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.

a. energy is absorbed in the reaction.

if in a given reaction the energy of products is greater than the energy of reactants it means that reaction is endothermic and during the reaction, the energy is absorbed by reactants. in an endothermic reaction, the products have more stored chemical energy than the reactants. and in this reaction the reactants are more stable than products before the compounds with less energy are always more stable.