Entropy is a measure of the disorder or randomness in a system. In thermodynamics, it is used to describe the amount of energy that is not available for work.
Entropy can be calculated using the formula ∆S = Q/T, where ∆S is the change in entropy, Q is the heat added or removed from the system, and T is the temperature in Kelvin.
Calculating ∆S for 1 mol of diatomic gas allows us to understand the change in entropy for a specific amount of gas in a given system. This can help us make predictions about the behavior of the gas and its surroundings.
The change in entropy (∆S) can vary for different types of gases depending on their molecular structure and interactions with their surroundings. For example, monatomic gases have a lower ∆S compared to diatomic gases due to their simpler structure.
Temperature has a direct impact on the change in entropy (∆S) for a diatomic gas. As temperature increases, the gas molecules have more energy and can move more freely, leading to an increase in ∆S. Conversely, as temperature decreases, ∆S decreases as the gas molecules have less energy and move less randomly.