Partial pressure

The pressure partial of a Perfect gas I in a mixture of perfect gases of total pressure $p\_\; \{early\}\; ~$ is defined as the Pression $p\_\; \{I\}\; ~$ which would be exerted by the molecules of the gas I if this gas occupied only all the volume offered to the mixture, at the temperature of this one. In the particular case of the Steam (here comparable with a perfect gas), one would speak rather about Steam pressure.

The Loi of Dalton, rigorously valid for an ideal mixture of perfect gases connects the pressure partial $p\_\; \{I\}\; ~$ and the total pressure $p\_\; \{early\}\; ~$ via the molar Fraction $x\_\; \{I\}\; ~$ of the component considered in the mixture:

$x\_\; \{I\}\; =\; \backslash \; frac\; \{n\_\; \{I\}\}\; \{n\_\; \{early\}\}$

where $n\_\; \{I\}\; ~$ is the number of mole S of an unspecified component located by the index $I\; ~$ in the mixture and $n\_\; \{early\}\; ~$ the full number of moles in the mixture.

the pressure partial of the component I is equal to the product of its molar fraction by the total pressure.

$p\_\; \{I\}\; =\; x\_\; \{I\}.\; p\_\; \{early\}\; ~$

The pressure of an ideal mixture of perfect Gaz is the nap pressures partial of each one of its components.

$\backslash \; sum\; p\_\; \{I\}\; =\; (\backslash \; sum\; x\_\; \{I\}).\; p\_\; \{early\}\; =\; p\_\; \{early\}\; ~$ because $\backslash \; sum\; x\_\; \{I\}\; =\; 1~$.

External bonds

• Conversion of units of pressure

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