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15 Nov 2019
Thermodynamics
Two volatile liquids A and B form a real (non-ideal) solution when mixed together at 300 K The gases above the solution form an ideal mixture. The two liquids are also in equilibrium with each other through the isomerization reaction A(liq)-B(liq) which proceeds only in the liquid phase. The equilibrium constant for the reaction is Keq xBXA. The vapor pressures of the pure liquids A and B at 300 K are p* = 0.3 bar and p* = 0.4 bar a) Considering all relevant constraints, use the Gibbs phase rule to determine the number of independent variables in the system. If possible, write down as many constraints as possible. b) The mole fraction of B in the gas phase is found to be yB-0.01. What is the mole fraction of A in the gas phase yA? c) Does pA for this mixture follow Raoult's Law or Henry's Law and why? Write the appropriate expression for xA in terms of pA d) Does pB for this mixture follow Raoult's Law or Henry's Law and why? Write the appropriate expression for xB in terms of pB
Thermodynamics
Two volatile liquids A and B form a real (non-ideal) solution when mixed together at 300 K The gases above the solution form an ideal mixture. The two liquids are also in equilibrium with each other through the isomerization reaction A(liq)-B(liq) which proceeds only in the liquid phase. The equilibrium constant for the reaction is Keq xBXA. The vapor pressures of the pure liquids A and B at 300 K are p* = 0.3 bar and p* = 0.4 bar a) Considering all relevant constraints, use the Gibbs phase rule to determine the number of independent variables in the system. If possible, write down as many constraints as possible. b) The mole fraction of B in the gas phase is found to be yB-0.01. What is the mole fraction of A in the gas phase yA? c) Does pA for this mixture follow Raoult's Law or Henry's Law and why? Write the appropriate expression for xA in terms of pA d) Does pB for this mixture follow Raoult's Law or Henry's Law and why? Write the appropriate expression for xB in terms of pB
aramracla23Lv4
26 May 2023
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