Charles’ law is one of the popular laws that explain the relationship between volume and temperature of a gas. Based on this law when pressure is kept constant then the volume for a fixed amount in case of dry gas is directly proportional to the absolute temperature too. When two parameters are arranged in the direct proportion then the changes made to any of the parameters will affect the other one too. Here is how Charles’ Law is given in the chemistry:
Charles’ Law is the special case of ideal gas that the volume of a fixed mass of a gas is always directly proportional to its temperature. The law is always applied to the ideal gases at a constant pressure where volume or temperature is subjected to change. The other popular form of Charles’ Law is given as –
\[\ \frac{V1}{T1} = \frac{V2}{T2} \]
Where V1 is the initial volume, V2 is the final volume, T1 is taken as the initial temperature, and T2 is the final temperature. Both are given in the terms of Kelvin. The concept of Charles’ Law was discovered by a French scientist in 1787 and later it was modified by Gay-Lussac in 1802 and used frequently till today. One more standard form of Charles’ Law is presented in the form of absolute temperature and the absolute volume.
Keep in mind that absolute temperatures are always measured in Kelvin, not in degree Celsius C or F. There are a plenty of application of Charles’ Law in the real-life too like cold weather or environment, balls or helium balloons shrink etc.