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That's not true. The molar volume of a gas is always greater than the molar volume of a liquid. I can't think of any exceptions to this.
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)
The volume is 50 %; the molar volume is 22,414 L.
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)
22.4 dm³
Use Boyle's law
The molar volume at STP(22.4 L/mol) can be used to calculate the molar mass of the gas.
Because neither is an ideal gas. Ideal gas molecules are assumed to be points with no spatial extensions, gas molecules have a finite size. The van der Waals equations of state need to be applied. This is the main reason.
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.
This is the molar volume of an ideal gas at a given temperature and pressure.
That's not true. The molar volume of a gas is always greater than the molar volume of a liquid. I can't think of any exceptions to this.
No, the molar ratio is not necessarily the same as the volume ratio for non-gaseous reactions. The molar ratio refers to the ratio of the number of moles of reactants or products involved in a chemical reaction. It is determined by the balanced chemical equation. On the other hand, the volume ratio refers to the ratio of the volumes of reactants or products in a reaction. In some cases, the volume ratio may be equal to the molar ratio, especially for ideal gases at the same temperature and pressure. This is known as the ideal gas law and is represented by Avogadro's principle. However, for non-gaseous reactions, the volume ratio may not necessarily be equal to the molar ratio. This is because the volume of a substance is influenced by factors such as density, state (solid, liquid, or gas), and the presence of solvents or other compounds. Therefore, it is important to use the molar ratio when determining stoichiometry and reaction quantities, rather than relying solely on volume ratios.
The molar volume of an ideal gas at 25 0C and 100 kPa is 0,875 436 4 cubic feet.
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)
At Standard Temperature and Pressure (STP), which is defined as 0 degrees Celsius (273.15 Kelvin) and 1 atmosphere pressure, the molar volume of an ideal gas is approximately 22.4 liters/mol. The molar mass of nitrogen gas (N₂) is approximately 28.02 grams/mol. To calculate the density (D) of nitrogen gas at STP, you can use the ideal gas law: � = Molar mass Molar volume at STP D= Molar volume at STP Molar mass ​ � = 28.02   g/mol 22.4   L/mol D= 22.4L/mol 28.02g/mol ​ � ≈ 1.25   g/L D≈1.25g/L Therefore, the density of nitrogen gas at STP is approximately 1.25 grams per liter.
No. Specific volume is the inverse of density. Molar volume specific volume divided by mols. (i.e. g/(mLxMols)
molar volume