Water vapor is an ideal gas. Calculate the internal energy change $(\Delta U)$ when $1 \, \text{mol}$ of water is vaporized at $1 \, \text{bar}$ pressure and $100 \, ^{\circ}C$. (Given: Molar enthalpy of vaporization of water at $1 \, \text{bar}$ and $373 \, K = 41 \, kJ \, \text{mol}^{-1}$ and $R = 8.3 \, J \, \text{mol}^{-1} \, K^{-1}$)
- A$4.100 \, kJ \, \text{mol}^{-1}$
- B$3.7904 \, kJ \, \text{mol}^{-1}$
- C$37.904 \, kJ \, \text{mol}^{-1}$
- D$41.00 \, kJ \, \text{mol}^{-1}$
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$B. HCl_{(g)} \rightarrow H_{(g)} + Cl_{(g)}$
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| $A$. Isothermal process | $i$. $q = \Delta U$ |
| $B$. Adiabatic process | $ii$. $W = - P \times \Delta V$ |
| $C$. Isobaric process | $iii$. $W = \Delta U$ |
| $D$. Isochoric process | $iv$. $W = - nRT \ln \left(\frac{v_f}{v_i}\right)$ |
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