For the phase diagram given, match the labels for: lodine, I, D. 3 A. al B 30 150 Regions A, B, C and D Lines 1, 2, and 3 Points a and b A Choose. Choose. liquid supercritical point D critical region supercritical fluid subliming / depositing triple point 2 Solid 3 vaporizing / condensing critical point a gas melting / freezing b Choose. 2.
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For the phase diagram given, match the labels for:
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- 6.25. Phosphorus exists as several allotropes that have varying properties. The enthalpy of transition from white P to red P, , is . The densities of white and red phosphorus are and , respectively. At what temperature does white phosphorus become the stable phase at of pressure? Assume the formula for phosphorus is .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 vapor pressure, ?, of a certain liquid was measured at two temperatures, ?. The data is shown in the table. T (K) P (kPa) 225 3.32 725 7.66 Keep the pressure units in kilopascals. If you were going to graphically determine the enthalpy of vaporizaton, Δ?vap, for this liquid, what points would you plot? To avoid rounding errors, use three significant figures in the ?‑values and four significant figures in the ?‑values. point 1: ?= point 1: ?= point 2: ?= point 2: ?= Determine the rise, run, and slope of the line formed by these points. rise= run= slope= What is the enthalpy of vaporization of this liquid? Δ?vap=
- Estimate the pressure (atm) necessary to melt ice at -10°C if the molar volume of liquid water is 18.01 mL/mol and the molar volume of ice is 19.64 mL/mol. Δ?̅ (delta S bar) for the process is 122.04 J/mol·K and you can assume that these values remain relatively constant with temperature.Constant Pressure Transitions The next phase diagram looks at the effect of changing pressure at constant temperature. a. Give the state(s) at each of the points 1 to 3.b. Give the state(s) at each of the points 4 to 8.c. Give the state(s) at points 9 and 10.d. Name, and explain the significance of, the point C.The vapor pressure, ?,P, of a certain liquid was measured at two temperatures, ?.T. The data is shown in the table. T (K) P (kPa) 325 3.53 775 6.53 Keep the pressure units in kilopascals. If you were going to graphically determine the enthalpy of vaporizaton, Δ?vap,ΔHvap, for this liquid, what points would you plot? To avoid rounding errors, use three significant figures in the ?x‑values and four significant figures in the ?y‑values. point 1: ?=x= point 1: ?=y= point 2: ?=x= point 2: ?=y= Determine the rise, run, and slope of the line formed by these points. rise=rise= run=run= slope=slope= What is the enthalpy of vaporization of this liquid?
- 1. Substance X has a heat of vaporization of 45.1 kJ/mol at its normal boiling point (423°C). For the process X( l) → X( g) at 1 atm and 423°C calculate the value of Δ S surr.a. 0b. –64.8 J/K molc. 64.8 J/K mold. –107 J/K mole. 107 J/K molFor ether, C2H5OC2H5, the heat of fusion at its normal melting point of -116 °C is 7.3 kJ/mol.The entropy change when 1.58 moles of solid C2H5OC2H5 melts at -116 °C, 1 atm is ______J/K.1. What phase change would occur iat a constant pressure of 0.25 atm the temperature was increased from 0C to 50C? 2.Trace the portion of the line representing melting/freezing with blue ink. Trace boiling/condensation with black ink and the portion representing sublimation in red ink? 3. At what point do all phases exist in equilibrium?
- To vaporize 100.0 g carbon tetrachloride at its normal boiling point, 349.9 K, and P =1 atm, 19.5 kJ of heat is required. Calculate DHvap for CCl4 and compare it with DU for the same process.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?Calculate the amount of energy that is required to heat and completely vaporize a 125 g sample of liquid benzene at 301 K to gaseous benzene at 353 K(molar mass = 78.11 g/mol).The following physical data may be useful:△Hvap = 33.9 kJ/molCliq = 1.73 J/g°CTmelting = 279.0 KTboiling = 353.0 K