Consider a binary mixture for which the excess Gibbs energy is given by GEIRT = 2.6x1x2. For each of the following overall compositions, determine whether one or two liquid phases will be present. If two liquid phases will be present, find their composi- tions and the amount of each phase present (phase fractions). a) Z₁ = 0.2 b) z₁ = 0.3 c) Z₁ = 0.5 d) z₁ = 0.7 e) Z₁ = 0.8

Consider a binary mixture for which the excess Gibbs energy is given by GEIRT = 2.6x1x2. For each of the following overall compositions, determine whether one or two liquid phases will be present. If two liquid phases will be present, find their composi- tions and the amount of each phase present (phase fractions). a) Z₁ = 0.2 b) z₁ = 0.3 c) Z₁ = 0.5 d) z₁ = 0.7 e) Z₁ = 0.8

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

(a) The heat evolved upon dissolution of atmospheric ozone into water is determined to be +5 kcal/mol at 298 K. Given that ozone has a Henry’s constant of 9.4 × 10−3 mol/L/atm at 298 K, determine its Henry’s constant at 273 K. Note that the definition of Henry’s constant is for the process air to water. (b) If the atmospheric ozone concentration in a polluted air is 100 ppbv, what is the concentration in equilibrium with a body of water in that region at 298 K? Note that you need to assume no losses of ozone other than absorption into water
2.28(b) Set up a thermodynamic cycle for determining the enthalpy of hydration of Ca?+ ions using the following data: enthalpy of sublimation of Ca(s), +178.2 kJ mol-1; first and second ionization enthalpies of Ca(g), 589.7 kJ mol-1 and 1145 kJ mol¬1; enthalpy of vaporization of bromine, +30.91 kJ mol-1; dissociation enthalpy of Br,(g), +192.9 kJ mol-1; electron gain enthalpy of Br(g), –331.0 kJ mol-1; enthalpy of solution of CaBr,(s), –103.1 kJ mol-'; enthalpy of hydration of Br¯(g), –337 kJ mol¬!.
b) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction СO(g) +2H2(g) — CHОН (g) At 298.15 K, AH.co (0)= -26.41 kcal/mol, AH AG.co (9)= -32.8079 kcal/mol, AG cH,oh(9)= -38.69 kcal/mol, °.CH20H(9)= -48.08 kcal/mol, The standard heat capacity of various components is given by, CO = a + bT + cT² + dT³, where C, is in cal/mol-K and T is in K b x10² с х105 d x10° Соmponent CH3OH а 4.55 2.186 -0.291 -1.92 CO 6.726 0.04 0.1283 -0.5307 H2 6.952 -0.0457 0.09563 -0.2079
= The vapor pressure of component A'is 300.3 torr, and that of component B is 70 torr at 35 °C. A Solution of A and B at 35 °C with x = 0.300 has a vapor pressure of 70.3 torr and a vapor composition of x = 0.275. (i) Calculate yand a, for component A and for component B in this solution. %3D -tin. (ii) Calculate u - Hi for each component of this solution. (iii) Calculate AG for the mixing of 0.200 mole of liquid component B and 0.800 mole of liquid chloroform at 35 "c. (iv) Calculate AGmix for the corresponding ideal solution.
The standard Gibbs energy of formation of NH3(g) at 298 K is ─16.6 kJ mol-1. Based on this data, calculate (a) the standard Gibbs energy of reaction and (b) the pressure equilibrium concentration for the reaction N2(g) + 3 H2(g) = 2 NH3(g) Answer:[-33.2; 6.6 x 105 ]
70.3(b) Calculate the Gibbs energy, entropy, and enthalpy of mixing when 25 g of hexane is mixed with 25 g of heptane at 298 K; treat the solution as ideal.
(2.) Sketch a boiling temperature – mole fraction phase diagram for a mixture of A and B (A more volatile than B) showing positive deviations from Raoult's law, labelling the important regions on the diagram, including the azeotropic point. Use the Gibbs phase rule to calculate the number of degrees of freedom for the azeotropic mixture.
(A) It is required to separate 1 mole of ethanol from ethanol-water mixture by using distillation Column at standard conditions. After 1 hour, it is found that the volume was double and the pressure increased to 152 kpa. Find the Temperature after 1 hour by using the ideal gas law: PV = nRT Given : R = 0.082 L.atm/mole.K (B) Calculate the capacity of a Base added to a solution contains 10 mole of ammonia (k, = 1.8x105) and 6 mole of ammonium chloride in 120 ml? Note: Atomic weight: H = 1, 0 = 16, C = 12, Ba = 137, Cl= 35 , N=14
Figure 5.2 shows the experimentally determined phase diagrams for the nearly ideal solution of hexane and heptane. (a) Indicate which phases are present in each region of the diagram. (b) For a solution containing 1 mol each of hexane and heptane molecules, estimate the vapour pressure at 70 °C when vaporization on reduction of the external pressure just begins. (c) What is the vapour pressure of the solution at 70 °C when just one drop of liquid remains? (d) Estimate from the figures the mole fraction of hexane in the liquid and vapour phases for the conditions of part b. (e) What are the mole fractions for the conditions of part c? (f) At 85 °C and 760 Torr, what are the amounts of substance in the liquid and vapour phases when zheptane = 0.40?
A reaction mixture (mixture 1) at 298 K has a N2O4(g) partial pressure of 0.1 bar anda NO2(g) partial pressure of 0.05 bar. Calculate the reaction Gibbs energy (∆??) formixture 1 at 298 K. A second reaction mixture (mixture 2) is prepared at 298 K with a N2O4(g) partialpressure of 0.05 bar and a NO2(g) partial pressure of 0.10 bar. (i) Calculate the reaction Gibbs energy (∆??) for mixture 2 at 298 K. (ii) Comment on the spontaneity of the forward reaction for mixture 1 and mixture 2.Support your answer with the values of ∆?? calculated for the two mixtures. please give solution and answer
At 1400. K, the equilibrium constant, KC, for the reactionH2O(g) + CH4(g) ⇆ CO(g) + 3 H2(g) (2.1)is KC = 4.7Give the expression for KC for reaction 2.1
3.2 The standard Gibbs energy of formation of H20 at 25.0 °C, A,G°, is -228.57 kJ.mol', for a standard state of 1 atm. The reaction is: 2 H20 (g)→02 (g) +2H2 (g) (a) Calculate 4,G° (kJ.mol') for the above reaction. (b) Calculate the value of the equilibrium constant, K, for the above reaction. (c) Calculate the value of K, at 5 atm.