Question

Under what conditions will a gas be most likely to exhibit the ideal gas properties predicted by the ideal gas law?

- High pressures and high temperature, because particles are forced closer together with higher kinetic energy, so intermolecular forces of attraction are weaker
- High pressure and low temperature, because particles are forced closer together and moving slower, so the volume of the particles is less significant
- Low pressure and high temperature, because particles are spread farther apart and moving faster, so the intermolecular forces of attraction are weaker
- Low pressure and low temperature, because particles are spread farther apart with lower kinetic energy, so the volume of the particles is less significant

Answer 1

A gas at very low volumes, when gas particles are very close together

A gas at very low temperatures, when gas particles have very little kinetic energy

A gas with highly polar molecules that have very strong inter-molecular forces

Step-by-step explanation:

According to kinetic molecular theory:

a) Ideal gases have large number of particles which were considered to be hard spherical objects.

b) these gas particles move randomly in a straight line.

c) the path of gas particles change when they collide with each other or walls of vessel.

d) there is no or negligible inter molecular interactions between the gas particles.

e) the inter molecular distances is much higher than the size of particles.

f) the gas particles occupy negligible volume of the vessel.

g) during collision of gas particles is perfectly elastic.

h) the average kinetic energy of particles is constant at a constant temperature. It varies directly with the temperature.

Answer 2

High pressure and low temperature, because particles are forced closer together and moving slower, so the volume of the particles is less significant