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Gaseous State of Matter
4
Gaseous State of Matter
Concept Map
What are the properties of Gas?
Introduction
The state of a substance known as gas has no set shape or volume. Other states of matter, such as solids and liquids, have a lower density than gases.
The kinetic molecular theory is a simple theoretical model that can explain the experimental facts about gas behavior. The following postulates, or assumptions, underpin this theory:
Kinetic Molecular Theory
- Gases are made up of a vast number of particles that behave like hard, spherical objects moving in a random manner.
- The space between particles is substantially smaller than the size of these particles. As a result, the majority of a gas's volume is empty space.
- No attraction exists between gas particles or between the particles and the container's walls. Impacts between gas particles and collisions with container walls are completely elastic. When a gas particle collides with another particle or the container's walls, none of its energy is wasted.
- The average kinetic energy of a collection of gas particles is solely determined by the gas's temperature.
Ideal Gas:
- A gas in which the molecules do not attract each other.
- Many gases, including nitrogen, oxygen, hydrogen, noble gases, some heavier gases like carbon dioxide, and mixtures like air, can be regarded as ideal gases within reasonable tolerances throughout a wide temperature and pressure range.
Ideal Gas vs Real Gas
Real Gas:
- The impact of gas particles occupying a finite volume and the strength of intermolecular forces cause a real gas to depart from ideal behavior.
- A real gas is something that exists. Oxygen, hydrogen, carbon dioxide, helium, carbon monoxide, and other gases are examples. Real gases exhibit tiny attraction and repulsive forces between particles, whereas ideal gases do not.
Gas Pressure
When gas particles collide with the container's walls, pressure is created. The higher the pressure, the more often the particles hit the walls and the quicker they are going when they do so. High temperature and low pressure are the best conditions for gases.
Gas Laws
The interdependence of temperature, pressure, quantity, and volume of a gas has led to the development of laws to characterize the interactions between them.
Boyle's Law
Gas Law 1
Boyle's Law (also known as Mariotte's Law), is a fundamental chemistry principle that describes the behavior of a gas at a constant temperature. It is a pressure-temperature relationship.
Formula:
Robert Boyle
Background
Robert Boyle is known as a natural philosopher in the chemistry field. He discovered that the volume of a gas decreases as the pressure increases and vice versa. And he is the proponent of the well-known Boyle's Law.
Increasing the available space allows the gas particles to spread out further, but this reduces the number of particles available to collide with the container, lowering pressure. Because the container's volume is reduced, the particles clash more frequently, increasing the pressure. Filling a tire with air is a nice example of this. As more air is introduced, the gas molecules become more compact, lowering their volume. The pressure rises as long as the temperature remains constant.
How does Boyle's Law work?
= First Pressure
= Second Pressure
= First Volume
= Second Volume
Formula
Charle's Law:
If the pressure remains constant, Charles's law states that the volume occupied by a fixed amount of gas is directly proportional to its absolute temperature. And it is a temperature-volume relationship.
Gas Law 2
Formula:
Jacques Charles
Background
Jacques Charles was a French inventor, scientist, mathematician, and balloonist. He discovered the gas law, named for his honour, Charle's Law, where if the pressure of a gas is held in a persistent manner, the increase in the temperature of the gas will increase its volume.
How does Charle's Law work?
Charle's law asserts that a gas's volume and temperature are proportional; as temperature rises, volume rises when pressure remains constant. The kinetic energy of the particles in a gas increases when it is heated, causing the gas to expand. When a gas is heated, the volume of the container must be raised to maintain the pressure. This law also explains why it is critical to follow the safety rule of never heating a closed container. When the temperature rises without the volume available to accept the expanding gas, pressure builds inside the container, which could lead to an explosion.
= First Volume
= Second Volume
= First Temperature
= Second Temperature
Formula
Gay-Lussac's Law:
When two or more gaseous substances mix to form a gaseous compound, the product's volume is either equal to or less than the total of the ingredients' volumes, and bears a simple ratio to this sum.
Gas Law 3
Formula:
Joseph Louis Gay-Lussac
Background
Joseph Louis Gay-Lussac was a French chemist and physicist who is the proponent of the known gas law, Gay-Lussac's Law, that explains that when the volume of a gas is kept constant, such as in a closed container, and heat is applied, the gas's pressure rises.
According to Gay-Lussac's law, the pressure exerted by a gas of a given mass and sustained at a constant volume varies directly with the absolute temperature of the gas. Lussac's In other words, when the mass is constant and the volume is constant, the pressure produced by a gas is proportional to its temperature.
How does Gay-Lussac's Law work?
= First Pressure
= Second Pressure
= First Temperature
= Second Temperature
Formula
Combined Gas Law:
The combined gas law states that the product of pressure and volume, as well as the absolute temperature of a gas, are equal.
Ideal Gas Law:
Gas Law 4
According to this law, the volume of a given amount of gas is directly proportional to the number of moles of gas, directly proportional to temperature, and inversely proportional to pressure.
Formula:
Combined Gas Law
Ideal Gas Law
Benoît Paul Émile Clapeyron
Background
Benoît Paul Émile Clapeyron was a French physicist who combined the old gas laws into one that is now called the Combined gas law. And the ideal gas law is a thermodynamic equation that relates the temperature, volume, and number of molecules (or moles) present in a gas sample.
Boyle's Law, Charles' Law, and Gay-Law Lussac is integrated into the combined gas law. It states that the product of pressure and volume, as well as the absolute temperature of a gas, are equal. The ideal gas law is obtained by adding Avogadro's law to the combined gas law. The ideal gas constant, Avogadro's Number, and both Boyle's and Charles' laws combine to define a theoretical ideal gas in which all particle collisions are exactly equal. Although the rules come close to explaining the behavior of most gases, there are minor mathematical discrepancies due to variances in particle size and minuscule intermolecular interactions in real gases. These key principles are, however, sometimes integrated into a single equation known as the ideal gas law. If you know the values of the other three variables, you can use this law to find the value of any of the other variables — pressure, volume, number, or temperature.
How does the Combined Gas Law and Ideal Gas Law work?
= First Pressure
= Second Pressure
= First Volume
= Second Volume
= First Temperature
= Second Temperature
= Pressure
= Volume
= Amount of substance
= Ideal gas constant
= Temperature
Formula
Ideal Gas Law
Combined Gas Law
Graham's Law :
The rate of effusion of a gas is inversely proportional to the square root of its density or molecular mass, per Graham's Law. While the diffusion rate states that the ratio of the square root of the molar mass of two gases equals the ratio of their diffusion rates.
Gas Law 5
Formula:
Thomas Graham
Background
Thomas Graham, a British chemist, completed his studies in science, and his discoveries have been of great scientific importance to the world today. His exceptional discoveries were the diffusion of gases and liquids, and by observing the effusion of gases, he derived the Graham's Law that was named after him.
Graham's law states that a gas's rate of diffusion is inversely proportional to its molar mass squared.
How does Graham's Law work?
= Rate of effusion/diffusion for gas 1
= Rate of effusion/diffusion for gas 2
= Molar mass of gas 1
= Molar mass of gas 2
Formula
Dalton's Law of Partial Pressure:
The pressure that a gas would exert in a mixture of gases if it alone occupied the entire volume of the mixture.
Gas Law 6
Formula:
John Dalton
Background
John Dalton, an English meteorologist and chemist, discovered the partial pressure, which is the pressure that each gas would exert if it were alone in the combination at the same temperature. And the gas law, Dalton's Law, was named after him.
The overall pressure exerted by a mixture of gases is equal to the sum of the partial pressures exerted by each of the constituent gases, according to Dalton's partial pressure equation. The partial pressure is the pressure that each gas would exert if it occupied the same volume of the mixture at the same temperature by itself.
How does Dalton's Law work?
= Partial Pressure of gas a
= Mole fraction of gas a
= Total Pressure of mixture
= Total Pressure
= Partial Pressure of each gas
Formula
Partial Pressure
Dalton's Law of Partial Pressure
Sources
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