Chapter 9, Problem 27E

One mole of ${\text{H}}_{\text{2}}\text{O}\left(\text{g}\right)$ at $\text{1}\text{.00 atm}$ and $\text{100}\text{.°C}$ occupies a volume of $\text{30}\text{.6 L}$ . When $\text{1 mole}$ of ${\text{H}}_{\text{2}}\text{O}\left(\text{g}\right)$ is condensed to $\text{1 mole}$ of ${\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$ at $\text{1}\text{.00 atm}$ and $\text{100}\text{.°C}$ , $\text{40}\text{.66 kJ}$ of heat is released. If the density of ${\text{H}}_{\text{2}}\text{O}\left(\text{l}\right)$ at this temperature and pressure is $\text{0}{\text{.996 g/cm}}^{\text{3}}$ , calculate $\text{ΔE}$ for the condensation of $\text{1 mole}$ of water at $\text{1}\text{.00 atm}$ and $\text{100}\text{.°C}$ .