How does temperature affect pressure at constant volume?

Answer 1

For the purpose of understanding this, think of temperature as movement - high temperature means the particles are excited, moving around with more energy. Think of pressure as how much those particles are 'trying to move apart' on average due to hitting each other and bouncing around.

If you want to increase the temperature without making them interact more (pressure), they need more room to move (volume).

It's a gross over-simplification of the physics, but it should help to visualize why the laws relating temperature, volume, and pressure are what they are.

Answer 2

Being given a constant volume, perhaps a sealed container, we also know that the mass can also not change significantly(E=mc2) with a change in temperature/energy. Temperature and pressure are propotional to each other and can be related to each other with the ideal gas equation PV=nRT, as well as others, but this is the most simple.

Firstly the question "what is pressure?" must be answered. Simply put it is the amount of particle collisions take place within a volume in a specific time. The more energy these particles have, the faster they move, and logically more collisions will take place within the same time period than the gas with less energy. The contrary would also be true i.e. decreasing the energy of this system=less pressure.

In answer to your question, it follows rather logically that temperature provides or removes energy from the given system depending on the difference between system and ambient/source temperatures.

I hope this helps =)

Answer 3

Pressure is proportional to temperature when the volume is held constant of an ideal gas.

Ideal Gas Law states:

PV=nRT or P=(nRT)/V

if the moles and volume are constant (R is always constant) we can call the (nR)/V portion of this constant c, so using this

P=cT

Answer 4

A direct relationship.

This means that when one variable goes up, the other also goes up. If one variable goes down, the other also goes down.

As the gas gets more compressed, the molecules have less space to move around , and they bump into each other more often, which means higher temperature. As a gas has less pressure, the molecules have more space to move around, bump into each other less, which means a lower temperature.

Answer 5

That depends on what the system is being subjected to...

If work is done on a system at constant volume, the temperature would be expected to increase. If heat is transferred out of a system at constant volume, the temperature it expected to increase. Chemical changes in a system may increase or decrease the temperature depending on what change occurs. Phase changes can occur at constant volume with no change in the temperature at all.

Answer 6

Change in volume is impossible at constant volume.

Answer 7

Gay-Lussac's law

Answer 8

V1/t1=v2/t2

Answer 9

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