We can continue using the ideal gas model to quantify parameters of a gaseous substance. The ideal gas law shows the relationship between factors that affect gases:
PV = nRT, where: P is pressure; V is volume; n is the number of moles; R is the universal gas constant (8.314 J/K/mol), and T is temperature (Kelvin).
Question: If the pressure of a gas increases while its volume stays the same, what will happen to its temperature?
Refer to the ideal gas law equation above. If pressure is increased (on the left side of the equation) and volume does not change, a factor on the right side of the equation must increase as well. The amount of gas (n) cannot change, so temperature must increase.
Think of a box that contains millions of tiny air molecules bouncing around and colliding. To increase the pressure (more collisions between the molecule and the container), the molecules must move faster. Faster moving molecules have more energy, and thus a higher temperature.
Question: How is the temperature of a gas affected if volume increases while pressure remains the same?