Question

Volume is inversely to pressure is:
A.Boyle’s law
B.Charles’s law
C.Avogadro’s principle
D.Ideal gas law

Answer 1

To solve this problem one should know about the Gas Laws based on the Kinetic Molecular Theory of Gases. Various gas laws are explained based on the Kinetic Molecular Theory of Gases. We need to find the law which shows the inverse proportion of volume with pressure.

Complete step by step answer:
Gas laws (Boyle’s law, Charles law, Avogadro’s principle, Dalton’s law of partial pressure) were based only on the practical observations. To explain these experimental facts, theoretically, a model was designed, according to which all gases are composed of molecules and these molecules are always in motion.
Various gas laws can be explained based on the Kinetic Molecular Theory of Gases. But to find the solution to the problem that volume is inversely proportional to pressure is given by which law. So we will consider all options one by one.
Option (A) Boyle’s law. It states that “At constant temperature, the volume of a given mass of gas is inversely proportional to its pressure.” The expression of Boyle’s law is given by
$V\alpha \dfrac{1}{P}$ Removing the proportionality constant we get,
$\Rightarrow PV = k$
Where $P$ is the pressure of the gas and,
$V$ is the Volume of the gas,
$k$ is the proportionality constant.
So we can conclude from Boyle’s law that volume is inversely proportional to pressure. At constant temperature, an increase in volume will lead to a decrease in pressure.
In Charles, law volume is directly proportional to a temperature, not pressure. So option (B) is wrong.
Option (C) Avogadro’s law. It states that an equal volume of gases has an equal number of moles at constant temperature and pressure.
Ideal gas law is also called the Ideal Gas equation. Considering the assumptions it can be expressed as $PV = nRT$ where $R$ is the universal gas constant and $P,V,T$ are pressure, volume and temperature respectively.

Therefore, the correct option is (A).

Note:
The kinetic molecular theory of gases explains the gaseous behavior based on experimental observation.There are certain assumptions of the kinetic theory of gases. All these assumptions are related to molecules, but molecules cannot be seen. Therefore, this model is also called the microscopic model.