Which of the assumption of the kinetic - molecular theory best explains Daltons law of partial pressure?
Which of the assumption of the kinetic - molecular theory best explains Daltons law of partial pressure?
The correct option is A Gas molecules move at random with no attractive forces between them.
Gas molecules move at random with no attractive forces between them implies that there are no van der Waals forces between gas molecules. If a mixture of non-interacting gases is in a container, the total pressure shall be equated to the sum of the partial pressures of the mixing gases.
The velocity of gas molecules is proportional to their Kelvin temperature but does not explain Dalton's law of partial pressure.
The amount of space occupied by a gas is much greater than the space occupied by the actual gas molecules, does not explain Dalton's law of partial pressure.
Collisions with the walls of the container or with other molecules are elastic as this explains how gas molecules are always moving without ever coming to rest.
Gas molecules move at random with no attractive forces between them.
Gas molecules move at random with no attractive forces between them implies that there are no van der Waals forces between gas molecules. If a mixture of non-interacting gases is in a container, the total pressure shall be equated to the sum of the partial pressures of the mixing gases.
The velocity of gas molecules is proportional to their Kelvin temperature but does not explain Dalton's law of partial pressure.
The amount of space occupied by a gas is much greater than the space occupied by the actual gas molecules, does not explain Dalton's law of partial pressure.
Collisions with the walls of the container or with other molecules are elastic as this explains how gas molecules are always moving without ever coming to rest.
