UF6 is a compound used in the process of enriching uranium. Use the attached thermodynamic data to calculate the temperature for the following phase transition shown at 1 atm. UF6(s) → UF6(g) UF.(g) UF6(s) AH,(g), kJ/mol -2148 -2197 AG, (g), kJ/mol -2029 -2008 s(g), J/K-mol 377 228

Question 2 The value of A H° for the reaction below is -126 kJ. The amount of heat that is released by the reaction of 24 grams of Na, 0, with water is kJ. 2Na202 (s) + 2H2O (1) → 4NaOH (s) + O2 (g) ... Atomic Weight: Na=23 O=16 Enter your answer below. Express the answer in one decimal place. Do not put the unit and sign.

For enthalpy 2 going in the heater, the result is -0.15 kj/mol air.  How was this obtained?

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Based on this diagram, answer the following questions: a) starting from a liquid mixture of 20 mol A and 80 mol B , at which T will it start to boil? b) Which would be the composition of the first vapour appeared? c) At which temperature will disappear the last liquid drop? Which will be its composition? d) How many boiling-condensation cycles would be needed for obtaining compound A with at least 90% purity? Give the composition of each vapour obtained in the process. Results: a) T ≈ 112.2 ºC, yA ≈ 0.30; b) T ≈ 115 ºC, xA ≈ 0.12; * c) 1st step: T ≈ 112.2 ºC yA ≈ 0.30 2nd step: T ≈ 108.5 ºC yA ≈ 0.422 3rd step: T ≈ 105.5 ºC yA ≈ 0.590 4th step: T ≈ 100.5ºC yA ≈ 0.720 5th step: T ≈ 97 ºC yA ≈ 0.820 6th step: T ≈ 94 ºC yA ≈ 0.865 7th step: T ≈ 92.7 ºC yA ≈ 0.925

Consider the reaction: N₂(g) + O2(g) → 2NO(g) Using standard absolute entropies at 298 K, calculate the entropy change for the system when 2.07 moles of N₂ (g) react at standard conditions. Substance So ASO = system NO(g) N₂ (9) O2(g) J/K J K. mol 210.8 191.6 205.1

Consider the following reaction: 4 NH3(g) + 5 O2(g) = 6 H20(g) + 4 NO(g) Calculate AG at 547 K for a mixture of 2.3 bar NH3(g), 3.0 bar O2(g), 4.9 bar H20(g), and 3.6 bar NO(g). State whether or not the reaction is spontaneous at these conditions. **AG° values can be found in textbook appendix** O -929 kJ/mol ; spontaneous -929 kJ/mol ; nonspontaneous O 929 kJ/mol ; spontaneous O 929 kJ/mol ; nonspontaneous

please type out or diagrams so that it is easy to read

Question 3 A vapour-liquid mixture of water (1) and furfural CSH4O2 (2) is maintained at 1.013 bar and 109.5 °C. Under these conditions, it is found that x1 = 0.10 and y1 = 0.81. The temperature of the mixture %3D is changed to 100.6 °C, and some (but not all) of the vapour condenses. The vapour phase may be assumed to behave as an ideal gas. The liquid-phase activity coefficients are independent of temperature but vary with concentration according to the van Laar equations. Determine: (a) The activity coefficients for water and furfural at 1.013 bar and 109.5 °C [9%] (b) The van Laar constants [6% ] Vapour pressure data: T=1006°C, Pa =1.0352 bar, Pl= 0.1193 bar T=109.5°C, Psal -14088 bar, Pal -0.1690 bar %3D

Determine the supersaturation ratio, S, required to permit 0.5-mmdiameter crystals ofsucrose (MW = 342 and ρc = 1,590 kg/m3) to grow if σs,L = 0.01 J/m2. Assume the temperature is 25°C.