Why does 1 mole of any gas occupy the same volume?

Why does a mole of any gas occupy the same volume as a mole of any other gas?

Avogadro’s hypothesis states that equal volumes of all gases at the same temperature and pressure contain equal numbers of particles. Since the total volume that a gas occupies is made up primarily of the empty space between the particles, the actual size of the particles themselves is nearly negligible.

Is one mole of any gas the same volume?

At standard temperature and pressure, one mole of any gas will occupy a volume of 22.4 L.

Why does one mole of any gas always occupy the same volume 22.4 L at standard temperature and pressure?

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 x L at some other temperature-pressure conditions.

How much does 1 mole of gas weigh?

The weight of one mole of octane molecules will be equal to the summation of the weights of eight carbon atoms (at 12 grams/mole each, from carbon’s mass number) plus 18 hydrogen atoms (at 1 gram/mole each). So, doing the math (8 x 12 + 1 x 18), we see that octane weighs 114 grams/mole.

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What is Avogadro gas law formula?

Avogadro’s Law is stated mathematically as follows: Vn=k, where V is the volume of the gas, n is the number of moles of the gas, and k is a proportionality constant.

What is the relationship between volume and pressure?

It is summarized in the statement now known as Boyle’s law: The volume of a given amount of gas held at constant temperature is inversely proportional to the pressure under which it is measured.