PV = nRT is the written equation for the ideal gas law and I think it would be useful if we could talk about what is really happening in this equation.
Now, an ideal gas is described in a theoretical outline that pretty much just says that a gas made of particles would have elastic collisions and no intermolecular forces hampering its expansion to a certain volume. This model is useful because it ignores some of the more delicate issues of gases by making assumptions.
Ok so for the PV, the pressure and volume of a gas are proportional that is if all else is kept constant, a decrease in volume, which would force these active gas particles closer together, would increase pressure.
Now the other side of the equation is nRT. R is a constant for an amount of pressure which is inversely proportional to the moles in question and temperature, it depends on which metric you are using. Temperature is T, the kinetic energy of molecules, and n is the number of moles and moles are a whole thing, something times Avagrado's number. So the higher the temperature, it would produce higher pressures and volumes for the same quantity of moles. A high amount of moles would have a higher pressure and volume for a fixed temperature.