Ideal gas law pressure is the pressure of an ideal gas, which is directly proportional to the number of moles of the gas, the temperature, and inversely proportional to the volume of the container it's in.
Key Points about Ideal Gas Law Pressure
- The gas particles do not interact with each other except through perfectly elastic collisions.
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The gas particles are considered point masses with no volume of their own.
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The average kinetic energy of gas particles is directly proportional to the absolute temperature.
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This law holds under conditions where real gases behave most like an ideal gas, typically at high temperatures and low pressures where molecular interactions are minimal.
Ideal Gas Law Pressure Formula |
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\( p \;=\; \dfrac{ n \cdot R \cdot T }{ V }\) (Ideal Gas Law Pressure) \( n \;=\; \dfrac{ p \cdot V }{ R \cdot T }\) \( R \;=\; \dfrac{ p \cdot V }{ n \cdot T }\) \( T \;=\; \dfrac{ p \cdot V }{ n \cdot R }\) \( V \;=\; \dfrac{ n \cdot R \cdot T }{ p }\) |
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| Symbol | English | Metric |
| \( p \) = pressure of gas | \(lbf\;/\;in^2\) | \(Pa\) |
| \( n \) = number of moles of gas | \(dimensionless\) | \(dimensionless\) |
| \( R \) = specific gas constant (gas constant) | \(ft-lbf\;/\;lbm-R\) | \(J\;/\;kg-K\) |
| \( T \) = temperature | \( R \) | \( K \) |
| \( V \) = volume | \( in^3 \) | \( mm^3 \) |
