99. Which one of the following expressions represents in Gibbs Helmholtz equation? a) A,G=A₂H + T P b) _4,H = 4,G – T (3(4,-6)), P c) 4,4 = 4,U+p(0 (474)
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- Chose the correct option that represents the change in Gibbs free er (A) dG =µdn, (B) dG =Eµn, (C) dG =-Eudn (D) dG =µ dn,At 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 = mol6) Calculate the final temperature of a sample of carbon dioxide of mass 16.0 g that is expanded reversibly and adiabatically from 500 cm³ at 298.15 K to 2.00 dm³.
- 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 catalystAt 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 2.1At 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 5.61 atm, PB = 4.31 atm, Pc = 5.66 atm, and P = 5.84 a %3D %3D What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ AGixn mol
- What is AG for the decomposition of CaCO3 at 298 K and a partial pressure of CO2 of 4.00x10-4 bar? CaCO3(s) → CaO(s) + CO2(g) AGrxn (298 K, Pco2 = 0.400 mbar) = ??? CO2(g) Compound AG°; (kJ mol·1) CACO3(s) СаО(s) -1129 -604 -394At 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 = 4.25 atm, Pg = 5.05 atm, Pc = 4.13 atm, and Pp 4.94 atm. %3D What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ mol4. The reaction of metallic cobalt (Co) with oxygen can be described by Co(s) + O2 CoO(s) in which the label (s) indicates reactants and products in a solid form. The Gibbs energy change for this reaction at oxygen pressure po, = latm is given by the expression, kJ AG (T) = -500.8- kJ =)T molK mol + (0.164- in which T is the temperature in kelvin. This energy change is per mole of O2 consumed. You might refer to the Ellingham diagram discussed in class and included in the lecture slides to see if the numbers seem to match the plot for that particular reaction. a) Recall that AG = AH - TAS, and that AH and AS only display a weak temperature dependence. Compare to the above equation for AG, What does that tell you about the sign of AS for the reaction? Is it positive or negative? Explain why the sign makes sense for that particular reaction, and also note the slope of this reaction in the Ellingham diagram. Is it consistent? Note that the slopes in the Ellingham diagram relate to the…
- Chose the correct option that represents the change in Gibbs free energy. (A) dG =Eµdn, (B) dG =£un (C) dG =-Eµdn, i (D) dG =µ> dn,At 25 °C, the equilibrium partial pressures for the reaction 3 A(g) + 4B(g) 2 C(g) + 3D(g) were found to be PA = 4.71 atm, PB = 4.26 atm, Pc = 5.75 atm, and P = 4.58 atm. What is the standard change in Gibbs free energy of this reaction at 25 °C? AGrxn = kJ mol5) Starting from the expression Cp – G, = T (P/ər), (V/ar). ' use the appropriate relations between partial derivatives to show that T(V/ar), Cp – Cy =