Molar gas volume is the volume of ONE moel of gas. It only depends on the pressure and temperature, not on the kind of gas. Molar volume at standard temperature and standard pressure is always 22,4 Litres (for any gas)
Molar volume of a gas is the volume that one mole will occupy. At STP, that value is 22.4 liters.
The molar volume of a liquid is greater than that of a gas because in a liquid, the particles are closer together and have stronger intermolecular forces holding them in place, resulting in a higher density compared to a gas where particles are more spread out and have weak intermolecular forces. This leads to a smaller volume per mole for gases compared to liquids.
Molar volume of gas is the volume which one mole of the gas occupies. According to Avogradro's law, ALL GAS HAVE THE SAME VOLUME AT THE SAME PRESSURE AND TEMPERATURE. So one mole of all gases occupies 22.4dm3 at s.t.p (273K 760mmHg) - i.e 22.4dm3 is the molar volume of all gases at s.t.p. (you can convert to other conditions of temperature and pressure using Boyle's, Charles' or General gas equations)
The molar volume of a gas at STP (standard temperature and pressure) is 22.4 L/mol. To calculate the molar mass of the gas, you can use the formula: Molar mass = (mass of gas / volume of gas) x molar volume at STP. In this case, with a mass of 60g and a volume of 5.6 dm3, the molar mass would be 60g/5.6dm3 x 22.4L/mol = 240 g/mol. Vapour density is calculated as 2 x molar mass, so in this case the vapour density would be 480 g/mol.
22.4 dm³
Molar volume is based on the volume occupied by one mole of gas molecules at a specific temperature and pressure. It is a macroscopic property and averages out the effect of individual gas particle size because the volume of the container is much larger compared to the size of gas particles. This allows molar volume to be consistent regardless of the size of the gas particles.
The molar volume of a liquid is greater than that of a gas because in a liquid, the particles are closer together and have stronger intermolecular forces holding them in place, resulting in a higher density compared to a gas where particles are more spread out and have weak intermolecular forces. This leads to a smaller volume per mole for gases compared to liquids.
Molar volume of gas is the volume which one mole of the gas occupies. According to Avogradro's law, ALL GAS HAVE THE SAME VOLUME AT THE SAME PRESSURE AND TEMPERATURE. So one mole of all gases occupies 22.4dm3 at s.t.p (273K 760mmHg) - i.e 22.4dm3 is the molar volume of all gases at s.t.p. (you can convert to other conditions of temperature and pressure using Boyle's, Charles' or General gas equations)
In the van der Waals equation, the excluded volume is considered to be less than the molar volume because it accounts for the volume occupied by gas molecules themselves, which reduces the available space for the gas particles to move around freely. This reduced effective volume results in a difference between the molar volume and the true volume of the gas.
The molar volume doesn't depend on the identity of the gas. One mole of any ideal gas at STP will occupy 22.4 liters.
22.4 dm³
You can find molar volume by dividing the volume of a gas by the number of moles of gas present. The equation to calculate molar volume is V = nRT/P, where V is volume, n is the number of moles, R is the ideal gas constant, T is temperature, and P is pressure.
At STP (standard temperature and pressure), one mole of any gas occupies a volume of 22.4 liters. This is known as the molar volume of a gas at STP.
The molar volume of hydrogen gas at STP (Standard Temperature and Pressure) is 22.4 liters per mole.
Use Boyle's law
Molar volume is based on the volume occupied by one mole of gas molecules at a specific temperature and pressure. It is a macroscopic property and averages out the effect of individual gas particle size because the volume of the container is much larger compared to the size of gas particles. This allows molar volume to be consistent regardless of the size of the gas particles.
Molar volume is the volume occupied by one mole of a substance at a specific temperature and pressure, typically measured in liters per mole. Molal volume is the volume of solvent used to dissolve one mole of solute and is typically expressed in liters per mole. Both are important concepts in chemistry for determining the properties of substances and solutions.
To find the density of fluorine gas, we first need to calculate the molar volume of the gas using the ideal gas law equation PV = nRT. From there, we can convert the molar volume to L/mol. Finally, we can find the density by dividing the molar mass by the molar volume. The density of fluorine gas at 7.00 x 10^2 torr and 27.0ºC is approximately 1.5 g/L.