How do Gases Change with Different Conditions?
This post will go through the basic laws that describe the relationship between the volume of a gas and temperature, pressure and the number of moles for Prelim Chemistry.
According to the syllabus, you will need to be able to:
- Conduct investigations and solve problems to determine the relationship between the Ideal Gas Law and:
- Gay-Lussac’s Law (temperature)
- Boyle’s Law
- Charles’ Law
- Avogadro’s Law
The Gas Laws
There are four main laws and the combined law. The laws and the relationships they describe (assuming the other factors are constant) are:
Gay Lussac’s Law -> pressure and temperature (volume and moles constant)
P1/T1 = P2/T2
Boyle’s Law -> pressure and volume (temperature and moles constant)
P1V1 = P2V2
Charle’s Law -> volume and temperature (pressure and moles constant)
V1/T1 = V2/T2
Avogadro’s Law -> volume and moles (pressure and temperature constant)
V1/n1 = V2/n2
Combined Law
(P1V1)/T1 = (P2V2)/T2
Note that these are simplified descriptions of the laws and it is advised you go through them in a little more depth.
The video below will better describe these concepts which will help you with understanding how to use them.
These describe the behaviour of gases under different conditions, including pressure, volume, temperature, and amount. These laws are important in understanding the properties of gases and how they interact with their surroundings.
One of the most fundamental is Boyle’s law, which states that the volume of a gas is inversely proportional to its pressure, provided the temperature and amount of the gas remain constant. Another important gas law is Charles’s law, which states that the volume of a gas is directly proportional to its temperature, provided the pressure and amount of the gas remain constant.
The combined gas law is a combination of Boyle’s law, Charles’s law, and Avogadro’s law, which states that the volume of a gas is directly proportional to the number of moles of the gas, provided the pressure and temperature remain constant.
The ideal one combines all of these laws into a single equation, relating the pressure, volume, temperature, and amount of a gas to each other. This law is particularly useful in understanding and predicting the behaviour of gases in a wide range of applications, from chemistry and physics to meteorology and engineering.
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