, as it
contributes to the understanding of complex systems as well as the properties of molecules. A
gas phase, unlike a solid or liquid phase, prefers to occupy the whole interplanetary at its
disposal. Ideal gases do not exist in fact, but they do exist in theory. Any gas molecule in the
system has a volume. Due to the conservation of energy and momentum inside the system, even
though gas particles will travel spontaneously, they do not have perfect elastic collisions. There
is also the law of the "Ideal Gas," which is a straightforward equation that can be used to
calculate the physical properties of a device that can be used as a baseline calculation. However,
we will not discuss the laws in this article, instead focusing on their features, forms, uses, and
advantages. [1]
Ideal Gases are an imaginary gas thought up by chemists and students that the Ideal Gas
Law would be much simpler if problems like intermolecular forces didn't exist to confuse it.
Ideal gases are basically point masses traveling in a straight line at a steady, arbitrary speed. The
hypotheses listed in the Kinetic-Molecular Theory of Gases explain its behavior. This concept of
an ideal gas differs from the Non-Ideal Gas definition in that it reflects how gas behaves in fact
(Pv = nRT). Let us concentrate on the Ideal Gas for the time being. [2]
Figure 1: This figure shows as the motion of both type of gases.

6. 3
1.2 History of Finding Ideal and Real Gases
Emile Clapeyron was a French physicist and engineer who was one of the pioneers of
thermodynamics. Emile Clapeyron is able to integrate the Boyles, Charles, and Avogadro's Laws
into the Ideal Gas Equation in 1984. Ideal the gas has been around since the early 17th century to
aid science in determining quantities, amounts, pressures, and temperatures when it comes to
matters of gas. Three key laws make up the Ideal Gas Laws: Charles' Law, Boyle's Law, and
Avogadro's Law. [3]
Ideal gases are gases that are unaffected
by external forces such as intermolecular forces.
They are a definition that has evolved over
hundreds of years and are based on the ideal gas
law, which is a synthesis of three other gas laws
found independently by Boyle. These three gas
laws are: Boyle's law, which states that the
volume and pressure of a gas are inversely
proportional at constant temperature
(P1V1=P2V2); Charles' law, which states that the
volume of a gas is directly proportional to its
absolute temperature at constant pressure (V1/T1
= V2/T2); and Avogadro's law, which states that
the volume of a gas is directly proportional to its
absolute temperature at constant pressure (V1/T
that notes that all gases have the same number of
moles per liter at the same temperature and pressure (n1/V1 = n2/V2). When these are added
together, they form Dmitri Mendeelev's ideal gas law (PV = nRT). [4]
Figure 2: This figure shows Dmitri
Mendeelev

7. 4
2.1 What are the Gases?
A gas is a state of matter that does not have a fixed form or thickness. Other states of
matter, such as solids and liquids, have a smaller density than gases. Between particles with a lot
of kinetic energy, there is a lot of empty space. The particles move quickly and collide, allowing
them to disperse, or scatter out, until they are uniformly dispersed within the container's volume.
[5]
2.2 The Two Types of Gases
Gases can be classifying into two class according to their types or by another word based on
two types. So, there are two type:
▪ Ideal Gases (Perfect Gases)
▪ Real Gases (Non-Ideal Gases)
Figure 3: Gas particles spread out to fill a container evenly, unlike
solids and liquids.

8. 5
2.2.1 Ideal Gases
Ideal Gases: Gases are difficult to
understand. They're teeming with billions
upon billions of energetic gas molecules that
might collide and interact. Since it's difficult
to precisely characterize a real gas, the notion
of an ideal gas was developed as a rough
approximation that can be used to model and
simulate the action of real gases. The concept
"ideal gas" describes a potential gas made up
of molecules that adhere to a set of laws. [6]
Ideal Gas Behaviors
The properties of an ideal gas are:
• An ideal gas is made up of a lot of similar molecules. In certain cases, an ideal gas differs
from a natural gas.
• In comparison to the amount occupied by the gas, the molecules themselves take up very
little space.
• The molecules follow Newton's laws of motion and travel in random motion. • The
molecules only undergo forces as they collide; any collisions are fully elastic and require
a negligible amount of time.
• Gas molecules that are lighter travel faster than those that are heavier.
• The density of an ideal gas should be ignored in the calculation since it has none; this is
because an ideal gas is referred to as an atom, and has no mass. [7]
Figure 4: Ideal Gas Law Surface for Fixed Amount
of Gas.

9. 6
Pressure, Volume, and Temperature Relationships in Ideal Gases
Figure 5: Ideal Gases have different relation via temperature, pressure volume and number
of mols.
2.2.2 Real Gases
At all normal pressure and temperature conditions, real gas is known as a gas that does
not obey gas laws. The action of the gas deviates from its ideal as it becomes vast and
voluminous. Velocity, volume, and mass are all characteristics of real gases. They liquefy when
cooled below their boiling point. The space filled by the gas is not insignificant when opposed to
the actual volume of the gas. [8]
Real Gas Behaviors
The Effect of Nonzero Gas Particle
Volume on Gas Behavior at Low and High
Pressures (a) At low temperatures, the space
filled by the molecules is small in comparison to
the container's volume. (b) At high temperatures,
Figure 6: This figure shows a behavior of
the real gases under two different pressure

10. 7
the molecules take up a considerable part of the container's length, limiting the amount of room
available for them to travel. [9]
Pressure, Volume, and Temperature Relationships in Real Gases
A plot of PV/nRT versus P for an ideal gas yields a horizontal line with an intercept of 1
on the PV/nRT axis. Real gases, on the other hand, deviate significantly from ideal gas behavior,
particularly at high pressures (part (a) of Figure 10.21 "Real Gases Do Not Obey the Ideal Gas
Law, Especially at High Pressures"). Real gases approximate ideal gas action only at low pressures
(less than 1 atm) (part (b) in Figure 10.21 "Real Gases Do Not Obey the Ideal Gas Law, Particularly
at High Pressures"). At higher temperatures, real gases often resemble ideal gas behavior more
closely, as seen in Figure 10.22 "The Effect of Temperature on the Behavior of Real Gases" for
N2. Why do natural gases behave so differently at high pressures and low temperatures than ideal
gases? The two fundamental assumptions underlying the ideal gas law—that gas molecules have
negligible volume and that intermolecular correlations are negligible—are no longer applicable
under these conditions. [10]
Figure 7: This figure shows the pressure, volume, and temperature
relationships in real gases
.

11. 8
2.3 Differences Between the Ideal Gases and The Real Gases?
To make you understand how ideal gas and real gas are different from each other, here
are the some of the major differences between ideal gas and real gas:
Difference between Ideal gas and Real gas:
Ideal Gases Real Gases
• No definite volume
• Elastic collision of particles
• No intermolecular attraction forces
• Does not really exists in environment
and is a hypothetical gas
• High pressure
• Does not obey gas laws at all
conditions of pressure and temperature
• Independent
• Obey this eq. Pv = nRT
• Definite volume
• Non elastic collision of particles
• Intermolecular attraction forces
• It really exists in the environment
• Pressure is less when compared to Ideal
gas
• Obeys gas laws at high temperature and
• low pressure
• Interacts with others
• Obey this eq.
[11]

12. 9
2.4 Applications of The Ideal and Real Gases
2.4.1 Applications of the Ideal gas
Ideal gases are used to calculate engine efficiencies and in different thermal equipment’s to
calculate potential performance parameters. Gas laws apply on all ideal or optimal gases. At
low pressures, high temperatures, or both, real gases obey the rules.
Ideal Gas and Airbags: Airbags in automobiles are another example of ideal gases in
everyday life. The operating mechanics of airbags are determined by ideal gas laws. As
airbags deploy, they easily fill with the appropriate gases to inflate and then fully inflate
when the car crashes.
In the laboratory: gases produced in a reaction are often collected by the displacement of
water from filled vessels. the amount of gas can then be calculated from the volume of water
displaced and the atmospheric pressure.
• Ideal Gas in Planes and Buildings: One environment where ideal gases are useful is in
commercial buildings. Ventilation units must be installed in any commercial building
where air ventilation is not otherwise adequate enough to maintain a balance between the
amount of oxygen and carbon dioxide in a building.
• Other Examples of Ideal Gas Laws: The relationship between the amounts of products
and reactants in a chemical reaction can be expressed in units of moles or masses of pure
substances, of volumes of solutions, or of volumes of gaseous substances. The ideal gases
can be used to calculate the volume of gaseous products or reactants as needed. [12]
2.4.2 Applications of the Real gas
Consider Supercritical carbon dioxide, a real gas (S-CO2). In comparison to generic
fluids, it needs less compression work at the critical stage. As a result, we can boost compressor
performance by using S-CO2. Furthermore, S-CO2 has a higher density, which contributes to its
compactness.
• Though cool air acts like an ideal gas at ordinary pressure, raising its pressure or
temperature raises the interactions between molecules, resulting in actual gas behaviour
that cannot be accurately modeled using the ideal gas rule.

13. 10
• Another example of natural gas is in a rocket nozzle, where the fuel is exposed to
extreme temperatures and pressures, causing it to deviate from the ideal gas law. This
actual gas impact should be taken into account in all empirical estimates. The great "Dr.
Van der Waals" appears. [13]
2.5 Deviations from Ideal Gas Law Behavior
At normal temperatures and pressures, the action of real gases generally correlates with the
predictions of the ideal gas equation to within 5%. Real gases deviate greatly from ideal gas
activity at low temperatures or high pressures. The Dutch physicist Johannes van der Waals
developed an explanation for these deviations and an equation that could match the behavior of
real gases over a much wider range of pressures in 1873, when looking for a way to relate the
behavior of liquids and gases. Van der Waals found that two of the kinetic molecular theory's
conclusions were dubious. Gas particles occupy a negligible fraction of the total volume of the
gas, according to the kinetic principle. The force of attraction between gas molecules is often
assumed to be zero. [14]
When it comes to gas measurements, it's usually fine to use the ideal gas law. However, at very
high pressures, near the critical stage, or near the condensation point of a gas, the approximation
gives significant error. A real gas, unlike an ideal gas, is subject to Van der Waals forces;
• Compressibility effects;
• Non-equilibrium thermodynamic effects;
• Variable specific heat capacity; and
• Variable composition, including molecular dissociation and other chemical reactions.
At pressures close to 1 atm, the first statement holds true. However, when the gas is
compressed, something happens to the truth of this assumption. Assume that all of the atoms or
molecules in a gas are crowded together in one corner of a cylinder, as seen in the diagram
below. The space occupied by these particles at normal pressures is a negligible fraction of the
overall volume of the gas. As a result, real gases are less compressible than ideal gases at high
pressures. At high pressures, the volume of a real gas is therefore greater than predicted by the
ideal gas equation. Van der Waals suggested that we subtract a term from the volume of a real

14. 11
gas before substituting it into the ideal gas equation to account for the fact that its volume is too
large at high pressures. As a result, he introduced a constant. [15]

15. 12
4. Conclusion
In previous sections in this report, we talked about gases and how they discovered also
with their properties, classifications, applications, etc. In this section we brief or summarize all
before sections as well as below points:
• Gas is one of the states o matter.
• All gases have physical or chemical properties.
• Ideal gas and real gas are different with each other.
• Ideal gases are the gas which have non real (actual) properties
• Real gas equation or real gas law can be derived from ideal gas law.

16. 13
5. References
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