Partial Pressure Calculator
Welcome to the partial pressure calculator  a device that can help you determine and understand partial pressure. Interested in some of the laws of chemistry, such as Dalton's law of partial pressure? Want to know how to calculate partial pressure? Worry no more. We present you with four partial pressure formulas, so keep reading!
Are you're also interested in thermodynamics? If so, check out our combined gas law calculator.
Dalton's law of partial pressures
Pressure is the force applied orthogonally over a surface. If a mixture of ideal gases (i.e., where the molecules don't interact with each other) is sealed within a container, the gases will diffuse and fill up all of the available space. The partial pressure of one component of this mixture is the pressure that this individual gas exerts.
Dalton's law states that:
the total pressure exerted on a container's walls by a gas mixture is equal to the sum of the partial pressures of each separate gas.
It can also be illustrated with an equation:
total pressure = p_{1} + p_{2} + ... + p_{n}
,
where p_{1}
, p_{2}
, and so on, up to p_{n}
, represent the partial pressure of each gaseous component.
It can also be presented as follows:
partial pressure = total pressure * mole fraction
where mole fraction
is the ratio of moles of the selected gas to the moles of the entire gas mixture.
It shows that the partial pressure of one component is proportional to its mole fraction.
The above formula is one of our calculator's four partial pressure formulas. Which one you choose depends on the data you've collected beforehand.
How to calculate partial pressure?  Ideal gas law
The ideal gas law states that:
p * V = n * R * T
where:
p
is the pressure of the gasV
is the volume of the gasn
is the number of moles of the gasR
is the gas constant, 8.3145 ^{J}/_{mol*K}T
is the temperature of the gas
If you want to calculate the partial pressure of one component of a gas mixture, use the following formula (derived from the one above):
p_{i} = (n_{i} * R * T) / v
where:
p_{i}
is the partial pressure of the individual gasn_{i}
is the amount of moles of the individual gasT
is the temperature of the mixtureV
is the volume of the mixture
Now you know how to calculate partial pressure using the ideal gas law. Let's move on to the last two forms of the partial pressure equation  both using Henry's law.
Another partial pressure equations  Henry's law
Henry's law states that:
the partial pressure of a gas above a liquid is proportional to the amount of gas dissolved in that liquid.
The coefficient of this proportionality is the Henry's law constant. In the table below, you can find its value for some of the most common gases in water at 298 K:
Element  Henry's law constant [^{litre*atm}/_{mol}]  Henry's law constant [atm] 

O_{2}  769.23  4.259*10^{4} 
H_{2}  1282.05  7.099*10^{4} 
Co_{2}  29.41  0.163*10^{4} 
N_{2}  1639.34  9.077*10^{4} 
He  2702.7  14.97*10^{4} 
Ne  2222.22  12.3*10^{4} 
Ar  714.28  3.955*10^{4} 
CO  1052.63  5.828*10^{4} 
Henry's law is only accurate at low gas pressures (pressures < 1000 hPa), constant temperatures (usually 293.15 K) and when the molecules are at equilibrium.
How to find partial pressure with Henry's law constant? There are two methods:
 Where the concentration of the solute is given:
pressure = K_{H1} * concentration
where
K_{H1}
is Henry's law constant in [^{litre*atm}/_{mol}].
 Where the mole fraction of the solute is given:
pressure = K_{H2} * mole fraction
where
K_{H2}
is Henry's law constant in [atm].
Let's use the Henry's law equation in an example. Let's say that you want to calculate the partial pressure of dinitrogen (N_{2}) in a container. Its concentration is 1.5 moles / L. All you need to do is check the Henry's law constant in the table above, and input the numbers into the partial pressure formula:
pressure = 1.5 ^{mol}/_{litre} * 1639.34 ^{litre*atm}/_{mol} = 2459 atm = 249159 kPa
Simple, right?
Fun facts about pressure

It is essential to consider pressure if you are an underwater diver. Divers usually breathe a mixture of oxygen and nitrogen. When diving down to about 35 meters, the standard mixture is safe. As the pressure increases during deeper dives, oxygen becomes toxic, potentially causing narcosis. That's why technical divers (those who dive very deep) use different breathing mixtures to casual divers.

In medicine, while performing an arterialblood gas test, physicians measure the partial pressure of carbon dioxide and oxygen. With these measurements, they can calculate the pH of their patient's blood.

You might find it surprising that air pressure changes with altitude and temperature. It's important for people trekking up high mountains  the lower the pressure, the harder it is to breathe.