Like most substances, bromine exists in one of the three typical phases. Br2 has a normal melting point of 27.2oC and a normal boiling point of 59oC. The triple point for Br2 is 27.3oC and 40 torr, and the critical point is 320oC and 100 atm. Using this information, sketch a phase diagram for bromine indicating the points described above. Based on your phase diagram, order the three phases from least dense to most dense. What is the stable phase of Br2 at room temperature and 1 atm? Under what temperature conditions can liquid bromine never exist? What phase changes occur as the temperature of a sample of bromine at 0.10 atm is increased from 250oC to 200oC?
Answer to relevant QuestionsConsider the following phase diagram. What phases are present at points A through H? Identify the triple point, normal boiling point, normal freezing point, and critical point. Which phase is denser, solid or liquid? Consider the following data for xenon: Triple point: ...... –121oC, 280 torr Normal melting point: ... –112oC Normal boiling point: ... –107oC Which is more dense, Xe(s) or Xe(l)? How do ...A special vessel (see Fig. 16.52) contains ice and super-cooled water (both at –10oC) connected by vapor space. Describe what happens to the amounts of ice and water as time passes. Figure 16.52. a. Use the following data to calculate the enthalpy of hydration for calcium chloride and calcium iodide. b. Based on your answers to part a, which ion, Cl2 or I2, is more strongly attracted to water? The solubility of nitrogen in water is 8.21 × 10-4 mol/ L at 0oC when the N2 pressure above water is 0.790 atm. Calculate the Henry’s law constant for N2 in units of L atm/mol for Henry’s law in the form P = kC, where C ...
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