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Calculate the free energy change for the following reaction at 25°C. 4 CuO(8) + CH4(g) 4...
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7. Consider: 4 Cuo(s) + CH4(g) + CO2(g) +4 Cu(s) + 2 H2O(g). The value of Kc for this reaction is 1.10 at 25°C. What is the value of K, ?
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Thermodynamics Gibbs Free energy Calculate Gibbs free energy for reaction of urea hydrolysis CO(NH2)2(aq) + H2O(0) = CO2(g) + NH3(e) From standard enthalpy and entropy data: AH° = 119 kJ AS9 = 354.8 J/K = 0.3578 kJ/K T = 25°C = 298°K AG = AH° – TYAS°
Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Refer to the AGⓇ values. 3 H2(g) + Fe, 0,(s) 2 Fe(s) + 3 H2O(g) AG" Calculate the standard change in Gibbs free energy for the reaction at 25 °C. Standard Gibbs free energy of formation values can be found in this table. C,H,(8) +4 C1,() 2 CCI, (1) + H2(g) AGE. kJ/mol
Calculate the standard free energy change at 25°C for the reaction 2 NO(g) + O2(g) → 2 NO2(g). Species ΔH°f, kJ/mol S°, J/(K · mol) NO (g) 91.3 210.7 O2 (g) 0.0 205.0 NO2 (g) 33.2 240.0 A) -157.8 kJ B) -532.6 kJ C) -72.6 kJ D) -4.7 kJ
Consider the following reaction and its equilibrium constant: 4 CuO(s) + CH4(g) ⇌ CO2(g) + 4 Cu(s) + 2 H2O(g) Kc = 1.10 A reaction mixture contains 0.38 M CH4, 0.96 M CO2 and 0.14 M H2O. Which of the following statements is TRUE concerning this system? The system is at equilibrium. The reaction will shift in the direction of reactants. The reaction quotient will increase. The equilibrium constant will increase. The reaction will shift in the direction of products.
Calculate the change in Gibbs free energy at standard conditions (TSS) and the equilibrium constant for each of the following reactions. (a) CH4(g) + H2O(g) equilibrium reaction arrow CO(g) + 3 H2(g); ?H° = +205.9 kJ, ?S° = +214.7 J/K ?G° 141.9 Correct: Your answer is correct. kJ K (b) CaCO3(s) equilibrium reaction arrow CaO(s) + CO2(g); ?H° = +179.2 kJ, ?S° = +160.2 J/K ?G° 131.5 Correct: Your answer is correct. kJ K
23. Question (1 point) W Calculate the free-energy change of the following reaction at 221°C: C2H(g) +302(g) → 2002(g) + 2H20(g) A Hºt, kJ/mol 52.3 Sº, J/mol K 219.5 C2H4(g) O₂(g) CO2(g) H2O(g) -393.5 205.0 213.6 188.7 -241.8 1st attempt
3) Calculate the standard free energy change (Go ) at 25 C for C (s) + O2 (g) ----- > CO2 (g) For which the value of Ho = -393.51 KJ/mol And the value for So = 2.83 J/mol K
Calculate standard free energy change using AHp and So values. Consider the reaction 2NH3(8) + 3N20(g)—__4N2(g) + 3H2O(g) Calculate the standard free energy change for this reaction at 25°C from AH°rxn and AS°rxn- AGºrxn = kJ/mol
Pi T2 = P₂ T 12) Calculate the standard free energy change at 25°C for the reaction 2 NO(g) + O2(g) → 2 NO2(g). 12 46°E AH-TAS Species | AHºf, kJ/mol NO () 91.3 02 (8) 0.0 NO2 (8) 5, J/(K.mol) 210.7 205.0 240.0 33.2 A) -4.7 kJ (B) -72.6 kJ C) -157.8 kJ D) -532.6 kJ 13) The Boltzmann formula is S=k In W. A perfect crystal has a molar entropy of 0 at absolute zero because A) W=NA...