Consider the reaction \[ \mathrm{CO}(\mathrm{g})+\mathrm{Cl}_{2}(\mathrm{~g}) \longrightarrow \mathrm{COCl}_{2}(\mathrm{~g}) \] Use the standard thermodynamic data in the tables linked above. Calculate \( \Delta G \) for this reaction at \( 298.15 \mathrm{~K} \) if the pressure of \( \mathbf{C O C l}_{2}(\mathrm{~g}) \) is reduced to \( 20.87 \mathrm{~mm} \mathrm{Hg} \), while the pressures of \( \mathrm{CO}(\mathrm{g}) \) and \( \mathrm{Cl}_{2}(\mathrm{~g}) \) remain at \( 1 \mathrm{~atm} \). ANSWER: \( \square \) \( \mathrm{kJ} / \mathrm{mol} \)
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\[ \mathrm{CO(g)} + \mathrm{Cl}_2(\mathrm{g}) \longrightarrow \mathrm{COCl}_2(\mathrm{g}) \] Show more…
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