The average kinetic energy of the particles would reduce, subsequently leading to reduced average motion of the particles. If the decrease in temperature persists, the particles eventually change phase and move to a less mobile state of matter than the phase in which they currently are in.
Explanation:
The image for the question is missing and we couldn't find thay online.
But it isn't hard to imagine what the image would be.
It is said to be a picture depicting particles that are in two different phases (liquid and gas).
What would likely happen if the temperature of the particles were decreased?
All particles of matter are said to always be in a constant state of motion (random motion); with the motion very evident in particles in gaseous phase than particles in liquid phase, then particles in the solid phase.
A decrease in temperature for any type of particles in whichever state will result in a reduced kinetic energy of such particles. As the kinetic energy with which the particles moving with constant, random motion is directly proportional to the absolute temperature of the system in which such particles are contained in.
So, a decrease in temperature for both gaseous and liquid particles will result in reduced and reduced kinetic energy and subsequently a reduction in the average motion of the particles.
For the gaseous particles, if the decrease in temperature continues to a point, the gaseous particles lose enough kinetic energy to change phase from gaseous form to a phase (liquid phase) where the motion is more restricted, average motion reduces and kinetic energy of the particles drop too. This is condensation; changing from gaseous phase to liquid phase.
The liquid particles follow a similar course too, only that a continuous decrease in temperature will lead to reduced motion and kinetic energy until the liquid particles 'freeze' by changing phase into the solid phase where the average motion is much more reduced and limited to vibrational motion about a particular fixed point.
Hope this Helps!!!
