The relationship between pressure and moles, when volume and temperature of a gas are held constant, is: P/n = k We could say then, that: If the number of moles is doubled, the pressure is halved. If the number of moles if halved, the pressure is doubled. If the number of moles is tripled, the pressure also triples. If the number of moles is halved, the pressure is quadrupled.

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The relationship between pressure and moles, when volume and temperature of a gas are held constant, is: P/n = k We could say then, that: If the number of moles is doubled, the pressure is halved. If the number of moles if halved, the pressure is doubled. If the number of moles is tripled, the pressure also triples. If the number of moles is halved, the pressure is quadrupled.

Chemistry
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P is proportional to n so, If the number of moles is tripled, the pressure also triples. If the number of moles is doubled, the pressure also doubled. Its like that.
The simplest way to explain this is like this: |dw:1439953251277:dw| let's look at this figure. say we keep the volume constant so we have in our formula \[P _{1}T _{1} = P _{2}T _{2}\] if we have 2 cylinders. A is at 298K and B is at say 300K if we keep volume constant, you notice that temperature = average kinetic energy of the particles right? that means how fast they move around. If we increase the temperature the gas molecules move faster and faster, which means that they hit the walls of the container more, at higher temperatures. if they hit the walls of the container more then that means that the pressure goes up as well. so when we raise the temperature we also raise the pressure (when we keep volume constant).

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