From the Catalyst University video in Lesson 3D, we learned that an integrated form of the Gibbs-Helmholtz equation can be written AG(T₂) AG(T₂) 1 1 #* (T) (7-7) T + AH*(T₂) 1 If AH° (280 K) = -25 kJ and AG (280 K) = 15 kJ at what temperature would the change in Gibbs energy vanish, that is, at what value of T does AG (7)=0? This represents an equilibrium condition. Report the temperature in K.
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- For the reaction X(g) + 2Y(g) = 3Z(g) K, = 2.08x10-2 at a temperature of 325 °C. Calculate the value of Kc . Express your answer numerically. View Available Hint(s) V ΑΣφ K = %3D2 When 50 cm' of hydrochloric acid of concentration 2.0 mol dm is added to 50 cm' of sodium hydroxide solution of concentration 2.0mol dm, the temperature increase is 13.0°C HCl(aq) + NAOH(aq) + NaCl(aq) + H,O(1) The experiment is repeated using 25 cm of the same hydrochloric acid and 50 cm' of the same sodium hydroxide solution. What is the temperature increase? O A 4.9°C I B 6.5°C I C 8.7°C D 13.0°Cthe following thermesdyna mic and partial prassuce data, detormine the Gibbs Energy (AG) for the reaction : Give 2 PeO cg) Clz cq> 2 2 Pe OCI (9) at 298 k in kJ /mol substance AG (KJ/ncol ) P (bar) Pe O cg> - 220.4 0.40 ch (q? Information is missing 0.17 PeOckgs 420.4 0.59
- Calcule el potencial estándar de la media reacción: HgS(s) + 2 H* (aq) + 2 e --> Hg() + H2S(g) si para la celda a continuación: Cd [Cd2*(1 M) || HgS(s) H* (1 M)| Hg() | H2S(1 atm)| Pt E°celda= -0.317 V y E° (Cd2+/Cd)= -0.403 V E° (HgS/Hg)= ? Seleccione una: a. 0.400 V b. 0.086 V O c. 0.720 V d. -.086 V e. -0.720 V(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 solid99. Which one of the following expressions represents in Gibbs Helmholtz equation? a) AG=AH+T (37) p b) _4,H= 4,G - T (8(476)) A)` c) 4,4 = 4₁U+p(0 (47¹) P
- If you apply the Gibbs-Duhem equation to an ideal 2 component solution, which of the following expressions can you derive (which expression is correct for an ideal 2 component system)? Hint: the chemical potential for an ideal solution is defined as 4 = u, + RT In aj. In z O P () dz=-P; ( dzz aln a ata P O P: () dzi = -P; () daa -) dri = -r2 a In P 8 In P dz2 dri = -22 O Pi dz; = -P ( dzy 8 in P a In P OR () dz = -P () dz zGive the conditions under which each of the following equations may be applied. (a) dA ≤ 0 (for equilibrium and spontaneity) (b) dG ≤ 0 (for equilibrium and spontaneity) P2 _ ΔΗ (Τ, - Τ) (c) In P₁ = R T₁T₂ (d) AG = nRT In P₂ P₁Calculate the standard Gibbs reaction energy for the reaction at 298 K, 2CH3CHO(g) + O2(g) - > 2CH3 COOH(I) Given the following data, Sm\deg (CH3CHO(g )) = 250.30 J K-1 mol-1 Sm\deg (O2(g)) = 205.10 JK -1 mol-1 Sm\deg (CH3COOH(l))=159.80~K-1~mol-1\backslash Delta fHm\deg (CH3CHO(g))=-166.20~kJ~mol-1\backslash Delta fHm\deg (O2(g)) = 0.00 kJ mol-1 \Delta fHm\ deg (CH3COOH(I)) = 484.50 kJ mol-1
- Consider the following reaction: CO₂ (g) + CCl4 (9) ≈ 2COCl₂ (g). Calculate AG for this reaction at 125 °C under the following conditions. Part A Pco₂ = 0.135 bar PCC₁ = 0.185 bar Pcocl₂ = 0.760 bar AFG= Submit VO —| ΑΣΦ Request Answer ? kJ mol-1the 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 S In 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 (B4O5(OH)42-) in solution will be measured by titration with standardhydrochloric acid…4. 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…