11th Class Chemistry Chapter 3(Gases Preparation) Online Short Questions with Answers Preparation

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ilmkidunya presents the updated and most important short questions of Chemistry Chapter 3 “Gases”. In the modern era students are getting smarter and they believe in smart work rather than hard work.

In the Chapter 3 Gases students will get to know the following important points:

States of Matter

Gases law

Gas equation

Avogadro's law

Delton law

Kinetic theory

State of plasma and much more topics related to the Chapter 3 Chemistry Gases

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Online Short Questions For Chapter 3 "11th Class Chemistry Short Questions Chapter 3 Preparation "

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Chemistry - 11th Class Chemistry Short Questions Chapter 3 Preparation

Question # 1

Justify that the volume of given mass of a gas becomes theoretically zero at -273^°C.

Ans 1:

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Prepare Complete Set Wise Questions For Chapter 3 "11th Class Chemistry Short Questions Chapter 3 Preparation "

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11th Class Chemistry Short Questions Chapter 3 Preparation - Set 1

Question # 1

Justify that the volume of given mass of a gas becomes theoretically zero at -273^°C.

Ans 1:

Submit

11th Class Chemistry Short Questions Chapter 3 Preparation - Set 2

Question # 1

Why the gases deviate from ideal behavior at high pressure and low temperature?

Ans 1: When the temperature of the gases are low, the attractive forces become dominant, so gases don't obey the gas laws. When the pressure of the gases are high, collisions become more frequent and force of attraction are created. Moreover, the actual volume of the gas molecules are no more negligible as compared to the volume of the vessel.

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11th Class Chemistry Chapter 3 Preparation

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First Year Chemistry Chapter 3 Online Short Questions Preparation for 1st Year Chemistry Chapter 3 Gases Preparation

States of Matter

Gases law

Gas equation

Avogadro's law

Delton law

Kinetic theory

State of plasma and much more topics related to the Chapter 3 Chemistry Gases

FSC Part 1 Subjects

Online Short Questions For Chapter 3 "11th Class Chemistry Short Questions Chapter 3 Preparation "

Chemistry - 11th Class Chemistry Short Questions Chapter 3 Preparation

Justify that the volume of given mass of a gas becomes theoretically zero at -273°C.

Why is the Boyle's law applicable only to the ideal gases?

What is absolute zero? What happens to real gases while approaching it?

Justify that 1 cm3 of H2 1 cm3 of CH4 at STP will have same number of molecules. When one molecule of CH4 is 8 times heavier that of hydrogen.

Lighter gases diffuse more rapidly than heavier gases. Give reason.

The amount of pressure which is decreased due to the forces of attraction is given by a/V2 where 'a' is the van der Waal's constant and V is the volume of the vessel.

Calculate the S.I unit of R.

Why the non-polar gases like H2 and He have a very low critical temperatures while polar gases like NH3 and SO4 have critical temperatures, sufficiently above room temperature?

What are isotherms? What happens to the positions of isotherms when they are plotted at high temperature for a particular gas?

Dalton's law of partial pressures is only applicable to those mixtures of gases which are Ideal and they do not react with each other under the given conditions. Why?

Prepare Complete Set Wise Questions For Chapter 3 "11th Class Chemistry Short Questions Chapter 3 Preparation "

Set 1

Set 2

11th Class Chemistry Short Questions Chapter 3 Preparation - Set 1

Justify that the volume of given mass of a gas becomes theoretically zero at -273°C.

Why is the Boyle's law applicable only to the ideal gases?

What is absolute zero? What happens to real gases while approaching it?

Justify that 1 cm3 of H2 1 cm3 of CH4 at STP will have same number of molecules. When one molecule of CH4 is 8 times heavier that of hydrogen.

Lighter gases diffuse more rapidly than heavier gases. Give reason.

The amount of pressure which is decreased due to the forces of attraction is given by a/V2 where 'a' is the van der Waal's constant and V is the volume of the vessel.

Calculate the S.I unit of R.

Why the non-polar gases like H2 and He have a very low critical temperatures while polar gases like NH3 and SO4 have critical temperatures, sufficiently above room temperature?

What are isotherms? What happens to the positions of isotherms when they are plotted at high temperature for a particular gas?

Dalton's law of partial pressures is only applicable to those mixtures of gases which are Ideal and they do not react with each other under the given conditions. Why?

11th Class Chemistry Short Questions Chapter 3 Preparation - Set 2

Why the gases deviate from ideal behavior at high pressure and low temperature?

Why do we get a straight line when pressures are plotted against inverse of volumes? This straight line changes its positions in the graph by varying the temperature. Justify it.

Why is the Boyle's law applicable only to the ideal gases?

How the behavior of real gases is given by van der waal's equation?

What is absolute zero? What happens to real gases while approaching it?

What are various scales of thermometry?

Charles's law is not obeyed when the temperature is measured on Celsius scale. Justify it.

In Joule-Thomson effect sudden expansion of the gas molecules needs energy. Why?

The amount of pressure which is decreased due to the forces of attraction is given by a/V2 where 'a' is the van der Waal's constant and V is the volume of the vessel.

Gases deviate more from the general gas equation at 0° C and deviate to less extent at 100° C. why?

11th Class Chemistry Chapter 3 Preparation

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Justify that the volume of given mass of a gas becomes theoretically zero at -273^°C.

Justify that 1 cm³ of H₂ 1 cm³ of CH₄ at STP will have same number of molecules. When one molecule of CH₄ is 8 times heavier that of hydrogen.

The amount of pressure which is decreased due to the forces of attraction is given by a/V₂ where 'a' is the van der Waal's constant and V is the volume of the vessel.

Why the non-polar gases like H₂ and He have a very low critical temperatures while polar gases like NH₃ and SO₄ have critical temperatures, sufficiently above room temperature?

Justify that the volume of given mass of a gas becomes theoretically zero at -273^°C.

Justify that 1 cm³ of H₂ 1 cm³ of CH₄ at STP will have same number of molecules. When one molecule of CH₄ is 8 times heavier that of hydrogen.

The amount of pressure which is decreased due to the forces of attraction is given by a/V₂ where 'a' is the van der Waal's constant and V is the volume of the vessel.

Why the non-polar gases like H₂ and He have a very low critical temperatures while polar gases like NH₃ and SO₄ have critical temperatures, sufficiently above room temperature?

The amount of pressure which is decreased due to the forces of attraction is given by a/V₂ where 'a' is the van der Waal's constant and V is the volume of the vessel.