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?

Gay Lusaac's law: The pressure Temperature Law

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.

58750.08068 is the answer i think

while cooking a piece of 1/2 pound beef steak, a cast iron pan (2.4kg in weight) was heated 260 celsius.