Calculate $\Delta \mathrm{S}^{\circ}$ for the following reaction: $\mathrm{SnCl}_{4}(\mathrm{l}) \rightarrow \mathrm{SnCl}(\mathrm{g})$.

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∻Solution∻ ‖ 1 ⋮ **Identify the reaction**: The given reaction is $ \mathrm{SnCl}_{4}(\mathrm{l}) \rightarrow \mathrm{SnCl}(\mathrm{g}) $. ‖ ‖ 2 ⋮ **Determine the standard entropy change ($\Delta S^{\circ}$)**: To calculate $\Delta S^{\circ}$, we need the standard molar entropies ($S^{\circ}$) of the reactants and products. The formula is: $$ \Delta S^{\circ} = \sum S^{\circ}(\text{products}) - \sum S^{\circ}(\text{reactants}) $$ Given the standard molar entropies: - $S^{\circ}(\mathrm{SnCl}_{4}(\mathrm{l})) = S^{\circ}_{\mathrm{SnCl}_{4}(\mathrm{l})}$ - $S^{\circ}(\mathrm{SnCl}(\mathrm{g})) = S^{\circ}_{\mathrm{SnCl}(\mathrm{g})}$ The calculation is: $$ \Delta S^{\circ} = S^{\circ}_{\mathrm{SnCl}(\mathrm{g})} - S^{\circ}_{\mathrm{SnCl}_{4}(\mathrm{l})} $$ ‖ ∻Answer∻ ⚹ The standard entropy change ($\Delta S^{\circ}$) for the reaction is calculated using the standard molar entropies of the reactants and products. ⚹ ∻Key Concept∻ ⚹ Standard entropy change ($\Delta S^{\circ}$) ⚹ ∻Explanation∻ ⚹ The standard entropy change for a reaction is determined by subtracting the sum of the standard molar entropies of the reactants from the sum of the standard molar entropies of the products. ⚹◊What is the standard entropy change ($\Delta \mathrm{S}^{0}$) for the reaction: $\mathrm{SnCl}_{4}(\mathrm{l}) \rightarrow \mathrm{SnCl}(\mathrm{g})$?⍭ Generate me a similar question◊

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