AP Chemistry
9.5 Free Energy and Equilibrium
9.3 Gibbs Free Energy and Thermodynamic Favorability
A student investigates the thermodynamic properties of a reaction between two gases at \(298\text{ K}\), represented by the balanced equation below.
\[ \text{X(g)} + \text{Y(g)} \rightleftharpoons \text{XY(g)} \]
The reaction has a standard enthalpy change, \(\Delta H^\circ\), of \(-10.0\text{ kJ/mol}_{\text{rxn}}\) and a standard entropy change, \(\Delta S^\circ\), of \(-110.0\text{ J}/(\text{mol}_{\text{rxn}}\cdot\text{K})\). Given that \(2.303 RT \approx 5.70\text{ kJ/mol}\) at \(298\text{ K}\) and \(\Delta G^\circ = -2.303 RT \log_{10} K\), what is the value of the equilibrium constant, \(K\), for the reaction at \(298\text{ K}\)?
\[ \text{X(g)} + \text{Y(g)} \rightleftharpoons \text{XY(g)} \]
The reaction has a standard enthalpy change, \(\Delta H^\circ\), of \(-10.0\text{ kJ/mol}_{\text{rxn}}\) and a standard entropy change, \(\Delta S^\circ\), of \(-110.0\text{ J}/(\text{mol}_{\text{rxn}}\cdot\text{K})\). Given that \(2.303 RT \approx 5.70\text{ kJ/mol}\) at \(298\text{ K}\) and \(\Delta G^\circ = -2.303 RT \log_{10} K\), what is the value of the equilibrium constant, \(K\), for the reaction at \(298\text{ K}\)?
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