From my rudimentary understanding of chemistry, pressure should be directly proportional to temperature for a constant mass of gas under the same volume (Charle'sCharles’s law).
However, in the diagram above, the vapour pressure seems to follow a non-linear relationship with the boiling point temperature of water.
Why is it the case that they are non-linear, and is there a mathematical relationship between the two quantities?
From my rudimentary understanding of chemistry, pressure should be directly proportional to temperature for a constant mass of gas under the same volume (Charle's law).
However, in the diagram above, the vapour pressure seems to follow a non-linear relationship with the boiling point temperature of water.
Why is it the case that they are non-linear, and is there a mathematical relationship between the two quantities?
From my rudimentary understanding of chemistry, pressure should be directly proportional to temperature for a constant mass of gas under the same volume (Charles’s law).
However, in the diagram above, the vapour pressure seems to follow a non-linear relationship with the boiling point temperature of water.
Why is it the case that they are non-linear, and is there a mathematical relationship between the two quantities?
From my rudimentary understanding of chemistry, pressure should be directly proportional to temperature for a constant mass of gas under the same volume (Charle's law).
However, in the diagram above, the vapour pressure seems to follow a non-linear relationship with the boiling point temperature of water.
Why is it the case that they are non-linear, and is there a mathematical relationship between the two quantities?
