Graphite burns in pure oxygen according to the equation For this reaction at the…

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

Problem

Graphite burns in pure oxygen according to the equation C(graphite)+O2(g)→CO2(g)C(\text{graphite}) + O_2(g) \to CO_2(g) For this reaction at 298 K298\,\text{K} the standard entropy change is ΔSrxn∘=−179.0 J mol−1 K−1\Delta S^\circ_{\text{rxn}} = -179.0\,\text{J mol}^{-1}\,\text{K}^{-1}. Additional information is provided in mixed units. Substance  S° C(graphite)C(\text{graphite}): 0.34 cal mol−1 K−10.34\,\text{cal mol}^{-1}\,\text{K}^{-1} CO2(g)CO_2(g): 213.6 J mol−1 K−1213.6\,\text{J mol}^{-1}\,\text{K}^{-1} The accepted literature value for the standard molar entropy of O2(g)O_2(g) at 298 K298\,\text{K} is 205.0 J mol−1 K−1205.0\,\text{J mol}^{-1}\,\text{K}^{-1}. (a) Convert the standard molar entropy of C(graphite)C(\text{graphite}) to SI units with the correct number of significant figures. (b) Using the data above, determine the standard molar entropy of O2(g)O_2(g) at 298 K298\,\text{K}. (c) Calculate the percent error of your result in part (b) relative to the literature value and comment on one plausible experimental or tabulation source of this discrepancy.

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