Skip to main content
Chemistry

Return to Question

doubts to questions
Source Link
edit approved Apr 23, 2019 at 15:36
Apoorv Potnis
edit approved Apr 23, 2019 at 15:36
Apoorv Potnis
  • 1.3k
  • 1
  • 16
  • 38

A gas described by van der Waals equation has the pressure that is lower than the pressure exerted by the same gas behaving ideally. True or false?

My approach

$$P(\text{ideal}) = P(\text{real}) + P(\text{changes due to intermolecular forces})$$

So the pressure of real gas can be more as well as less than that if a gas behaving ideally depending on whether intermolecular forces are repulsive or attractive in nature.

DoubtsQuestions

  1. The answer to the question is given as True. So I want to understand what is wrong about my approach.

  2. Since the intermolecular forces depend on $a$, for attractive nature $a$ is positive. Is $a$ negative for repulsive nature of forces?

A gas described by van der Waals equation has the pressure that is lower than the pressure exerted by the same gas behaving ideally. True or false?

My approach

$$P(\text{ideal}) = P(\text{real}) + P(\text{changes due to intermolecular forces})$$

So the pressure of real gas can be more as well as less than that if a gas behaving ideally depending on whether intermolecular forces are repulsive or attractive in nature.

Doubts

  1. The answer to the question is given as True. So I want to understand what is wrong about my approach.

  2. Since the intermolecular forces depend on $a$, for attractive nature $a$ is positive. Is $a$ negative for repulsive nature of forces?

A gas described by van der Waals equation has the pressure that is lower than the pressure exerted by the same gas behaving ideally. True or false?

My approach

$$P(\text{ideal}) = P(\text{real}) + P(\text{changes due to intermolecular forces})$$

So the pressure of real gas can be more as well as less than that if a gas behaving ideally depending on whether intermolecular forces are repulsive or attractive in nature.

Questions

  1. The answer to the question is given as True. So I want to understand what is wrong about my approach.

  2. Since the intermolecular forces depend on $a$, for attractive nature $a$ is positive. Is $a$ negative for repulsive nature of forces?

Tweeted twitter.com/StackChemistry/status/1120477656531841025
Became Hot Network Question
added 14 characters in body; edited tags; edited title
Source Link
andselisk ♦
andselisk ♦
  • 38.5k
  • 14
  • 133
  • 223

Can the van der Walls'Waals coefficients be negative in the van der Walls'Waals equation for real gases?

This was the question asked-

True/False- A gas described by van der Walls' equation has the pressure that is lower than the pressure exerted by the same gas behaving ideally.

A gas described by van der Waals equation has the pressure that is lower than the pressure exerted by the same gas behaving ideally. True or false?

My approach-

My approach

P(ideal) = P(real) + P(changes due to intermolecular forces)$$P(\text{ideal}) = P(\text{real}) + P(\text{changes due to intermolecular forces})$$

So the pressure of real gas can be more as well as less than that if a gas behaving ideally depending on whether intermolecular forces are repulsive or attractive in nature.

Doubts- 1. The answer to the question is given as True. So I want to understand what is wrong about my approach.

Doubts

  1. Since the intermolecular forces depend on 'a', for attractive nature 'a' is positive. Is 'a' negative for repulsive nature of forces?

  1. The answer to the question is given as True. So I want to understand what is wrong about my approach.

  2. Since the intermolecular forces depend on $a$, for attractive nature $a$ is positive. Is $a$ negative for repulsive nature of forces?

Can the van der Walls' coefficients be negative in the van der Walls' equation for real gases?

This was the question asked-

True/False- A gas described by van der Walls' equation has the pressure that is lower than the pressure exerted by the same gas behaving ideally.

My approach-

P(ideal) = P(real) + P(changes due to intermolecular forces)

So the pressure of real gas can be more as well as less than that if a gas behaving ideally depending on whether intermolecular forces are repulsive or attractive in nature.

Doubts- 1. The answer to the question is given as True. So I want to understand what is wrong about my approach.

  1. Since the intermolecular forces depend on 'a', for attractive nature 'a' is positive. Is 'a' negative for repulsive nature of forces?

Can the van der Waals coefficients be negative in the van der Waals equation for real gases?

A gas described by van der Waals equation has the pressure that is lower than the pressure exerted by the same gas behaving ideally. True or false?

My approach

$$P(\text{ideal}) = P(\text{real}) + P(\text{changes due to intermolecular forces})$$

So the pressure of real gas can be more as well as less than that if a gas behaving ideally depending on whether intermolecular forces are repulsive or attractive in nature.

Doubts

  1. The answer to the question is given as True. So I want to understand what is wrong about my approach.

  2. Since the intermolecular forces depend on $a$, for attractive nature $a$ is positive. Is $a$ negative for repulsive nature of forces?

Source Link
Groverkss
Groverkss
  • 367
  • 4
  • 14

Can the van der Walls' coefficients be negative in the van der Walls' equation for real gases?

This was the question asked-

True/False- A gas described by van der Walls' equation has the pressure that is lower than the pressure exerted by the same gas behaving ideally.

My approach-

P(ideal) = P(real) + P(changes due to intermolecular forces)

So the pressure of real gas can be more as well as less than that if a gas behaving ideally depending on whether intermolecular forces are repulsive or attractive in nature.

Doubts- 1. The answer to the question is given as True. So I want to understand what is wrong about my approach.

  1. Since the intermolecular forces depend on 'a', for attractive nature 'a' is positive. Is 'a' negative for repulsive nature of forces?