Do all gases have the same molar volume at the same temperature and pressure?

Do all gases have the same molar volume at the same temperature and pressure?

A modern statement is: Avogadro’s law states that “equal volumes of all gases, at the same temperature and pressure, have the same number of molecules.” For a given mass of an ideal gas, the volume and amount (moles) of the gas are directly proportional if the temperature and pressure are constant.

Does molar volume change with temperature and pressure?

According to Boyle’s Law, the volume and pressure of a gas are inversely proportional (as long as temperature remains constant).

Why do all gases have the same molar volume?

Consider this: If the pressure of a gas is equal to the force exerted by gas particles pushing on the sides of whatever container it’s stored in, and the volume of a gas depends on its pressure (Boyle’s Law), then the molar volumes of every gas are the same.

Why do all gases have the same volume?

As all gases that are behaving ideally have the same number density, they will all have the same molar volume. At STP this will be 22.4 L. This is useful if you want to envision the distance between molecules in different samples. For instance if you have a sample of liquid water, it has a mass density of 1 g mL-1.

Does the molar volume of a gas depend on pressure and temperature?

The volume of gas is proportional to many different factors, though. Based on the ideal gas equation, volume is proportional to moles and temperature. It is inversely proportional to pressure.

What is the difference between molar volume and standard molar volume?

Summary – STP vs Standard Molar Volume Standard molar volume is the volume of a mole of a substance at STP. The difference between STP and standard molar volume is that STP gives temperature by the unit K (Kelvin) and pressure by Pa (Pascal) whereas standard molar volume is given by L/mol (Liters per mole) unit.

What would happen to V if’n is increased?

If V increases, n increases. If V decreases, n decreases. Avogadro’s Law states that if P and T are constant, the volume is directly proportional to the number of moles. If the amount of gas in a container is increased, the volume increases.

Can two different sized molecules have the same molar volume?

You have the right thought process; if two real gases have different sized molecules, they won’t have the same molar volume. The issue is that your statement about gases at STP refers to ideal gases which by assumption are just point particles that only interact via elastic collisions.

Why are the pressures of different gases the same?

Even though the particle sizes are different for each case (think about a real case with helium, neon, and argon), the pressures would all be the same. Why? Because number density is what governs pressure for a gas system where temperature is constant. The number densities here are all the same, 10 particles per unit of volume.

Why does one mole of gases occupy the same space?

According to my thinking, it may be due to equal diffusion of all particles when at a particular temperature and pressure. So going by this, one mole of all gases should occupy the same at some other temperature-pressure conditions.

What is the molar volume of an ideal gas?

The molar volume, symbol V m is the volume occupied by one mole of a substance (chemical element or chemical compound) at a given temperature and pressure. At S.T.P conditions the molar volume of any ideal gas is 22.711 d m 3.