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Entropy change in an ideal gas is a measure of the disorder or randomness of its molecules. It is calculated by taking into account the change in temperature, volume, and pressure of the gas.
This is because an ideal gas follows the laws of thermodynamics, specifically the Second Law which states that in a closed system, the entropy of the system will either remain constant or increase over time. Since an ideal gas does not experience any change in temperature, volume, or pressure, its entropy remains constant and therefore the change in entropy is equal to zero.
No, the entropy change of an ideal gas is only equal to zero when there is no change in its temperature, volume, or pressure. If any of these factors change, the entropy will also change accordingly.
A zero entropy change in an ideal gas indicates that the gas is in a state of thermodynamic equilibrium, where there is no net exchange of energy or matter occurring within the system.
The entropy change of an ideal gas is directly related to its internal energy. An increase in internal energy leads to an increase in entropy, while a decrease in internal energy leads to a decrease in entropy. This relationship is described by the Second Law of Thermodynamics.
