[Solved] Critical temperature for carbon dioxide and methane are 31.1∘C and −81.9∘C respectively. Which of these has stronger intermolecular forces and why? - Chemistry Part-I

Name: Video solution 2: [Solved] Critical temperature for carbon dioxide and methane are 31.1∘C and −81.9∘C respectively. Which of these has stronger intermolecular forces and why? - Chemistry Part-I
Uploaded: 2022-05-21T10:57:20.000Z
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Description: Video solution 2: [Solved] Critical temperature for carbon dioxide and methane are 31.1∘C and −81.9∘C respectively. Which of these has stronger intermolecular forces and why? - Chemistry Part-I

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Chemistry Part-I

States of Matter

Critical temperature for carbon dioxide and methane are 31.1^{

Chemistry Part-I

Class 11

NCERT

Chapter 1: Some Basic Concepts of Chemistry

44 questions

Chapter 2: Structure of Atom

85 questions

Chapter 3: Classification of Elements and Periodicity in Properties

50 questions

Chapter 4: Chemical Bonding and Molecular Structure

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Chapter 5: States of Matter

28 questions

In terms of Charles' law, explain why - 273

^{\circ} C

is the lowest possible temperature.

Critical temperature for carbon dioxide and methane are

31. 1^{\circ} C

and

- 81. 9^{\circ} C

respectively. Which of these has stronger intermolecular forces and why?

Explain the physical significance of Van der Waals parameters.

View all question

Chapter 6: Thermodynamics and Thermochemistry

36 questions

Chapter 7: Equilibrium

101 questions

Question

Easy

Solving time: 2 mins

Critical temperature for carbon dioxide and methane are $31. 1^{\circ} C$ and $- 81. 9^{\circ} C$ respectively. Which of these has stronger intermolecular forces and why?

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Updated on: May 21, 2022

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Chemistry Part-I (NCERT)

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Critical temperature for carbon dioxide and methane are

31. 1^{\circ} C

and

- 81. 9^{\circ} C

respectively. Which of these has stronger intermolecular forces and why?

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Text solutionVerified

Higher is the critical temperature, more easily the gas can be liquefied and greater are the intermolecular forces of attraction. Hence,

C O_{2}

has stronger intermolecular forces than

H_{2} O

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Practice more questions from Chemistry Part-I (NCERT)

In terms of Charles' law, explain why - 273

^{\circ} C

is the lowest possible temperature.

Critical temperature for carbon dioxide and methane are

31. 1^{\circ} C

and

- 81. 9^{\circ} C

respectively. Which of these has stronger intermolecular forces and why?

Explain the physical significance of Van der Waals parameters.

View all

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Question Text	Critical temperature for carbon dioxide and methane are $31. 1^{\circ} C$ and $- 81. 9^{\circ} C$ respectively. Which of these has stronger intermolecular forces and why?
Updated On	May 21, 2022
Topic	States of Matter
Subject	Chemistry
Class	Class 11
Answer Type	Text solution:1 Video solution: 2
Upvotes	337
Avg. Video Duration	3 min

Critical temperature for carbon dioxide and methane are $31. 1^{\circ} C$ and $- 81. 9^{\circ} C$ respectively. Which of these has stronger intermolecular forces and why?

Text solutionVerified

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Critical temperature for carbon dioxide and methane are 31.1∘C and −81.9∘C respectively. Which of these has stronger intermolecular forces and why?

Text solutionVerified

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Critical temperature for carbon dioxide and methane are $31. 1^{\circ} C$ and $- 81. 9^{\circ} C$ respectively. Which of these has stronger intermolecular forces and why?