Waiting for answer This question has not been answered yet. You can hire a professional tutor to get the answer.

QUESTION

states that, at the same temperature and pressure, equal volumes of all gases have the same number of molecules.

Another statement is, volume is directly proportional to the number of moles. The volume increases as the number of moles increases. It does not depend on the sizes or the masses of the molecules.

V ∝ n, where V is the volume and n is the number of moles.

V/n = k, where k is a proportionality constant.

We can rewrite this as

V_1/n_1 = V_2/n_2

Equal volumes of hydrogen, oxygen, or carbon dioxide contain the same number of molecules.

One mole of an ideal gas occupies 22.4 L at STP. This is its molar volume.

Example Problem:

A 6.00 L sample at 25.0 °C and 2.00 atm contains 0.500 mol of a gas. If we add 0.250 mol of gas at the same pressure and temperature, what is the final total volume of the gas?

Solution:

The formula for Avogadro's law is:

V_1/n_1 = V_2/n_2

V₁ = 6.00 L; n₁ = 0.500 mol

V₂ = ?; n₂ = 0.500 mol + 0.250 mol = 0.750 mol

V_2 = V_1 × n_2/n_1

V_2 = 6.00 L × (0.750 mol)/(0.500 mol) = 9.00 L