Dalton's Law of Partial Pressures
Imagine you're in a room full of people talking. Each person contributes to the overall noise. If you could somehow measure the sound from just one person, that's their "partial noise." The total noise is just the sum of everyone's individual contributions. Gases behave the same way.
When you have a mixture of gases — say oxygen, nitrogen, and carbon dioxide — each gas behaves as if it were alone in the container. It doesn't care about the other gases. It bounces around, hits the walls, and exerts its own pressure. That pressure is called its partial pressure.
The key assumption: the gases must not react with each other. If they react, the rule breaks down.
The Precise Statement
Dalton's Law of Partial Pressures says:
The total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of each individual gas.
Mathematically:
Ptotal=P1+P2+P3+…
where P1, P2, P3, etc. are the partial pressures of each gas.
What Exactly Is a Partial Pressure?
The partial pressure of a gas in a mixture is the pressure that gas would exert if it alone occupied the entire container at the same temperature.
Think of it this way: if you have a 1-litre flask containing oxygen and nitrogen at room temperature, the oxygen molecules don't know the nitrogen molecules exist. They just keep hitting the walls. The pressure from oxygen alone is its partial pressure. The pressure from nitrogen alone is its partial pressure. Add them up, and you get the total pressure.
Pi=ntotalni×Ptotal
Here ni is the number of moles of gas i, and ntotal is the total number of moles. This formula lets you find a gas's partial pressure if you know its mole fraction and the total pressure.
Why Does This Work?
Gases are mostly empty space. The molecules are far apart and move independently. In an ideal gas, there are no attractive or repulsive forces between molecules. So each gas in a mixture behaves exactly as it would alone. The pressure each gas exerts depends only on its own number of molecules, not on what other gases are present.
Dalton's Law works perfectly for ideal gases. Real gases at very high pressures or low temperatures may show small deviations because molecules do interact slightly. But for most exam problems, you treat them as ideal.
A Simple Example
Suppose you have a container with 2 moles of oxygen and 3 moles of nitrogen at a total pressure of 5 atm. The mole fraction of oxygen is 2/5=0.4, and of nitrogen is 3/5=0.6.
Partial pressure of oxygen: 0.4×5=2 atm
Partial pressure of nitrogen: 0.6×5=3 atm
Total: 2+3=5 atm — checks out.
Why It Matters
Dalton's Law is everywhere in chemistry and biology. When you breathe, the partial pressure of oxygen in your lungs determines how much oxygen enters your blood. In scuba diving, the partial pressure of nitrogen affects decompression sickness. In industrial processes, knowing partial pressures helps control reaction rates.
The core idea: in a mixture of non-reacting gases, each gas is independent. Its contribution to total pressure is its partial pressure, and the total is just the sum.
Dalton's law of partial pressures is a standard NCERT/CBSE Class 11 Chemistry topic under states of matter, and "Dalton's law of partial pressures formula and numericals" is a commonly searched revision query. It's also a recurring important-question topic in JEE Main and NEET, especially in gas-mixture and mole-fraction problems.