Diffusion is the movement of a substance from an area of high concentration to an area of low concentration. This process occurs faster in gases and liquids than in solids because their particles move more freely and randomly.
The word "diffusion" comes from the Latin word diffundere, meaning "to spread out."
Increasing temperature or pressure speeds up the rate of diffusion.
Diffusion of Gases Gases have a remarkable property of spreading out and intermixing throughout the space available to them, even against gravity.
For example, if a bottle of ammonia is opened in one corner of a room, its smell can be detected in the opposite corner.
Let’s understand this with an example:
Suppose we have two gas jars — one containing air (colourless) and the other containing reddish-brown bromine gas. If we invert the air over the bromine jar and remove the cover between them, the gases begin to intermix. Over time, both jars appear reddish-brown.
Even though bromine is heavier than air, it travels upward while the lighter air moves downward. This happens due to the rapid movement of gas molecules and the presence of intermolecular spaces in gases. The high velocities of gas molecules allow them to overcome gravitational forces and mix with each other.
Thus, diffusion is defined as: The spontaneous intermixing of two or more gases, even against gravity.
Thomas Graham studied the diffusion of gases and formulated a relationship between the rate of diffusion and the density of a gas. This is known as Graham’s Law of Diffusion, which states:
At constant temperature and pressure, the rate of diffusion of a gas is inversely proportional to the square root of its density.
Mathematically:
Where:
If r₁ and r₂ are the rates of diffusion of two gases with densities d₁ and d₂ respectively, then:
Since the molecular mass (M) of a gas is twice its vapor density:
Where M₁ and M₂ are the molecular masses of the two gases.
The rate of diffusion of a gas is the ratio of the volume of the gas diffused to the time taken for diffusion:
Where V is the volume diffused and t is the time taken. If two gases diffuse for the same time, their relative rates of diffusion can be compared.
Effusion is a specific type of diffusion in which gas particles pass through a fine orifice or pinhole without colliding with each other.
Example 1: The rate of diffusion of hydrogen gas (H₂) and an unknown gas is 3:1, measured under the same temperature and pressure conditions. What is the molecular mass of the unknown gas?
Given:
Using Graham’s law of diffusion:
Where:
Substitute the given values:
Square both sides:
Solve for M2:
Answer: The molecular mass of the unknown gas is 18 g/mol.
Example 2: What will be the ratio of the rate of diffusion of CO2:CO if the initial moles of CO2 and CO are 4 mol and 5 mol, respectively?
Solution:
Graham’s Law of Diffusion, states:
Where:
Given:
Using Graham’s law:
Answer: The ratio of the rates of diffusion:
(Session 2025 - 26)