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- Given the following data about xenon, normalboilingpoint=108Cnormalmeltingpoint=112Ctriplepoint=121Cat281mmHgcriticalpoint=16.6Cat58atm (a) Construct an approximate phase diagram for xenon. (b) Estimate the vapor pressure of xenon at -115C. (c) Is the density of solid Xe larger than that for liquid Xe?7. (5)Consider the phase diagram given below atm ス50 T°C aら 50 15 100 |50 200 Identify the normal boiling point, and normal freezing point. fp. Which phase, solid or liquid is most densed? bp Indicate the Triple point and the critical point on the diagram.Sulfur exhibits two solid phases, rhombic and monoclinic. Use the accompanying phase diagram for sulfur given below to answer the questions that follow. (A). How many triple points are in the phase diagram? (B). What phases are in equilibrium at the topmost triple point? (C). How many phase transitions are there when rhombic sulfur at 1 atm and 80°C is heated to 500°C at constant pressure?
- (3) Vapor pressure of liquid ethanol is 7291 Pa at 20°C. (a) one student reports that the vapor pressure is 31741 Pa at 52°C. Another student reports it to be 31741 Pa at 502°C. Which of the results is correct? Why? (b) calculate the normal boiling temperature of ethanol (assume Patm=101,325Pa).2. Below is the phase diagram of sulphur. At 95.4°C, the densities of rhombic and monoclinic sulphur are 2.07 g cm³ and 1.96 g cm³, whilst the enthalpy change for phase transition from rhombic to monoclinic sulphur is 0.3 kJ mol1. Sulfur 153°C, 1420 atm Liquid 95.4°C 115.21°C 1 atm P Monoclinic 444.6°C 115.2°C, 3.2 x 105 atm Rhombic 95.3°C, 5.1 x 10-6 atm Gas TQuestion 7 Use the phase diagram below to state what would be observed when a sample of carbon dioxide, initially at 1.00 atm and 298 K, is subjected to the following cycle: Isobaric cooling to 210 K, Solid Critical point 72.9 Liquid 67 5.11 Triple point 1.0 Gas 154.7 216.8 298.15 (7,) (T) 304 2 (T) Temperature, TIK O A. Gas will be formed. B. More liquid will be formed O C. Gas is formed since solid sublime at 1 atm. D. Solid, gas mixture. OE. Liquid, gas mixture 15°C Light rain )ENG platm
- ANS B ONLY a. The molar volume of a certain solid is 142.0 cm3 mol−1 at 1.00 atm and 427.15 K, its melting temperature. The molar volume of the liquid at this temperature and pressure is 152.6 cm3 mol−1. At 1.2 MPa the melting temperature changes to 429.26 K. Calculate the enthalpy (KJ/mol) and entropy of fusion (J/mol-K) of the solid. b. Calculate the melting point of ice under a pressure of 10 MPa. Assume that the density of ice under these conditions is approximately 0.915 g cm−3 and that of liquid water is 0.998 g cm−3. From the result of the calculation, what happens when you increase the pressure on water, will it freeze or will the ice melt?The standard boiling point of pure toluene is 384 K. At 384 K, the equilibrium vapor pressure of another pure liquid E is 0.250 bar. Their latent heats of vaporization delta Hm,vap are 32.30 kJ/mol for toluene and 16.15 kJ/mol for E. At what temperature would you estimate that the two substances, toluene and E, have the same equilibrium vapor pressure?2. Which one of the following statements is incorrect? (a) According to the Gibbs phase rule, four phases of a pure substance cannot exist (b) All triple points correspond to a gas-liquid-solid equilibrium (c) The triple point in a P-T diagram becomes a triple line in a P-V diagram (d) The chemical potential determines which of several phases is the most stable
- The melting point of water at the pressure of the interest (1 atm) is 0 oC and the enthalpyof fusion is 6 kJmol-1. The boiling point is 100 oC and the enthalpy of vaporization is40kJmol-1.Calculate ΔH and ΔS for the transformation of 5 grams of H2O (ice) from (s, -10/X oC)to H2O (g, 1000/X oC)cp (water)= 75.3 joule/mole.K. cp (ice)=36.2 joule/mole.K x=4.5The fragment of H2O phase diagram is shown. A) What transition (e.g. liquid--> solid, solid-->gas... or none) would be observed when a sample of H2O initially at 0.003atm and -5 C is heated at constant pressure to 50 C? B) How many phases coexist at point with T = 100 oC and p = 1 atm?2. All liquids have characteristic vapor pressure that vary with temperature. The characteristic vapor pressure for pure water at 22°C is 19.827 mm Hg and at 30.0°C is 31.824 mm Hg. Use these data to calculate the change in enthalphy per mole for the vaporization