Question

Using Avogadro's hypothesis prove that molar volume of any gas is 22.4 litre at STP.​

Answer 1

Answer:

Explanation:

In 1811, Amadeo Avogadro explained that the volumes of all gases can be easily determined. 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. A given volume of a gas with small light particles such as hydrogen  (H2)  contains the same number of particles as the same volume of a heavy gas with large particles such as sulfur hexafluoride,  SF6 .

Gases are compressible, meaning that when put under high pressure, the particles are forced closer to one another. This decreases the amount of empty space and reduces the volume of the gas. Gas volume is also affected by temperature. When a gas is heated, its molecules move faster and the gas expands. Because of the variation in gas volume due to pressure and temperature changes, the comparison of gas volumes must be done at one standard temperature and pressure. Standard temperature and pressure (STP) is defined as  0oC   (273.15K)  and  1atm  pressure. The molar volume of a gas is the volume of one mole of a gas at STP. At STP, one mole ( 6.02×1023  representative particles) of any gas occupies a volume of  22.4L

Answer 2

Answer:

All gases will occupy a volume of 22.4L at 273K and 1 atm pressure. Standard pressure is 1 atmosphere or 760 mm Hg. The proof of this, has been shown using Avogadro's hypothsis.

Explanation:

The molar volume of a gas is the volume of one mole of a gas at STP. At STP, temperature is taken as 273K and pressure is taken as 1atm. We can use the equation of ideal gas to calculate the volume of 1 mole of gas.

Complete step by step answer:

At STP, one mole (6.023×1023

representative particles) of any gas occupies a volume of 22.4L . A mole of any gas occupies 22.4L at standard temperature and pressure (273K and 1atm).

PV=nRT

Where P=1atm,R=0.0821Latmmol−1K−1,T=273K,n=1mol

Substituting these values in the above equation we get,

1×V=1×0.08201×273

V=1×0.08201×273

V=22.4L

Standard Molar Volume of any gas is defined as the volume occupied by one mole of that gas at STP. Standard temperature is 0∘C

or 273 K.The above statement was a law given by Avogadro. It is an experimental gas law relating the volume of a gas to the amount of substance of gas present in that particular volume. This law is a specific case of the ideal gas law. Avogadro's law states that "equal volumes of all gases, at the same temperature and pressure, have the same number of particles."

Thus, all gases will occupy a volume of 22.4L at 273K and 1 atm pressure. Standard pressure is 1 atmosphere or 760 mm Hg. So 1 mole of any gas at STP occupies 22.4 litres of volume

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