please show all work for both... (especially #12 I need help with the most. incl
ID: 705866 • Letter: P
Question
please show all work for both... (especially #12 I need help with the most. including formulas)
12. The enthalpy of vaporization of liquid mercury is 59.11 kJ/mol. What quantity of energy as heat is required to vaporize 0.500 mL of mercury at 357 °C, its normal boiling point? The density of mercury is 13.6 g/ml 13. Answer the following questions using Figure 11.12: (a) What is the approximate equilibrium vapor pressure of water at 60 °C? Compare your answer with the data in Appendix G At what temperature does water have an equilibrium vapor pressure of 600 mm Hg? (c) Compare the equilibrium vapor pressures of water and ethanol at 70 °C. Which is higher?Explanation / Answer
Ans 12 :
Density = mass / volume
13.6 = m / 0.500
m = 6.8 grams
Number of moles of mercury = 6.8 / 200.59
= 0.034 mol
Energy required for vaporization = number of moles × enthalpy of vaporization
= 0.034 × 59.11
= 2.004 KJ
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