In the previous article, we discussed Microstates and how they are differentiated by the storage of quanta in two solids. In this article, we are going to be discussing how Entropy fits into this relationship.

Entropy is the direct measure of the probability of each configuration of quanta. Scientists have observed is that a situation where quanta are the most spread out is also the situation that holds the largest amount of Entropy. In the example from the previous article, the combination of four quanta within each of the solids would be the combination that also has the highest Entropy.
Energy is also thereby the measurement of the spread of energy within a given situation. Low Entropy occurs when energy or quanta is concentrated in a particularly solid, whereas high Entropy occurs when energy or quanta is spread out.

Since energy and quanta are equivalent to heat why is it that on a sunny day, ice cream always melts when in a system with six bonds and eight quanta there is an eight percent chance of solid one actually acquiring more energy and increasing in temperature, while solid two decreases in quanta and decreases in temperature? This is because systems in real life are composed of millions of bonds and even more quanta. This increase in both bonds and energy decreases the chance of solid one increasing in temperature and solid two decreasing in temperature to such a minuscule number that the occurrence of that event happening is close to none.

Entropy is a tricky subject, but the understanding of it is essential to why we know certain things are hot and others are cold. It is also known as time’s arrow, and is the reason why our hot chocolate emits wisps of condensation in the winter, and why our grills emit the same wisps when we barbecue.