If I remember correctly it is a little more complicated than that. The general equation PV=nRT for an ideal gas is elementary knowledge. The fact is that when you increase temperature many things can happen. It depends on how you treat your system. In general if you increase temperature in an open system the pressure will remain fairly constant, but the volume will increase. If it is a closed system in which the volume is not allowed to expand the pressure will increase with increased temperature. You also have to remember chemical properties also such as phase changes. Hope that rambling mess helps lol.
The Standard Gas Law; PV=nrt shows, by inspection, if no other variable changes, pressure decrease will result in temperature decrease. And, of course, vice versa.
It's important to note that this is not valid in the free atmosphere because this assumes a constant volume. In reality, when air warms, volume increases and pressure will remain the same.
Not really, The opposite in a closed container. If you're referring to the atmosphere generally, there are a lot of other factors, but it sort of describes barometric pressure.
That is false. Volume increases when pressure decreases. From Boyle's law, P1V1 = P2V2 at constant temperature, or PV = a constant at constant temperature.
That is false. Volume increases when pressure decreases. FromBoyle's law, P1V1 = P2V2 at constant temperature, or PV = aconstant at constant temperature.
It increases because it just does
False, see Boyle's law
I think you meant what happens to the gas particles when the temperature decreases. If the volume of gas is constant(eg in a fixed container), the pressure of the gas will decrease. If the gas is in a container with a variable volume(eg. balloon), the volume of gas will decrease.
A loss of gas, or a decrease in temperature.
If the temperature decreases, the volume is also going to decrease, and if the pressure decreases, the volume is going to increase. So they balance each other out, if they are decreased at the same rate.
For a given mass at constant temperature, the pressure time tghe volume is a constant. pV=C
If the volume is constant, the density does not change with temperature. With increasing temperature there is still the same number of molecules confined to the same volume of space, so no difference in density.
as the pressure decreases the volume of gas increases at constant temperature
At constant temperature p.V=constant, so pressure INcreases when decreasing the volume.
Assuming the volume is kept constant, the pressure will also decrease in this case.
False, see Boyle's law
...pressure decreases.
...pressure decreases.
...pressure decreases.
Temperature is directly proportional to volume i.e. as temperature increases volume of gas also increases and as it decreases, the volume also decreases
kinetic energy increases with the increase in temperature is a postulate in kinetic molecular theory of matter.if the pressure is kept constant when temperature decreases the kinetic energy of the molecules decreases resulting in decrease in the volume of the gas. Charle's Law state's that For a given mass of dry gas at constant pressure ,volume is directionally proportional to temperature ie V~T
It will increase? No it will decrease when the same amount of gas is held at constant temperature.
As pressure increases, if temperature is constant, the gas will decrease in volume.
I think you meant what happens to the gas particles when the temperature decreases. If the volume of gas is constant(eg in a fixed container), the pressure of the gas will decrease. If the gas is in a container with a variable volume(eg. balloon), the volume of gas will decrease.