Chemistry

Chemistry

Problem

The following elementary reactions have known standard entropy changes. (1) CaCO3(s)→CaO(s)+CO2(g)ΔS1∘=+160.5 J mol−1 K−1\displaystyle \text{CaCO}_3(s) \rightarrow \text{CaO}(s) + \text{CO}_2(g) \qquad \Delta S_1^\circ = +160.5\,\text{J\,mol}^{-1}\,\text{K}^{-1} (2) CaO(s)+H2O(l)→Ca(OH)2(s)ΔS2∘=−83.4 J mol−1 K−1\displaystyle \text{CaO}(s) + \text{H}_2\text{O}(l) \rightarrow \text{Ca(OH)}_2(s) \qquad \Delta S_2^\circ = -83.4\,\text{J\,mol}^{-1}\,\text{K}^{-1} What is ΔS∘\Delta S^\circ for the overall reaction? CaCO3(s)+H2O(l)→Ca(OH)2(s)+CO2(g)\displaystyle \text{CaCO}_3(s) + \text{H}_2\text{O}(l) \rightarrow \text{Ca(OH)}_2(s) + \text{CO}_2(g) a) +243.9 J mol−1 K−1+243.9\,\text{J\,mol}^{-1}\,\text{K}^{-1} b) −6.3 J mol−1 K−1-6.3\,\text{J\,mol}^{-1}\,\text{K}^{-1} c) +77.1 J mol−1 K−1+77.1\,\text{J\,mol}^{-1}\,\text{K}^{-1} d) −77.1 J mol−1 K−1-77.1\,\text{J\,mol}^{-1}\,\text{K}^{-1}

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