When the conditions are normal, all gases have similar behaviour. However, even slight changes in physical conditions such as pressure, temperature, or volume cause a deviation. The behaviour of gases is studied using gas laws. A gas’s state variables, such as pressure, volume, and temperature, reveal its real nature. As a result, gas laws are the relationships that exist between these variables. Let’s learn more about the crucial gas rules!
The gas laws are a set of rules that control the behaviour of gases by establishing correlations between the following variables:
- The amount of space occupied by gas.
- The force that a gas exerts on the container’s walls.
- The gas’s absolute temperature.
- The quantity of a gaseous material (or the number of moles of gas).
All gases behave similarly under ordinary conditions. When the physical parameters related to the gas (such as temperature, pressure, and volume) are changed, alterations in their behaviour occur. The gas laws, which were named after the scientists who discovered them, essentially describe the behaviour of gases.
When the conditions are normal, all gases exhibit comparable behaviour. However, a little change in physical variables like as pressure, temperature, or volume causes a divergence. Gas laws are an examination of the behaviour of gases. A gas’s state variables, such as pressure, volume, and temperature, reveal its true nature. As a result, gas laws are relationships between these variables.
At constant temperature, Boyle’s law describes the relationship between a gas’s pressure and volume. So, according to Boyle’s law, doubling the pressure reduces the volume of a gas by half at a constant temperature. The explanation for this is the intermolecular force that exists between the molecules of a gaseous substance. Because of the distributed molecules, a gaseous substance fills a larger volume of the container in its free condition. When pressure is applied to a gaseous medium, the molecules move closer together and take up less space. In other words, the applied pressure is proportional to the density of the gas. The volume of a gas is inversely proportional to its pressure under constant temperature. Its formula is as follows:
Boyle’s Law can be used to calculate the current pressure or volume of a gas and is also written as
In 1787, Jacques Charles studied the impact of temperature on the volume of a gaseous substance under constant pressure. He conducted this research to better understand the technology behind hot air balloon flights. According to Charle’s law, the volume of a gas in a closed system with constant pressure is directly proportional to the temperature (in Kelvin). This means that as the temperature rises, the volume rises, and as the temperature falls, the volume falls. This law essentially outlines the relationship between the temperature and volume of a gas. Charle’s law can be stated mathematically as;
V1 / T1 = V2 / T2
The Gay-Lussac equation expresses the relationship between temperature and pressure at constant volume. The law asserts that for a particular gas, the pressure is directly proportional to the temperature at a constant volume. When you heat up a gas, the molecules gain energy and travel quicker. When the molecules are cooled, they slow down and the pressure lowers. The Gay-Lussac law, which is mathematically written as; can be used to determine the change in temperature and pressure.
P1 / T1 = P2 / T2
According to Avogadro’s law, if the gas is an ideal gas, the system has the same number of molecules. The law also indicates that if the volume of gases is equal, the number of molecules will be the same as the ideal gas only when the volume is identical. This statement can be stated numerically as
V1 / n1 = V2 / n2
Where V denotes the volume of an ideal gas and n denotes the number of gas molecules in the preceding equation. The temperature in this location is measured on the Kelvin scale. Because the volume here is constant, the graph for Gay-Law Lussac’s is referred to as an isochore.
Amedeo Avogadro merged the conclusions of Dalton’s Atomic Theory with Gay Lussac’s Law in 1811 to create the Avogadro’s Law, which is an essential Gas law. Avogadro’s law states that under constant temperature and pressure, the volume of all gases equals an equal number of molecules. In other words, under constant temperature and pressure, the volume of any gas is directly proportional to the number of molecules in that gas.
The previous gas laws provide an overview of the many properties of gases at various temperatures, pressures, volumes, and masses. These laws may appear insignificant, but they play a significant role in our daily lives. The difference in gaseous behaviour under altered conditions can affect everything from respiration to hot air balloons and automobile tyres.
The combined gas law, also known as a general gas equation, is formed by merging three gas laws: Charle’s law, Boyle’s law, and Gay-Lussac law. The law describes the relationship between temperature, volume, and pressure for a given amount of gas. If we want to compare the same gas in different situations, the law can be expressed as follows:
(P1 * V1) / T1 = (P2 * V2) / T2
The ideal gas law, like the combined gas law, is a synthesis of four separate gas laws. Avogadro’s law is applied here, and the combined gas law is transformed into the ideal gas law. This law connects four different variables: pressure, volume, the number of moles or molecules, and temperature. Essentially, the ideal gas law describes the relationship between the four factors listed above. The ideal gas law is stated mathematically as;
where, V = volume of gas, T = temperature of the gas, P = pressure of the gas, R = universal gas constant and n denotes the number of moles.
Application of Gas Laws
- When the physical conditions of the environment change, the behaviour of gas particles deviates from their regular behaviour. The numerous laws known as gas law can be used to investigate these changes in gas behaviour.
- The gas laws have been around for a long time, and they greatly assist scientists in determining quantities, pressure, volume, and temperature when it comes to gas.
- Furthermore, the gas law, as well as newer variants, are used in a variety of practical applications using gas. For example, measurements of respiratory gases, tidal volume, and vital capacity, among other things, are taken at room temperature, despite the fact that these exchanges occur in the body at 37 degrees Celsius.
- The law is also frequently utilised in thermodynamics and fluid dynamics. It can be employed in weather prediction systems.
Question 1: What are gas laws?
A gas’s state variables, such as pressure, volume, and temperature, reveal its true nature. As a result, gas laws are relationships between these variables.
Question 2: What is the effect of temperature on a gas?
The state variables of a gas, such as pressure, volume, and temperature, reflect the true nature of the gas. As a result, gas laws are based on the interactions of these variables.
Question 3: What is Avogadro’s law?
According to Avogadro’s law, if the gas is an ideal gas, the system has the same number of molecules. The law also indicates that if the volume of gases is equal, the number of molecules will be the same as the ideal gas only when the volume is identical.
Question 4: Name the four variables in ideal gas law?
The four distinct variables are pressure, volume, the number of moles or molecules, and temperature.
Question 5: What is the relation between temperature and volume in gases?
When the temperature increases, the volume increases, and when the temperature falls, the volume falls. Thus, they are directly proportional to each other.
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