Q3: An equimolar liquid mixture of ethanol and water is in equilibrium with its vapor at 50° C. Calculate: (1) The system pressure (2) The composition of the vapor. (3) The average molecular mass of the liquid phase. Antoine constants |Component A Water Ethanol 3816.44- 46.13 3703.98- 41.01 18.30 16.91
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- (a)At 0 oC, liquid water and ice are in equilibrium at standard pressure, so they have the SAME molar Gibbs energy. When raise from 1.0 bar to 100 bar, how much Gibbs free energy change in the liquid phase ? (molar mass of water 18 g mol-1; mass density of ice = 0.9150 g cm-3; mass density of liquid water, 0.9999 g cm-3) Set the initial Gibbs energy = 0 if you like. (b) how much Gibbs free energy change in the solid phase? c) under this process according to your calculation , solid changes to liquid. Liquid changes to solidCoiled coils are protein domains that lead to the formation of multimers (dimers,trimers, tetramers, etc.). They are found in a wide range of proteins. Here we willconsider the trimerization reaction. We may write the chemical equilibrium as3 M(aq) ⇄ T(aq)where M and T represent, respectively, the monomer and trimer species. Given that∆rG0 = −25.00 kJ mol−1 at 37 0C (with the standard state the normal one for reactionsin solution, namely c0 = 1.0 mol dm−3):A) What is the equilibrium constant for the formation of the trimer at 37 0C? B) Suppose that in a particular experiment at 37.00 0C the initial concentrations ofthe monomer if [M]0 = 2.00×10−2 µM and the initial concentration of the trimeris also [T]0 = 2.00 × 10−2 µM. What is ∆rG for the formation of the trimer atthe specified temperature? C) For the conditions given in part (B) will trimers spontaneously convert to monomers?Give a very short justification of your answer. D) Suppose that ∆rH0 and ∆rS0 are independent of the…Consider the synthesis of sulphur trioxide from its elements at 25oC:1/4 S8 (s) + 3O2(g) → 2SO3 (g) Thermodynamic Data: Species ∆fHo(kJ/mol)(at 298.15 K) So (J/K.mol)(at 298.15 K) ∆fGo (kJ/mol)(at 298.15 K) S8(s) 102 431 50 O2(g) 205 SO3 (g) -396 257 -371 2.1.1 Calculate ∆rGo , using only Gibbs energy values.2.1.2 Calculate the equilibrium constant, K, at 25oC for this reaction 2.1.3 Calculate ∆Ssurr for the synthesis of sulphur trioxide at 25oC 2.1.4 Calculate ∆Suniv for the synthesis of sulphur trioxide at 25oC 2.1.5 Calculate ∆rG at 25oC when the reaction mixture consists of 2.3 mg of S8, 3.5 bar O2 and 1.50 bar SO3. Please calculate 2.1.2
- Consider the synthesis of sulphur trioxide from its elements at 25oC:1/4 S8 (s) + 3O2(g) → 2SO3 (g) Thermodynamic Data: Species ∆fHo(kJ/mol)(at 298.15 K) So (J/K.mol)(at 298.15 K) ∆fGo (kJ/mol)(at 298.15 K) S8(s) 102 431 50 O2(g) 205 SO3 (g) -396 257 -371 2.1.1 Calculate ∆rGo , using only Gibbs energy values.2.1.2 Calculate the equilibrium constant, K, at 25oC for this reactionThe ∆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.For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction C2H6(g)+H2(g)↽−−⇀2CH4(g) the standard change in Gibbs free energy is ΔG°=−32.8 kJ/mol . What is ΔG for this reaction at 298 K when the partial pressures are PC2H6=0.500 atm , PH2=0.100 atm , and PCH4=0.800 atm ?
- Calculate the partial pressure of PCl5 at 1.00 bar total pressure and 400 K: PCl3 + Cl2 ---> PCl5 The original reaction mixture contains 1.00 mol PCl3 and 2.00 mol Cl2. Let the Gibbs free energy change be -3533 J.In this topic, the Clausius inequality was highlighted. Which of the three statements explain the importance of Clausius inequality in the discussion on determining the spontaneity of the process? It is the foundation, or basis at which the other conditions were derived. The Clausius inequality is the most general expression of the condition of spontaneity. The Clausius inequality considers simultaneously the entropy of the system under study and that of the environment or surroundings. A. Only 1 and 2 are correct. B. Only 1 is correct. C. 1, 2, and 3 are all correct. D. None of the other choices are correct. E. Only 3 is correctCalculating Thermodynamic Values from an Equilibrium ConstantBackgroundAs discussed in lecture, the free energy for a reaction can be related to the equilibriumconstant through the formula below.K = e (-ΔG° / RT)Therefore if Kc for a reaction is known, Go can be determined, or vice versa. Furthermore, ifyou have the value for Go at two different temperatures, you can calculate H and S throughthe familiar equation for Gibbs energy below, since you have two unknowns but also twoequations.G = H – T SIn this lab you will be studying the solubility of borax (Na2B4O5(OH)4*8H2O), a slightly solublesodium salt, at two different temperatures. When solid borax is added to water, theequilibrium below is established.Na2B4O5(OH)4*8H2O (s) 2 Na+ (aq) + B4O5(OH)42- (aq) + 8 H2O(l)If you measure the concentrations for those substances that show up in the reaction quotient,then the Kc for the reaction at that temperature can be calculated. In this lab, theconcentration of borate ion…
- iv) Determine the volume change ΔV for the transformation from rhombic to monoclinic sulphur.v) Estimate the pressure at which rhombic and monoclinic sulphur coexist in equilibrium at a temperature of 373 K.For the complete neutralization reaction between a 1 M strong acid and a 1 M strong base of equal initial volumes that is marked by a temperature rise, the entropy of neutralization is positive (ΔSrxn > 0) whereas the Gibbs free energy is negative (ΔGrxn < 0). Is this true or false? Please explain.Estimate the equilibrium constant for the gas-phase isomerization reaction HNC=HCN, at 1900 K using the data below (assume constant over the temperature range). delta H_f S^0 HNC +201 kJ/mol 218 J/(mol K) HCN +135 202 a.) 9.6 b.) 2.2x10^5 c.) 0.015 d.) 280 (show work please)