Using Boyle's law why is a graph showing the relationship between pressure and volume not linear?

Answer 1

Well, what is #"Boyle's Law...?"#

#"Boyle's Law..."#, which is an EXPERIMENTAL gas LAW...holds that at constant temperature, and constant quantity of gas, #Pprop1/V#...where #prop# means #"proportional to...."#...

And so #P=k/V#...and #k=PV#...but this HOLDS for pressures and volumes given the STATED boundary conditions....

And thus the normal expression of #"Boyle's Law..."#, #P_1V_1=P_2V_2#....

And when we graph pressure against volume for a given quantity of gas at constant temperature....we gets...

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Answer 2

A graph showing the relationship between pressure and volume based on Boyle's law is not linear because Boyle's law states that at constant temperature, the pressure of a given amount of gas is inversely proportional to its volume. This means that as pressure increases, volume decreases, and vice versa. Therefore, when pressure and volume are plotted on a graph, they form a curve rather than a straight line. This is because the relationship between pressure and volume is not linear but rather exponential.

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Answer from HIX Tutor

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.

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