The ideal Gas Law states the following:
pV=nRT
p=pressure [pa]
V=volume [m³]
n=number of moles
R=constant
T=temperature [K]
So, if you multiply the number of moles by 2, and all the other variables are not changed, your volume will also be multiplied by 2.
The volume is doubled.
At a constant volume the pressure increase.
The ideal Gas Law states the following: pV=nRT p=pressure [pa] V=volume [m³] n=number of moles R=constant T=temperature [K] So, if you multiply the number of moles by 2, and all the other variables are not changed, your volume will also be multiplied by 2.
the volume doubles
The product PV remain constant in a closed system at constant temperature.
The volume is doubled.
At a constant volume the pressure increase.
The ideal Gas Law states the following: pV=nRT p=pressure [pa] V=volume [m³] n=number of moles R=constant T=temperature [K] So, if you multiply the number of moles by 2, and all the other variables are not changed, your volume will also be multiplied by 2.
the volume doubles
the volume doubles
The product PV remain constant in a closed system at constant temperature.
If the number of moles of a gas doubles at constant pressure and temperature, the volume of the gas will also double according to Avogadro's law. This is because the volume of a gas is directly proportional to the number of moles present.
When the number of moles of a gas doubles and all else is constant, then the volume also doubles.
When the number of moles of a gas doubles and all else is constant, then the volume also doubles.
If the number of moles of gas decreases, the volume of the gas will decrease as well, assuming constant temperature and pressure. This is described by Boyle's Law, which states that the volume of a gas is inversely proportional to the number of moles of gas when pressure and temperature are held constant.
When the number of moles of a gas doubles and all else is constant, then the volume also doubles.
The volumes doubles