Calculate the Gibbs free energy of mixing at a temperature of 25 °C for the mixing of two ideal gases that are in the molar ratio 1:4. The total moles of the two gases combined are 15 moles. Take the universal gas constant, R to be 8.3145 J mol-k!. The pressure of the system is kept constant. A. 18.6 kJ B. -18.6 kJ C.-62.41 J D. 62.41 J E. -1.56 kJ

Calculate the Gibbs free energy of mixing at a temperature of 25 °C for the mixing of two ideal gases that are in the molar ratio 1:4. The total moles of the two gases combined are 15 moles. Take the universal gas constant, R to be 8.3145 J mol-k!. The pressure of the system is kept constant. A. 18.6 kJ B. -18.6 kJ C.-62.41 J D. 62.41 J E. -1.56 kJ

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter6: Equilibria In Single-component Systems

Section: Chapter Questions

Problem 6.32E

See similar textbooks

Similar questions

The ∆G° of vaporization for benzene at 298 K and 1.00 atm is 4.883 kJ/mol. Calculate the pressure, in atm, of benzene vapor in equilibrium with benzene liquid at 298 K.
A solution containing 1.470 g of dichlorobenzene in 50.00 g of benzene boils at 80.60 degree C and a pressureof 1.00 bar. The boiling point of pure benzene is 80.09 degree C, and the molar enthalpy of vaporization of purebenzene is 32.0 kJ/mol. Determine the molecular mass of dichlorobenzene
Calculate the entropy and enthalpy of vaporization for 1 mole of water at room temperature (25oC) and 1 atm from these thermodynamic data:Cm,p(H2O, liquid) = 75.29 J/K·mol, Cm,p(H2O, gas) = 33.58 J/K·mol and ∆vapH(H2O) = 40700 J/ mol (at 100oC)
(3A) Calculate the Gibbs free energy of mixing for 50.0 g water and 50.0 g ethanol at constant 298 K and1.00 bar. What is it about your answer that tells vou that this mixing is spontaneous?AmixG = NRT (x1 In x1 + x2 In x2)
Two phases "a" and "b" of a pure substance are in equilibrium at some temperature and pressure. Which must be true? A)Molar enthalpies of both phases are equal. B)Chemical potentials of both phases are equal C) Molar entropies of both phases are equal D) Volumesof both phases are equal
The Gibbs energy of a pure substance is identical to another thermodynamic quantity: the chemical potential, . How does the chemical potential of liquid water relate to the chemical potential of solid ice at standard pressure (1 bar)? How does this change at high pressure? Does the rate at which the wire moves through the ice depend on the amount of weight placed on the wire? If so, how? Consider whether or not this is an equilibrium process. Does it matter how thick the wire is? If so, why? Does it matter if the wire can conduct heat? If so, why?
2. All liquids have characteristic vapor pressure that vary with temperature. The characteristic vapor pressure for pure water at 22°C is 19.827 mm Hg and at 30.0°C is 31.824 mm Hg. Use these data to calculate the change in enthalphy per mole for the vaporization
A metal salt with the formula MCl2MCl2 crystallizes from water to form a solid with the composition MCl2⋅6H2OMCl2⋅6H2O. The equilibrium vapor pressure of water above this solid at 298 KK is 17.5 mbarmbar . What is the value of ΔrG∘Δr�∘? Express your answer with the appropriate units.
Consider a pure liquid in equilibrium with its vapor at constant temperature. a) write an expression relating the chemical potential of the liquid, u(l), and vapor, u(g). b) express u(g) in terms of the vapor pressure of the pure liquid, P.
The vapour pressure of benzene between 10°C and 30°C fits the expression log(p/Torr) = 7.960 − 1780/T, in K. Calculate (a) the enthalpy of vaporization and (b) the normal boiling point of benzene. Answer: ∆???? = 34.08 kJ/mol ?) ???. ??
In a thermodynamic study, a scientist focuses on the propertiesof a solution in an apparatus as illustrated. A solution iscontinuously flowing into the apparatus at the top and out atthe bottom, such that the amount of solution in the apparatusis constant with time. (a) Is the solution in the apparatusa closed system, open system, or isolated system? (b) If the inletand outlet were closed, what type of system would it be?
Solid benzene melts at 28.35 °C when the pressure is 85.2 MPa. The molar volumes of solid and liquidbenzene at these conditions are 74.25 cm3 mol-1and 82.55 cm3 mol-1, respectively.High Temperature Materials and Processes 26 (2007) 365-369 a. When the pressure is increased to 128 MPa, benzene is found to melt at 39.85 °C. Calculate theenthalpy and entropy of fusion of the solid. b. Estimate the freezing temperature of benzene at 92.5 MPa