Ch 3 Chemistry Class 11 Notes

• Here are the detailed ch 3 class 11 chemistry notes to help you prepare for your exams.
• Name the states of matter. Which state is the simplest one?
• What are the Properties of Gases? Gases don’t have a definite volume and occupy all the available space. The volume of a gas is the volume of the container. 2. They don’t have a definite shape and take the shape of the container just like liquids. 3. Due to low densities of gases, as compared to those of liquids and solids, the gases bubble through liquids and tend to rise up.
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• Gases can diffuse and effuse. This property is negligible in solids but operates in liquids as well. 5. Gases can be compressed by applying a pressure because there are large empty spaces between their molecules. 6. Gases can expand on heating or by increasing the available volume. Liquids and solids, on the other hand, do not show an appreciable increase in volume when they are heated. 7. When sudden expansion of gases occurs cooling takes place. It is called Joule-Thomson effect.
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• What are the Properties of Liquids? 1. Liquids don’t have a definite shape but have a definite volume. Unlike solids they adopt the shape of the container. 2. Molecules of liquids are in a constant state of motion. The evaporation and diffusion of liquid molecules is due to this motion. 3. The densities of liquids are much greater than those of gases but are close to those of solids.
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• The spaces among the molecules of liquids are negligible just like solids. 5. The intermolecular attractive forces in liquids are intermediate between gases and solids. The melting and boiling points of gases, liquids and solids depend upon the strength of such forces. 
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• What are the properties of solids?
• Give quantitative definition of Charles’s law. Throw some light on the factor 1/273 in Charles’s law. 
• Why Kelvin scale of temperature justifies Charles’s law?
• Tell about Celsius scale of temperature. 
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• Tell about Fahrenheit scale of temperature.
• Tell about absolute or Kelvin scale of temperature. 
• Calculate the value of ideal gas constant according to STP.
• Calculate the value of gas constant in SI units. 
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• How Dalton’s law of partial pressures is applicable to the collection of gases under water?
• How Dalton’s law of partial pressure finds application in breathing process?
• Why pilots feel uncomfortable breathing at high altitudes? 
• Why deep sea divers take oxygen mixed with an inert gas?
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• Mention main postulates of kinetic molecular theory.
• Prove Charles’s law according to KMT/Prove Boyle’s law according to KMT/Prove Avogadro’s law according to KMT/Prove Graham’s law according to KMT. (Any one can be asked)
• Differentiate between natural and artificial plasma. 
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• What are the characteristics of plasma? 
• What are the applications of plasma? (Mention any four applications as an answer to short question)
• Why is the Boyle’s law applicable only to the ideal gases?
• When a gas obeys the Boyle’s law, the isotherms for the gas can be plotted. How is it true?
• What are isotherms? What happens to the positions of isotherms when they are plotted at high temperature for a particular gas?
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• The plot of PV versus P is a straight line. Justify.
• Greater the temperature closer the straight line of P versus 1/V to the pressure axis, Justify. 
• The plot of PV vs P is a straight line at constant temperature and with a fixed number of moles of an ideal gas. Justify. 
• Why lighter gases diffuse more rapidly than heavier gases?
• Some of the postulates of Kinetic Molecular Theory are faulty. Justify OR Write down two faulty assumptions of KMT of gases. 
• Rate of diffusion of ammonia is more than that of HCl. Why?
• Pressure of ammonia gas at given conditions is less as calculated by Vander Waal equation than that calculated by general gas equation. Why?
• Dalton’s law of partial pressures is only obeyed by those gases which don’t have attractive forces among their molecules. Explain it. 
• Under which conditions gases behave ideally?