Difference between revisions of "Van der Waals equation"
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| − | The '''van der Waals equation'' is an [[equation of state]] in [[thermodynamics]] relating the [[physics | physical]] quantities [[pressure]], [[volume]], [[temperature]], and [[van der Waals force]]s in a [[gas]]. | + | The '''van der Waals equation''' is an [[equation of state]] in [[thermodynamics]] relating the [[physics | physical]] quantities [[pressure]], [[volume]], [[temperature]], and [[van der Waals force]]s in a [[gas]]. |
| − | == | + | ==Equation== |
| − | + | The law states: | |
| − | The | + | <cmath>\left(P-\alpha\frac{n^2}{V^2}\right)(V-\beta n)=nRT</cmath> |
| − | <cmath>(P-\alpha\frac{n^2}{V^2})(V-\beta n)=nRT</cmath> | + | where <math>\alpha</math> and <math>\beta</math> are dependent on the gas, <math>V</math> is the volume, <math>P</math> is the pressure, <math>n</math> is the number of [[mole]]s of gas, <math>R</math> is the [[universal gas constant]], <math>T</math> is the temperature. |
| − | where <math>\alpha</math> and <math>\beta</math> are dependent on the gas, <math>V</math> is the volume, <math>P</math> is the pressure, <math>n</math> is the number of | ||
The van der Waals equation is useful for high-pressure gases where the [[ideal gas law]] is inaccurate. | The van der Waals equation is useful for high-pressure gases where the [[ideal gas law]] is inaccurate. | ||
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{{stub}} | {{stub}} | ||
| + | [[Category:Physics]] | ||
Latest revision as of 10:44, 6 June 2008
The van der Waals equation is an equation of state in thermodynamics relating the physical quantities pressure, volume, temperature, and van der Waals forces in a gas.
Equation
The law states:
![\[\left(P-\alpha\frac{n^2}{V^2}\right)(V-\beta n)=nRT\]](http://latex.artofproblemsolving.com/f/2/d/f2decc732e59bb1aa2381b0a590bf6ee5290b227.png)
where 
and 
are dependent on the gas, 
is the volume, 
is the pressure, 
is the number of moles of gas, 
is the universal gas constant, 
is the temperature.
The van der Waals equation is useful for high-pressure gases where the ideal gas law is inaccurate.
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