(a) What is the difference between the states of phase equilibrium and metastability (b) Explain with the aid of neatly drawn binary phase diagrams the following terms
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- a) The following temperature composition data were obtained for a mixture of two liquids A and B at one atmosphere, where x is the mole fraction of A in the liquid and y is the mole fraction of A in the vapour, at equilibrium.t/ oC 125 130 135 140 145 150xA 0.91 0.65 0.45 0.30 0.18 0.098yA 0.99 0.91 0.77 0.61 0.45 0.25the boiling points are 124 oC for A and 155 oC for B. Plot the temperature-composition diagram for the mixture on a graph sheet. What is the composition of the vapour in the equilibrium with the liquid of composition i) xA = 0.50 and ii) xB= 0.33What is ΔSsys for a freezing phase transition at 29.7 °C for a compound that freezes at 29.7 °C and the ΔHsys = -19.45 kJ mol-1 for this process? Express your answer in J mol-1 K-1 to at least two significant figures.The following temperature/composition data were obtained for a mixture of two liquids A and B at 1atm, where x is the mole fraction in the liquid and y the mole fraction in the vapour at equilibrium.T (°C) 110 120 130 140xA 0.73 0.43 0.25 0.10yA 0.96 0.78 0.60 0.36The boiling points are 105°C for A and 150°C for B. What is the composition of the vapour in equilibrium with the liquidof composition (a) xA = 0.35 and (b) xB = 0.25?
- A saturated solution of copper(ll) sulfate, with excess of the solid, is present in equilibrium with its vapour in a closed vessel. (a) How many phases and components are present? (b) How many degrees of freedom are available, and what are they?The table below shows temperature/composition data collected for a mixture of methylbenzene (M) and octane (O) at 1 atm. Recall that x stands for the mole fraction in the liquid and y stands for the mole fraction in the vapor in equilibrium. The boiling points for methylbenzene (M) and octane (O) are 110.60C and 125.60C, respectively. Construct the phase diagram with Temperature vs. xM. What is the composition of the vapor in equilibrium with the liquid of composition (a) xM = 0.250 and (b) xO = 0.250. T (0C) 110.9 112.0 114.0 115.8 117.3 119.0 121.1 123.0 xM 0.908 0.795 0.615 0.527 0.408 0.300 0.203 0.097 yM 0.923 0.836 0.698 0.624 0.527 0.410 0.297 0.164Give the relation between gas-phase composition and liquid-phase composition at equilibrium.
- The following temperature composition data were obtained for a mixture of two liquids A and B at one atmosphere, where x is the mole fraction of A in the liquid and y is the mole fraction of A in the vapour, at equilibrium. V °C XA YA 125 0.91 0.99 130 0,65 0.91 135 0.45 0.77 140 0.30 0.61 145 0.18 0.45 150 0.098 0.25 the boiling points are 124 °C for A and 155 °C for B. Plot the temperature-composition diagram for the mixture on a graph sheet. What is the composition of the vapour in the equilibrium with the liquid of composition i) XA = 0.50 and ii) Xp=0.33The following temperature-composition data were obtained for a mixture of octane (O) and methylbenzene (M) at 1.00 atm, where x is the mole fraction in the liquid and y the mole fraction in the vapour at equilibrium. The boiling points are 110.6oC and 125.6oC for M and O, respectively Plot the temperature-composition diagram for the mixture. What is the composition of the vapour in equilibrium with the liquid of composition (i)Xm =0.250 and (ii) Xo =0.250?A liquid-vapour mixture whose composition is 60 mole % of benzene is contained within a vessel at 60C. What fraction of moles are both methanol and in the liquid phase?
- It is found that the boiling point of a binary solution of A andB with xA = 0.6589 is 88 °C. At this temperature the vapour pressuresof pure A and B are 127.6 kPa and 50.60 kPa, respectively. (i) Is thissolution ideal? (ii) What is the initial composition of the vapour abovethe solution?Draw a complete phase diagram for One-component system of H2O. Discuss how phase rule can be applied to the ‘phase boundaries’ and ‘phase regions’.Establish the phase equilibrium for nonreacting systems in terms of the specific Gibbs function of the phases of a pure substance