a. Calculate the standard Gibbs free energy change for the process of dissolution of benzene in water. b. Find the chemical potential of benzene solution standard state ΔfGo(C6H6,aq).
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A: The change in Gibbs free energy = -2808 kJ mol-1 Mass of the person = 65 kg
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a. Calculate the standard Gibbs free energy change for the process of dissolution of benzene in water.
b. Find the chemical potential of benzene solution standard state ΔfGo(C6H6,aq).
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- Actually, the carbon in CO2(g) is thermodynamically unstable with respect to the carbon in calcium carbonate(limestone). Verify this by determining the standardGibbs free energy change for the reaction of lime,CaO(s), with CO2(g) to make CaCO3(s).Determine the standard Gibbs free energy change, rG, for the reactions of liquid methanol, of CO(g), and ofethyne, C2H2(g), with oxygen gas to form gaseous carbondioxide and (if hydrogen is present) liquid water at298 K. Use your calculations to decide which of thesesubstances are kinetically stable and which are thermodynamically stable: CH3OH(), CO(g), C2H9(g), CO2(g),H2O().C6H12O6(aq) + 6O2(g) 6CO2(g) + 6H2O(l)ΔH = –2802.7 kJ mol –1a) Write an expression for the equilibrium constant for this reaction.b) At equilibrium, the concentration of the reactants and products are determined as [CO2] = 0.30 M, [O2] = 0.040 M and [C6H12O6] = 0.065 M. Determine the value of the equilibrium constant (Kc) and predict the whether the products or reactants will be favoured at equilibrium.c) Given that the concentrations of the reactants and products at a particular time are [CO2] = 0.65 M, [O2] = 0.020 M and [C6H12O6] = 0.055 M, determine the reaction quotient (Qc). Compare the Kc and Qc values and predict the favoured direction of the reaction.d) Explain the effect on equilibrium of:i) Increasing temperatureii) Increasing pressureiii) Decreasing the concentration of oxygeniv) Increasing the concentration of carbon dioxidev) Adding a catalyst
- ) Determine the standard enthalpy change and std. Gibbs free energy change of reaction at 400 k for the reaction Co(g) +2H2(g) → CH;OH (g) At 298.15 K, AH?,co (»= -26.41 kcal/mol, AH9,cH,0H(0)= -48.08 kcal/mol, AG,co ()= -32.8079 kcal/mol, AG?.cH,oH()= -38.69 kcal/mol, The standard heat capacity of various components is given by, C = a + bT + cT² + dT³, where C§ is in cal/mol-K and T is in K |Component CH;OH CO b x10 с х105 -0.291 0.1283 a d ×10" 4.55 6.726 2.186 0.04 -0.0457 -1.92 -0.5307 -0.2079 6.952 0.09563For the oxidation of iron to form iron(III) oxide: 4Fe(s) + 3O2(g) ⟷⟷ 2Fe2O3(s) ΔSo = –549.73 J∙K–1 at 298 K. The enthalpy of formation of Fe2O3(s) is –824.2 kJ∙mol–1. What is the standard change in Gibbs free energy for this reaction at 298 K? A)-660 kJ B)-1,485 kJ C)-988 kJ D)-1,812 kJAt 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 2 B(g) = C(g) + 2 D(g) were found to be PA = 4.24 atm, PB = 5.83 atm, Pc = 4.52 atm, and Pp = 4.85 atm. %3| What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ AGXN = 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 -0.2079At 25 °C, the equilibrium partial pressures for the reaction A(g) + 2B(g) = C(g) + D(g) were found to be PA = 5.66 atm, PB = 4.89 atm, Pc = 5.31 atm, and PD = 5.46 atm. What is the standard change in Gibbs free energy of this reaction at 25 °C? AGixn = kJ molThe Gibbs energy for a reaction Mg(s) + H₂O(g) → MgO(s) + H₂(g) at a particular temperature is AG = -100.0 kJ/mol. At the same time under the sa conditions, A,G° = +341 kJ/mol. Which of the following statements is true? The reaction is at equilibrium and P(H₂O) = P(H₂). The reaction proceeds in the reverse direction to produce more H₂O(g). The reaction proceeds in the forward direction to produce more H₂(g). The reaction is at equilibrium and P(H₂O) > P(H₂). The reaction is at equilibrium and P(H₂O) < P(H2).
- At 25 'C, the equilibrium partial pressures for the reaction 3 A(g) + 3 B(g) C(g) + 3 D(g) were found to be PA = 5.52 atm, P = 5.48 atm, Pe = 5.29 atm, and P, = 4.39 atm. What is the standard change in Gibbs free energy of this reaction at 25 "C? kJ AGn = molΣ II For a gaseous reaction, standard conditions are 298 K and a partial pressure of 1 atm for all species. For the reaction N,(g) + 3 H, (g) = 2 NH, (g) the standard change in Gibbs free energy is AG° = –32.8 kJ/mol. What is AG for this reaction at 298 K when the partial pressures are PN, = 0.450 atm, PH, = 0.250 atm, and PNH = 0.650 atm? kJ/mol = 9V 50:8 11/8 PrtScr Insert Delete F10 F11 F12 F7 F4 KA & Backspac 24 % 60 H. B.The standard enthalpy of combustion of the solid glycine (the amino acid, NH2CH2COOH) is −969 kJ mol−1 at 298 K and its standard molar entropy is 103.5 J K−1 mol−1. Calculate the standard Gibbs energy of formation of glycine at 298 K. Note that the nitrogen-containing species produced on combustion is taken to be N2(g).