Ideal Gas State Equation

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Temperature:
Kelvin
Pressure:
atm
Gas Constant:
J/kg*K
Mass:
kg
Specific Volume:
m^3/kg
Specific Volume:
lb/feet^3
Volume:
m^3
Density:
kg/m^3

The Ideal Gas Law is a fundamental equation in thermodynamics that describes the relationship between the pressure, volume, temperature, and quantity of gas in a system. The equation is written as:

PV=nRT

Where:

P = Pressure of the gas
V = Volume of the gas
n = Number of moles of gas
R = Universal gas constant (8.314 J/(mol·K))
T = Temperature in Kelvin (K)
Why it's important:
The Ideal Gas Law helps predict the behavior of gases under various conditions. It's used in many fields, including chemistry, physics, engineering, and environmental science. While it's an idealization (it assumes gases behave perfectly), it works well for many gases at high temperatures and low pressures.

How it works:
The equation expresses how gases behave in a closed system:

When you increase the temperature, the gas molecules move faster, causing an increase in pressure (if volume is constant).
If you increase the volume (with constant temperature), pressure will decrease because gas molecules have more space to spread out.
When it's used:
The Ideal Gas Law is generally applicable in situations where:

The gas behaves ideally (low pressure, high temperature).
Intermolecular forces and the size of gas molecules are negligible.
For real gases, deviations from the Ideal Gas Law occur at high pressures and low temperatures, where gases condense or experience significant molecular forces.