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×31st Oct 2019 @ 2 min read

The graph of Boyle's law is known as pressure-volume graph or *PV* curve. It is as follows:

As observed from the graph above, pressure increases with a decrease in volume, and vice versa. Thus, pressure is inversely proportional to volume. Other parameters (temperature and amount of gas) are constant in the graph above.

Volume is on the *x*-axis and pressure, on the *y*-axis. The equation of the curve is *PV* = *k*, which is the equation of Boyle's law. The curve is hyperbolic in nature having two asymptotes: *P* = 0 (horizontal) and *V* = 0 (vertical).

Note: An asymptote is a line or curve such that the distance between it and a given curve tends to zero as *x* and/or *y* coordinates tends to infinity.

As volume tends to positive infinity, pressure tends to zero, and we get the horizontal asymptote, *P* = 0.

When volume approaches zero, pressure approaches infinity, and it results in the vertical asymptote, *V* = 0.

Graphs of Boyle's law can be plotted at different temperatures. Each curve in the graphs below is at a constant temperature and such curves are called isotherms.

The above graph is a pressure-volume graph plotted at three different temperatures (*T*_{1}, *T*_{2}, and *T*_{3}). As observed from the graph, with an increase in temperature, curves shift upwards. This is because of increase in the value of *k*.

The graph of pressure vs inverse volume is a straight line passing through the origin and having the positive slope, *k*.

The graph above is a straight line parallel to the *x*-axis. This proves the product of pressure and volume at a constant temperature and amount of gas is constant. The lines in the graph are independent of volume (or pressure).

The equation of Boyle's law is *PV* = *k*. Taking the logarithm to both sides.

The plots are a straight line with the *y*-intercept of log *k*.

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Thanks for your response!

John Dalton

28th Jan 2022

28th Jan 2022

Awesome!

Robert Boyle

20th Jan 2022

20th Jan 2022

man what u guys are doing is phenomenal .

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