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In a mixture of gases, each gas has a partial pressure which is the hypothetical pressure of that gas if it alone occupied the volume of the mixture at the same temperature. The total pressure of an ideal gas mixture is the sum of the partial pressures of each individual gas in the mixture.. It relies on the following isotherm relation: : : * ''Vx'' is the partial volume of any individual gas component (X) : * ''Vtot'' is the total volume in gas mixture : * ''px'' is the partial pressure of gas X : * ''ptot'' is the total pressure of gas mixture : * ''nx'' is the amount of substance of a gas (X) : * ''ntot'' is the total amount of substance in gas mixture The partial pressure of a gas is a measure of thermodynamic activity of the gas's molecules. Gases dissolve, diffuse, and react according to their partial pressures, and not according to their concentrations in gas mixtures or liquids. This general property of gases is also true in chemical reactions of gases in biology. For example, the necessary amount of oxygen for human respiration, and the amount that is toxic, is set by the partial pressure of oxygen alone. This is true across a very wide range of different concentrations of oxygen present in various inhaled breathing gases or dissolved in blood. ==Dalton's law of partial pressures== (詳細はDalton's Law of Partial Pressures )〕 This equality arises from the fact that in an ideal gas the molecules are so far apart that they don't interact with each other. Most actual real-world gases come very close to this ideal. For example, given an ideal gas mixture of nitrogen (N2), hydrogen (H2) and ammonia (NH3): : p__3} |align=left|= partial pressure of nitrogen (N2) |- !align=right| |align=left|= partial pressure of hydrogen (H2) |- !align=right| |align=left|= partial pressure of ammonia (NH3) |} 抄文引用元・出典: フリー百科事典『 ウィキペディア（Wikipedia）』 ■ウィキペディアで「Partial pressure」の詳細全文を読む スポンサード リンク
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