In which phase boundary is the equation, p = P* + - In applicable AV. T* O Solid-liquid boundary O Liquid-vapor boundary O Solid-vapor boundary Miscibility boundary
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- 1. It is the lowest temperature at which a liquid is present in a solid-liquid system. 2. It is the point where the concentrations of both equilibrium phases in a liquid-liquid system are equal. 3. What do you call the state at which the compositions of the vapor and liquid are equal? 4. In a vapor liquid system, at what point will the mixture becomes a saturated vapor? Choices Dew point critical point triple point bubble point azeotrope eutectic point immisibility supercritical fluid plait pointMelting enthalpy of ice at 1 bar 9.134 kJ /mol; At 0 ° C, the density of water is 999.9 kg m-3, and the density of ice is 812.0 kg m-3. Assuming that the molar volume and enthalpy change in fusion are constant, find the freezing point of water at 85 bar using the information given?Based on the phase diagram illustated below, what is the phase condition of the given two-component system (w and b)? 3.5 bar at 0.32 of b 4.5 bar at 0.55 of b 1.2 bar at 0.23 of w 3.5 bar at 0.8 of w A. liquid w + vapor B. All liquid C. All vapor
- What is the change in the boiling point of water at 1000 C per Pa change under atmospheric pressure conditions? The molar enthalpy of vaporization is 40.69 kJ mol-1, the molar volume of liquid water is 0.019 x 10-3 m3 mol-1, and the molar volume of steam is 30.199 x 10-3m3 mol-1, all at 100.000 C and 1.01325 bar. (Hint: change in temperature per change in pressure, dT/dP).How many phases are present at each of the points a–d indicated in Fig. 4.1a?In the systems given below determine the number of phases, number of components with names and degrees of freedom using the Gibbs Phase rule. I. S(rhombic) ⇆ S(monoclinic) ⇆ S(liquid) ⇆ S(gas) II. PCl5 (g) ⇆ PCl3 (g) + Cl2 (g) i) PPCl3 = PCl2 ii) PPCl3 ≠ PCl2 (PA – is partial pressure of A)
- An unknown liquid is 2.77x104 Pa at 25°C and 5.643x104 Pa at 50 °C. has the x kJ/mol enthalpy of vaporization (ΔHvap), based on the Clausius-Clapeyron equation. What is the value of x in 3 significant figures?give 5 examples of a 1 phase diagram and show its phase rule1. What is the apparent hard-sphere diameter of CO2 at 0°C? The viscosity of CO2(g) at 1 atm and 0°C is 139 μP (micropoise). 2. When equal amounts of hydrogen, H2, and iodine, I2, are mixed together at a total pressure of 1 bar, the partial pressure of hydrogen iodide, HI, vapour produced from by the reaction H2(g) + I2(g) ⇌ 2 HI(g) is 22.8 kPa. Calculate the equilibrium constant for the reaction. 3. The equilibrium constant for the reaction 2HCl(g) + O2(g) ⇌ H2O(g) + Cl2(g) is 13300 at 400 K and 429 at 500 K. Use the van't Hoff equation to determine the standard enthalpy of reaction.
- Melting enthalpy of ice at 1 bar 9.134 kJ /mol; At 0 ° C, the density of water is 999.9 kgm-3, and the density of ice is 812.0 kg m-3. Assuming that the molar volume and enthalpy change in fusion are constant, find the freezing point of water at 85 bar using the informationgiven?At the pressure of 1.68 atm, the enthalpy of fusion is 4.96 kJ/mol at freezing point 140.83 K and enthalpy of vaporization is 32.82 kJ/mol at boiling point 398.75 K. Calculate the slope dP/dt (atm/K) of the solid-vapor boundary for gas A at 169.07 K. Assume gas A behaves ideally.Pressure was exerted with a piston on molten naphthalene at 95 °C. The vaporpressure of naphthalene when the applied pressure is 1.0 bar is 2.0 kPa. What is thevapor pressure when the pressure on the liquid is 15 MPa? The mass density ofnaphthalene at this temperature is 1.16 g cm-1.