Question

When the temperature of a gas in a rigid container decreases, the particles of the gas move slower and experience fewer collisions with each other and the container walls. Because of this, it is sometimes necessary to add more air to automobile tires in the winter.Which gas law applies in this situation?

Answer 1

Gay Lusaac's law: The pressure Temperature Law

Step-by-step explanation:

First off, it is important to understand that the fewer collisions experienced by the particles with each other and the walls of the container is referring to the pressure.

SO, form the question, we can tell that temperature and pressure are directly proportional to each other. As temperature increases, the particles move faster which in turn leads to increased pressure.

After that has been established, we look up the gas laws and find the pone that gives a temperature-pressure relationship and this is the Gay-Lussac's Law: The Pressure Temperature Law. This law states that the pressure of a given amount of gas held at constant volume is directly proportional to the Kelvin temperature. As the pressure goes up, the temperature also goes up, and vice-versa.

Answer 2

When the temperature of a gas within a rigid container decreases, the particles on average move more slowly and do not collide with one another or the container walls as often. It is the the ideal gas law that applies in this situation and states that a decrease in the temperature of a gas also results in a decrease in the pressure. Thus, automobile tyres which have a colder gas in the winter sometimes need additional air to provide suffiicient pressure.