If the number of moles doubles, the volume will also double, all things being equal.
When the number of moles of a gas doubles and all else is constant, then the volume also doubles.
According to Boyle's Law, if the volume of a gas is decreased while keeping the temperature and number of gas particles constant, the pressure of the gas will increase. This is because there is less space for the gas particles to occupy, leading to more frequent collisions with the walls of the container, resulting in an increased pressure.
If the volume is doubled and the number of molecules is doubled while the temperature is held constant, the pressure of the gas sample will remain the same. This is because both the volume and the number of molecules increased by the same factor, resulting in no net change in pressure according to the ideal gas law.
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.
The number of atoms in a mole of any pure substance is called?
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 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.
The product PV remain constant in a closed system at constant temperature.
At a constant volume the pressure increase.
The volumes doubles
The volumes doubles
The volumes doubles
the volume doubles
Increasing the temperature the number of particles remain constant and the pressure increase.
the volume doubles