AP Chemistry
9.3 Gibbs Free Energy and Thermodynamic Favorability
The vaporization of liquid water is represented by the following equation.
\[ \text{H}_2\text{O}(l) \rightleftharpoons \text{H}_2\text{O}(g) \]
At \(298\text{ K}\), the standard enthalpy of vaporization, \(\Delta H^\circ\), is \(+44.0\text{ kJ/mol}_{\text{rxn}}\), and the standard entropy of vaporization, \(\Delta S^\circ\), is \(+118\text{ J/}(\text{mol}_{\text{rxn}}\cdot\text{K})\). Based on this information, what is the value of the standard Gibbs free energy change, \(\Delta G^\circ\), for the vaporization of water at \(298\text{ K}\)?
\[ \text{H}_2\text{O}(l) \rightleftharpoons \text{H}_2\text{O}(g) \]
At \(298\text{ K}\), the standard enthalpy of vaporization, \(\Delta H^\circ\), is \(+44.0\text{ kJ/mol}_{\text{rxn}}\), and the standard entropy of vaporization, \(\Delta S^\circ\), is \(+118\text{ J/}(\text{mol}_{\text{rxn}}\cdot\text{K})\). Based on this information, what is the value of the standard Gibbs free energy change, \(\Delta G^\circ\), for the vaporization of water at \(298\text{ K}\)?
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