Need to solve for pressure, volume, or temperature? Our Perfect Gas Law Calculator helps you instantly determine the missing variable in the Ideal Gas Equation ($PV=nRT$). Whether you’re a student or a professional engineer, get accurate results and step-by-step breakdowns below.
Perfect Gas Law Calculator
Leave one field empty to calculate its value.
Perfect Gas Law Formula:
Source: Ideal Gas Law (Wikipedia) | LibreTexts Chemistry
Variables:
- P: Pressure (measured in atm)
- V: Volume (measured in Liters)
- n: Amount of substance (in moles)
- R: Gas Constant ($0.08206\text{ L}\cdot\text{atm/mol}\cdot\text{K}$)
- T: Absolute Temperature (in Kelvin)
Related Calculators:
- Boyle’s Law Calculator
- Charles’s Law Calculator
- Gay-Lussac’s Law Calculator
- Combined Gas Law Calculator
What is the Perfect Gas Law Calculator?
The perfect gas law calculator is an online tool designed to solve for any variable in the state equation of a hypothetical ideal gas. It relates pressure, volume, temperature, and quantity of gas particles.
By assuming particles have no volume and no intermolecular forces, the Ideal Gas Law provides an excellent approximation for real gases under high temperatures and low pressures.
How to Calculate (Example):
Suppose you have 2 moles of gas at a temperature of 300K in a 10L container. To find the pressure:
- Identify given values: $n=2$, $T=300$, $V=10$, $R=0.08206$.
- Rearrange formula for P: $P = \frac{nRT}{V}$.
- Calculate: $P = \frac{2 \times 0.08206 \times 300}{10} = 4.9236\text{ atm}$.
Frequently Asked Questions (FAQ):
What is the difference between ideal gas and perfect gas? Often used interchangeably, a perfect gas is an ideal gas that also has constant specific heats.
Does this use Celsius or Kelvin? You must use Kelvin. To convert Celsius to Kelvin, add 273.15.
What happens if the pressure is too high? Real gases deviate from the ideal behavior as intermolecular forces become significant.
What is the R value used? We use the standard atmospheric constant: $0.08206\text{ L}\cdot\text{atm}\cdot\text{mol}^{-1}\cdot\text{K}^{-1}$.