Import Question JSON

$\text{Hint: Use the concept of the 2nd law of thermodynamics}$ $\text{Step 1: Understand what entropy is and how it's defined}$ $\text{Entropy (S) is a thermodynamic property that measures the degree of disorder or randomness in a system. It is related to the second law of thermodynamics, which states that the entropy of an isolated system always increases over time.}$ $\text{Step 2: Examine the mathematical definition of entropy}$ $\text{According to the second law of thermodynamics, for a reversible process, the change in entropy (}\Delta\text{S) is defined as:}$ $\Delta\text{S} = \frac{q_{\text{rev}}}{\text{T}}$ $\text{where:}$ $q_{\text{rev}} = \text{heat transferred in a reversible process (J)}$ $\text{T} = \text{temperature (K)}$ $\text{Step 3: Determine the unit of entropy based on this definition}$ $\text{From the equation above, we can derive the unit of entropy:}$ $\text{Unit of } \Delta\text{S} = \frac{\text{Unit of heat}}{\text{Unit of temperature}} = \frac{\text{Joule (J)}}{\text{Kelvin (K)}}$ $\text{For molar entropy, we include mol}^{-1} \text{ in the unit:}$ $\text{Unit of molar entropy} = \text{J K}^{-1} \text{mol}^{-1} \text{ or } \text{J mol}^{-1} \text{K}^{-1}$ $\text{The correct representation is J mol}^{-1} \text{K}^{-1}\text{, which indicates joules per mole per kelvin.}$ $\text{Therefore, the unit of entropy is J mol}^{-1} \text{K}^{-1}$