In any mixture of gases, each component gas exerts a partial pressure that contributes to the total pressure. At ordinary temperatures and pressure, you can apply the ideal gas law to calculate the partial pressure of each gas.

### What Is Partial Pressure?

Let's start by reviewing the concept of partial pressure. In a mixture of gases, the partial pressure of each gas is the pressure that gas would exert if it was the only one occupying that volume of space.

This assumes the temperature of the system is constant and the gas behaves as an ideal gas, following the ideal gas law:

PV = nRT

where P is pressure, V is volume, n is number of moles, R is the gas constant, and T is temperature.

The total pressure is then the sum of all the partial pressures of component gases. For *n* components of a gas:

P_{total} = P_{1} + P_{2} + P_{3} +... P_{n}

When written this way, this variation of the Ideal Gas Law is called Dalton's Law of Partial Pressures. Moving around terms, the law can be rewritten to relate moles of gas and total pressure to partial pressure:

P_{x} = P_{total} (n / n_{total})

**Partial Pressure Question**

A balloon contains 0.1 moles of oxygen and 0.4 moles of nitrogen. If the balloon is at standard temperature and pressure, what is the partial pressure of the nitrogen?

**Solution**

Partial pressure is found by Dalton's Law:

**P _{x} = P_{Total} ( n_{x} / n_{Total} )**

where

P_{x} = partial pressure of gas x

P_{Total} = total pressure of all gases

n_{x} = number of moles of gas x

n_{Total} = number of moles of all gases

**Step 1**

Find P_{Total}

Although the problem does not explicitly state the pressure, it does tell you the balloon is at standard temperature and pressure. Standard pressure is 1 atm.

**Step 2**

Add up the number of moles of the component gases to find n_{Total}

n_{Total} = n_{oxygen} + n_{nitrogen}

n_{Total} = 0.1 mol + 0.4 mol

n_{Total} = 0.5 mol

**Step 3**

Now you have all the information needed to plug the values into the equation and solve for P_{nitrogen}

P_{nitrogen} = P_{Total} ( n_{nitrogen} / n_{Total} )

P_{nitrogen} = 1 atm ( 0.4 mol / 0.5 mol )

P_{nitrogen} = 0.8 atm

**Answer**

The partial pressure of the nitrogen is 0.8 atm.

### Helpful Tip for Performing the Partial Pressure Calculation

- Be sure to report your units correctly! Typically, when using any form of the ideal gas law, you'll be dealing with moles, temperature in Kelvin, volume is in liters, and pressure is in atmospheres.
- Remember real gases are not ideal gases, so although the calculation will have very little error under ordinary conditions, it won't be precisely the true value. For most situations, the error is negligible.