Important Questions for JEE Advanced
FAQs on JEE Advanced Gaseous and Liquid States Important Questions
1. How important is the gaseous and liquid state chapter for the JEE advanced exam?
This chapter is an integral part of the portion, as it contains some fundamental concepts that are essential for students to understand solving some complex problems. This chapter consists of multiple concepts such as properties of gases, mass, volume, pressure, boiling point, melting point, surface tension as well as some really significant gas laws which should not be neglected by students as they are not only building bridges but the concerns are formula based which ultimately makes them easy to solve. This chapter provides an insight into gases and liquids which are really indispensable concepts in terms of physical chemistry.
2. What are some properties of gases as discussed in the chapter Gaseous and Liquid States?
Gases are a phase of matter in which particles are far apart from one another, move in random directions, and aren't attracted to one another. Properties of gases are listed below:
gases do not have a definite shape and volume.
gases can occupy the whole space that is accessible to them.
They have high compressibility.
gases have unlimited indispensability.
gases exert pressure on the wall of whatever object they are in.
due to negligible intermolecular forces gases have very low densities.
3. What are the main gas laws that students shouldn't miss while studying the chapter Gaseous and Liquid States for JEE Advanced?
A few important gas laws that students should study are mentioned below:
1. Boyle’s law: Boyle’s law states that at constant temperature the volume of a given mass of awful gas is inversely proportional to the pressure. Boyle's law is also termed Mariotte’s Law. Boyle's law was coined by physicist Robert Boyle in 1662. It can also be derived from the kinetic theory of gas assuming ideal gas.
2. Charle’s Law: Charle’s law States that at constant pressure, the volume of a given mass of a gas is directly proportional to its absolute temperature. It is formulated by physicist J.A.C Charle’s in 1787.
4. What is Graham’s Law of Diffusion/Effusion as discussed in the chapter Gaseous and Liquid States?
Comes important concepts we need to understand Graham’s laws are diffusion and effusion. Diffusion is the ability of a gas to mix spontaneously and form a homogeneous mixture, while effusion is the process in which a gas is allowed to escape under pressure through a fine orifice from a closed container.
This law was proposed by Thomas Graham, and it states that at constant temperature and pressure the rate of diffusion or a fusion of a gas is inversely proportional to the square root of its density and directly proportional to its pressure.
Some applications of Graham’s Law of diffusion are:
- They help determine the molecule's mass of gases.
- They help calculate the density of gases.
- Separation of Isotopes.
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5. What are some assumptions of the kinetic theory of gas as discussed in the chapter Gaseous and Liquid States?
The kinetic theory of gas was originally suggested by Bernoulli, After which a few physicists further defined it. Some assumptions of the kinetic theory are listed below:
Gases are made up of molecules moving randomly in all directions.
Gas molecules cannot attract or repel each other.
All the gas molecules adhere to Newton's law of motion.
Collisions between two molecules or between a molecule and a wall are elastic.
An individual molecule has negligible volume as compared to the total volume of the gas.
Kinetic energy of a gas molecule depends upon the absolute temperature.
Force of gravity has no effect whatsoever on the speed of gas molecules.