Why are polar gases, such as H2O and NH3, more likely to deviate from the ideal gas behaviors described by the kinetic molecular theory? (3 points) Question 4 options:

1)

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

2)

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

3)

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

4)

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

HCl, H2O, and NH3 are the most polar of these, so they won't behave ideally because the particles have greater attractive forces between them. How does the kinetic-molecular theory explain the pressure exerted by gases? ... Particles are always in motion and when they are contained, they are elastic collisions.

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

Explanation:

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