What happens to temperature of a gas when pressure increases?
When you increase the pressure and compress the molecules they start to move faster and that raises the temperature. The gas from is compressible, it will not keep the same volume as it is compressed. If the pressure stay the same the volume stay the same. You are not paying attention in class. If you have a air compressor with tank, and you turn it on after it is run a while, you can not touch the air line to tank as it will burn your hand, turn off the compress and check the pressure. Come back in the morning and you can touch the compressor all over, it will be cool, recheck the tank pressure , and it will be the same as it was the night before. You draw the conclusion.
Let’s visualize this with the ideal gas equation: PV = nRT, where P = pressure V = volume n = number of moles R = Reynold’s constant T = temperature So your first question asks what happens to the temperature when pressure INCREASES. From the equation PV = nRT, if volume remains constant but pressure goes up, we see that the right side of the equation must go up to balance with the overall increase on the left side of the equation. Since n and R don’t change, temperature must go UP. Similarly, PV = nRT can be used for the second question as well. If temperature decreases and pressure remains constant, in order to compensate for the decrease on the right hand side of the equation (the “nRT” part), the volume must DECREASE (since pressure is constant and there’s nothing else to change but volume on the left side).
