entropy increase as temperature increases why
Because the molecules are more randomly positioned.
Why don’t dipole-dipole forces have much affect on a gas?
The molecules are relatively far apart. In a liquid or a solid the molecules are much closer together. The molecules in a gas are much further apart UNLESS we are talking about LOW LOW temperatures OR HIGH HIGH pressure.
The relationship between temperature and entropy can be explained by the concept of microstates and macrostates in statistical mechanics. Entropy is a measure of the number of possible microstates of a system, which corresponds to the "disorder" or "randomness" of the system. Temperature, on the other hand, is a measure of the average kinetic energy of particles in the system.
As the temperature of a system increases, the average kinetic energy of its particles also increases. This leads to an increase in the number of accessible energy states or microstates that the system can occupy. Since entropy is a measure of the number of microstates, it follows that an increase in temperature leads to an increase in entropy.
To better understand this relationship, consider a simple example of a gas in a container. At a low temperature, the gas particles have low kinetic energy, and they are mostly confined to a small region of the container. This results in a relatively small number of possible microstates and therefore low entropy.
As the temperature increases, the gas particles gain more kinetic energy and move around with greater speed. This leads to an increased number of possible arrangements of the particles within the container, resulting in a larger number of microstates and hence higher entropy.
Therefore, the increase in temperature causes an increase in the energy distribution and randomness of particle positions, leading to a higher number of available microstates and hence a higher entropy.