Dalton's law of partial pressure ?

Dalton's law of partial pressure states that the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of each individual gas in the mixture. This means that each gas in a mixture exerts its own pressure independently of the other gases present. The partial pressure of a gas is the pressure that gas would exert if it were the only gas in the container.

Dalton's Law of Partial Pressures

Statement:
The total pressure exerted by a mixture of non-reacting gases is equal to the sum of the partial pressures of the individual gases.

Definition of Partial Pressure:
The partial pressure of a gas in a mixture is the pressure that the gas would exert if it occupied the entire volume of the mixture alone.

Mathematical Equation:
```
Total Pressure = P = P1 + P2 + P3 + ... + Pn
```
where:

- P is the total pressure
- Pi is the partial pressure of the ith gas
- n is the number of gases in the mixture

Assumptions:

- The gases are non-reacting, meaning they do not interact chemically with each other.
- The gases behave ideally, obeying the ideal gas law.
- The gases are all at the same temperature.

Applications:

- Determining the partial pressure of individual gases in a mixture
- Calculating the total pressure of a gas mixture
- Analyzing the effects of different gas compositions on pressure
- Used in fields such as scuba diving, meteorology, and gas chromatography

Example:

Suppose we have a mixture of nitrogen (N2) and oxygen (O2) in a closed container. The partial pressure of nitrogen is 20 kPa and the partial pressure of oxygen is 80 kPa. According to Dalton's law, the total pressure of the mixture is:

```
P = P1 + P2
P = 20 kPa + 80 kPa
P = 100 kPa
```