How does temperature affect the ideal gas law?

As the temperature is increased, the gas becomes more "ideal" and the same is true if the pressure is decreased/volume increased.

As temperature increases or decreases, certain quantities are affected...let's start with what is the ideal gas law!

##PV## = ##nRT##

The product of ##P## and volume ##V## is equal to the product of the number of moles ##n## and the ideal gas constant ##R## and temperature ##T##.

##R## = ##8.31## ##J/(mol*K)##

Let's imagine a container filled with an ideal gas and the piston is fixed in place.

If I add heat to the system, the temperature ##T## will increase...what about the other quantities?

Remember the piston is fixed so the volume ##V## will remain constant. But the right side of the equation has increased! Therefore the pressure ##P## will increase. What if the piston is allowed to move?

If I remove the heat source the ##T## will decrease. This will lower the amount of that the particles will have. This means that they will exert less pressure on the container! So pressure on the moveable piston will decrease, then it will begin to lower, decreasing the volume!

As the temperature is increased, the gas becomes more "ideal". The same is true if the pressure is decreased/volume increased.