If a gas is kept in a container with a constant volume and the pressure is reduced, how will the temperature of the gas be affected? a. it will increase. b. it will remain constant. c. none of these d. it will decrease.

Gases are intricate. They contain countless trillions of energetic gas molecules that can collide and possibly interact. Since it's challenging to precisely characterize a real gas, the idea of an ideal gas was developed as a rough approximation that aids in modeling and predicting the behavior of real gases. The phrase ideal gas refers to a fictitious gas made up of molecules that observe the following principles:

The molecules in an ideal gas are not attracted to or drawn away from one another.
The molecules of an ideal gas occupy no space.

The ideal gas equation can be given as:

PV = nRT

where;

P =pressure,

V = volume,

n = moles of gas,

R = rydberg constant,

T = temperature.

The pressure law states that for a constant volume of gas in a container, the temperature of the gas is directly proportional to its pressure which means there are more collisions with each other and the sides of the container and hence the pressure is increased.

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