Temperatures in Kelvin and pV / T = constant

The Kelvin scale is the SI unit for temperature, based directly on the properties of gas particles under the kinetic theory. Zero on the Kelvin scale, also known as absolute zero, is the point at which all particle motion stops.
Temperature in Kelvin (K) can be converted from degrees Celsius (°C) using the formula T(K) = T(°C) + 273.
The pressure and volume of a gas are directly related to its temperature. This relationship is represented by the formula pV=KT, where p is the pressure, V is the volume, K is a constant value, and T is the temperature.
The formula pV / T = constant is the law of gases, also known as Gay-Lussac’s law, which says that for a fixed volume of gas at a constant pressure, the temperature of the gas is directly proportional to its pressure.
This law implies that if you double the temperature of a gas (measured in Kelvin), the pressure will also double. Similarly, if you halve the temperature, the pressure will halve as well.
Real-life applications of this principle include tyre pressure, which can increase in hot weather due to increased gas temperature, and aerosol cans, which warn against incineration, as high temperatures will increase the pressure inside the can to unsafe levels.
Understanding these principles is crucial for further learning in physics and chemistry, as well as practical tasks ranging from tyre maintenance, the use of gas cylinders, and understanding weather patterns.
It’s important to remember that these relationships hold true only in ideal gas conditions. In real-world scenarios, factors like intermolecular forces and the volume of individual particles become significant and need to be considered.
Practice problems, diagrams, and demonstrations can help solidify understanding of these concepts and their applications.