Question

Boyle law
critical pressure​

Answer 1

Explanation:

Q.1

Boyle’s law states the relation between volume and pressure at constant temperature and mass. Robert Boyle conducted an experiment on gases to study the deviation of its behaviour in changed physical conditions.

It states that under a constant temperature when the pressure on a gas increases its volume decreases. In other words according to Boyle’s law volume is inversely proportional to pressure when the temperature and the number of molecules are constant.

$p  ∝ 1/V$

$p = k /V$

k here is a proportionality constant, V is the Volume and p is the pressure. On rearranging, we get: k= pV. Now, if a fixed mass of gas undergoes an expansion at constant temperature then the final volume and pressure shall be p2 and V2. The initial volume and initial pressure here is p1 and V1 then according to Boyle’s law: p1×V1 = p2×V2 = constant (k)

$p1/p2  =  V2/V1$

So according to Boyle’s law, if the pressure is doubled then at constant temperature the volume of that gas is reduced to half.

Q.2

Definition 1

The critical pressure of a substance is the pressure corresponding to the critical point (or the critical state) of the substance. The critical point of a substance can be defined as the point on the temperature and pressure scale in which a liquid substance can coexist with its vapour.

Definition 2

The critical pressure is the vapor pressure of a fluid at the critical temperature above which distinct liquid and gas phases do not exist. ... The point at which the critical temperature and critical pressure is met is called the critical point.

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