Avogadro's Law

What is Avogadro’s Law?

Avogadro’s law, also known as Avogadro’s principle or Avogadro’s hypothesis, is a gas law which states that the total number of atoms/molecules of a gas (i.e. the amount of gaseous substance) is directly proportional to the volume occupied by the gas at constant temperature and pressure.

Avogadro’s law is closely related to the ideal gas equation since it links temperature, pressure, volume, and amount of substance for a given gas.

Table of Content

• Formula and Graphical Representation
• Derivation
• Molar Volume of a Gas
• Examples of Avogadros Law
• What are the Limitations of Avogadro’s Law?
• Solved Exercises on Avogadro’s Law
• Recommended Videos
• Frequently Asked Questions – FAQs

Avogadro’s law is named after the Italian scientist Amedeo Carlo Avogadro, who suggested that two dissimilar ideal gases occupying the same volume at a given (constant) temperature and pressure must contain an equal number of molecules.

Formula and Graphical Representation

At constant pressure and temperature, Avogadro’s law can be expressed via the following formula:

V ∝ n

V/n = k

Where V is the volume of the gas, n denotes the amount of gaseous substance (often expressed in moles), and k is a constant. When the amount of gaseous substance is increased, the corresponding increase in the volume occupied by the gas can be calculated with the help of the following formula:

V₁/n₁ = V₂/n₂ ( = k, as per Avogadro’s law).

The graphical representation of Avogadro’s law (with the amount of substance on the X-axis and volume on the Y-axis) is illustrated below.

Here, the straight line (which indicates that the two quantities are directly proportional) passes through the origin, implying that zero moles of gas will occupy zero volume.

Derivation

Avogadro’s law can be derived from the ideal gas equation, which can be expressed as follows:

PV = nRT

Where,

• ‘P’ is the pressure exerted by the gas on the walls of its container
• ‘V’ is the volume occupied by the gas
• ‘n’ is the amount of gaseous substance (number of moles of gas)
• ‘R’ is the universal gas constant
• ‘T’ is the absolute temperature of the gas

Rearranging the ideal gas equation, the following equation can be obtained.

V/n = (RT)/P

Here, the value of (RT)/P is a constant (since the temperature and pressure kept constant and the product/quotient of two or more constants is always a constant). Therefore:

V/n = k

Thus, the proportionality between the volume occupied by a gas and the number of gaseous molecules is verified.

Molar Volume of a Gas

As per Avogadro’s law, the ratio of volume and amount of gaseous substance is a constant (at constant pressure and temperature). The value of this constant (k) can be determined with the help of the following equation:

k = (RT)/P

Under standard conditions for temperature and pressure, the value of T corresponds to 273.15 Kelvin and the value of P corresponds to 101.325 kilo Pascals. Therefore, the volume occupied by one mole of a gas at STP is:

Volume occupied by 1 mole of gas = (8.314 J.mol^-1.K^-1)*(273.15 K)/(101.325 kPa) = 22.4 litres

Therefore, one mole of any gaseous substance occupies 22.4 litres of volume at STP.

Examples of Avogadros Law

The process of respiration is a great example of Avogadro’s law. When humans inhale, the increase in the molar quantity of air in the lungs is accompanied by an increase in the volume of the lungs (expansion of the lungs). An image detailing the change in volume brought on by an increase in the number of gaseous molecules is provided below.

Another common example of Avogadro’s law is the deflation of automobile tyres. When the air trapped inside the tyre escapes, the number of moles of air present in the tyre decreases. This results in a decrease in the volume occupied by the gas, causing the tyre to lose its shape and deflate.

What are the Limitations of Avogadro’s Law?

Despite being perfectly applicable to ideal gases, Avogadro’s law provides only approximate relationships for real gases. The deviation of real gases from ideal behaviour increases at low pressure and high temperature.

It is important to note that gases molecules having relatively low molecular masses (such as helium and hydrogen) obey Avogadro’s law to a greater extent than heavier molecules.

Solved Exercises on Avogadro’s Law

Example 1

One mole of helium gas fills up an empty balloon to a volume of 1.5 litres. What would be the volume of the balloon if an additional 2.5 moles of helium gas is added? (Assume that the temperature and the pressure are kept constant)

Given,

The initial amount of helium (n₁) = 1 mol

The initial volume of the balloon (V₁) = 1.5 L

The final amount of helium (n₂) = 1 mol + 2.5 mol = 3.5 mol

As per Avogadro’s law, V₁/n₁ = V₂/n₂

Therefore, the final volume of the balloon (V₂) = (V₁n₂)/n₁ = (1.5L*3.5mol)/1mol = 5.25 L

The balloon would occupy a volume of 5.25 litres when it contains 3.5 moles of helium gas.

Example 2

A tyre containing 10 moles of air and occupying a volume of 40L loses half its volume due to a puncture. Considering that the pressure and temperature remain constant, what would be the amount of air in the deflated tyre?

Given,

The initial amount of air (n₁) = 10 mol

The initial volume of the tyre (V₁) = 40 L

The final volume of the tyre (V₂) = 20 L

According to Avogadro’s law, the final amount of air in the tyre (n₂) = (V₂n₁)/V₁ = 5 moles.

The deflated tyre would contain 5 moles of air.

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