Dalton's Law of Partial Pressures
The partial pressure of an ideal gas in a mixture is equal to the pressure it would exert if it occupied the same volume alone at the same temperature. This is because ideal gas molecules are so far apart that they don't interfere with each other at all. Actual real-world gases come very close to this ideal.
A consequence of this is that the total pressure of a mixture of ideal gases is equal to the sum of the partial pressures of the individual gases in the mixture as stated by Dalton's law. For example, given an ideal gas mixture of nitrogen (N2), hydrogen (H2) and ammonia (NH3):
| where: | |
| = total pressure of the gas mixture | |
| = partial pressure of nitrogen (N2) | |
| = partial pressure of hydrogen (H2) | |
| = partial pressure of ammonia (NH3) |
Read more about this topic: Partial Pressure
Famous quotes containing the words law, partial and/or pressures:
“And what other great nation has statutes and ordinances as just as this entire law that I am setting before you today? But take care and watch yourselves closely, so as neither to forget the things that your eyes have seen nor to let them slip from your mind all the days of your life; make them known to your children and your children’s children...”
—Bible: Hebrew, Deuteronomy 4:8,9.
“And meanwhile we have gone on living,
Living and partly living,
Picking together the pieces,
Gathering faggots at nightfall,
Building a partial shelter,
For sleeping and eating and drinking and laughter.”
—T.S. (Thomas Stearns)
“Today’s pressures on middle-class children to grow up fast begin in early childhood. Chief among them is the pressure for early intellectual attainment, deriving from a changed perception of precocity. Several decades ago precocity was looked upon with great suspicion. The child prodigy, it was thought, turned out to be a neurotic adult; thus the phrase “early ripe, early rot!””
—David Elkind (20th century)