Standard Gibbs energy of formation, in kJ molH, at 25°C + 124.5 Benzene, C6H6(1) Carbon dioxide, CO2(g) – 394.4 Carbon monoxide, CO(g) Cyclohexane, C6H12(1) - 137.2 + 26.7 Ethanoic acid, CH3COOH (1) - 299.8 Ethanol, C2H5OH(1) Water, H20(1) - 174.8 - 237.1 1. Calculate the standard Gibbs energy change for the following reactions at 25°C: (а) С>Н:ОН() + 0-(g) —> СНСООН() —+ Н20() (b) 2 CO2(g) → 2 CO(g) + O2(g) Which of the above reactions, as written, is spontaneous at the standard state? [- 362.1; +514.4]

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2. The vapor pressure of tetrachloromethane (tcm) and trichloroethylene (tce) can be expressed as the following functions of T (°C) in the range between the boiling point of pure tem (76.7°C) and tce (87.2°C): 2790.78 In(Picm/torr) × 15.8401 T + 226.4 2345.4 In(Pice/torr) 15.0124 – T + 192.7 Use the information to answer the following questions about a tcm+tce mixture. a. Make a graph of T vs. Xtce and Yice (similar to Figure 24.5) and use this graph to calculate the answers to questions b-d. (Hint: see Example 24-5 on page 975 and lecture slides) b. What is the normal boiling point of the mix when the mole fraction of tce is 0.6 (xtce = 0.6)? c. At the boiling point calculated in (b), what are the mole fractions of tcm and tce (Ytcm and ytce) in the vapor? d. What is the normal boiling point of the condensate of the vapor in (c)?