Why are polar gases, such as H2O and NH3, more likely to deviate from the ideal gas behaviors described by the kinetic molecular theory?

A. The density of these gases is high, increasing the number of collisions and reducing their elasticity.

B. The fluidity of these gases is high, resulting in a higher average kinetic energy.

C. The particles have a significant volume, reducing the space between the moving particles.

D. The particles have high intermolecular forces, reducing the elasticity of their collisions.

Question

Ciara Montgomery

Chemistry

22 March, 20:04

Why are polar gases, such as H2O and NH3, more likely to deviate from the ideal gas behaviors described by the kinetic molecular theory?

A. The density of these gases is high, increasing the number of collisions and reducing their elasticity.

B. The fluidity of these gases is high, resulting in a higher average kinetic energy.

C. The particles have a significant volume, reducing the space between the moving particles.

D. The particles have high intermolecular forces, reducing the elasticity of their collisions.

+3

Answers (2)

Know the Answer?

Tucker Newton · Answer 1

The answer is:

D. The particles have high intermolecular forces, reducing the elasticity of their collisions.

Jose Mckee · Answer 2

The answer is: D. The particles have high intermolecular forces, reducing the elasticity of their collisions.

Hydrogen bonds are formed between water molecules (H2O) and ammonia molecules (NH3).

Hydrogen bond is an electrostatic attraction between two polar groups that occurs when a hydrogen atom (H), covalently bound to a highly electronegative atom such as flourine (F), oxygen (O) and nitrogen (N) atoms.

In ideal gas, all collisions are perfectly elastic, there is no loss of kinetic energy during the collision.