AP Chemistry
6.9 Hess’s Law
6.8 Enthalpy of Formation
6.5 Energy of Phase Changes
The standard enthalpies of formation, \(\Delta H_f^\circ\), for gaseous and liquid water at \(298\text{ K}\) and \(1\text{ atm}\) are given in the table below.
Which of the following best explains why the standard enthalpy of formation of \(\text{H}_2\text{O}(l)\) is more negative than that of \(\text{H}_2\text{O}(g)\)?
| Substance | State | \(\Delta H_f^\circ\text{ (kJ/mol)}\) |
|---|---|---|
| \(\text{H}_2\text{O}(g)\) | Gas | \(-242\) |
| \(\text{H}_2\text{O}(l)\) | Liquid | \(-286\) |
Which of the following best explains why the standard enthalpy of formation of \(\text{H}_2\text{O}(l)\) is more negative than that of \(\text{H}_2\text{O}(g)\)?
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