At the combustion of carbon monoxide proceeds according to the balanced equation 2 ,…

CHEMISTRY · Multi-part · A Level · Chemistry · Thermodynamics · Thermodynamics

Problem

At 298 K298\,\text{K} the combustion of carbon monoxide proceeds according to the balanced equation 2 CO(g)+O2(g)→2 CO2(g)2\,\mathrm{CO}(g) + \mathrm{O}_2(g) \rightarrow 2\,\mathrm{CO}_2(g) The standard molar entropies of two of the substances participating in the reaction are given in the table. Substance  S∘(298 K)S^\circ(298\,\text{K}) CO2(g)\mathrm{CO}_2(g)   213.6 J mol−1 K−1213.6\,\text{J mol}^{-1}\,\text{K}^{-1} O2(g)\mathrm{O}_2(g)   205.0 J mol−1 K−1205.0\,\text{J mol}^{-1}\,\text{K}^{-1} The standard entropy change for the reaction at 298 K298\,\text{K} is ΔSrxn∘=−173.6 J mol−1 K−1\Delta S^\circ_{\text{rxn}} = -173.6\,\text{J mol}^{-1}\,\text{K}^{-1}. (a) Determine the standard molar entropy of CO(g)\mathrm{CO}(g) at 298 K298\,\text{K}. (b) The reaction shows a decrease in the number of gas particles. Using your numerical result from part (a), explain quantitatively whether the sign and magnitude of ΔSrxn∘\Delta S^\circ_{\text{rxn}} are consistent with this observation.

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