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- Another step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.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().Calculate (a) the standard reaction entropy and (b) the change in entropyof the surroundings (at 298 K) of the reaction N2(g) + 3 H2(g) → 2 NH3(g). (c) Hence calculate the standard Gibbs energy of the reaction.
- In a particular biological reaction taking place in the body at 37 °c, the change in enthalpy was -135 kJ mol-1 and the change in entropy was - 136 J K-1 mol-1. (a) Calculate the change in Gibbs energy. (b) Is the reaction spontaneous? (c) Calculate the total change in entropy of the system and thesurroundings.In a particular biokgikal reaction taking place in the body at 37 C, the change in enthalpy was -125 kJ mol' and the change in entropy was -126 JK' mol". (a) Cakulate the change in Gibbs energy. (b) Is the reaction spontaneous? (e) Cakulate the total change in entropy of the system and the surroundings.At 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 4 B(g)=2C(g)+D(g) were found to be PA = 4.74 bar, Pg 5.52 bar, Pc = 4.94 bar, and Pp 5.78 bar. What is the standard change in Gibbs free energy of this reaction at 25 °C? ?
- 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…At 25 °C, the equilibrium partial pressures for the reaction 2 A(g) + 2 B(g) = C(g) + 3 D(g) were found to be PA = 4.41 bar, PB 5.54 bar, Pc = 4.92 bar, and P, = 5.18 bar. What is the standard change in Gibbs free energy of this reaction at 25 °C? kJ/molThe decomposition of a generic diatomic element in its standard state is represented by the equation X2(g) → X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 5.17 kJ mol¹ at 2000. K and -50.69 kJ mol¹ at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG = 5.17 kJ mol-1. What is K at that temperature? K at 2000. K = At 3000. K, AG = -50.69 kJ mol-1. What is K at that temperature? K at 3000. K =
- The reduction of iron(III) oxide (Fe2O3) to pure iron during the first step of steelmaking, 2 Fe2O3(s) 4 Fe(s) + 302 (g) is driven by the high-temperature combustion of coke, a purified form of coal: C(s) + 0,(g) → CO₂ (g) Suppose at the temperature of a blast furnace the Gibbs free energies of formation AG, of CO2 and Fe2O3 are -412. kJ/mol and -836. kJ/mol, respectively. Calculate the minimum mass of coke needed to produce 470. t of pure iron. (One metric ton, symbol t, equals 1000-kg.) Round your answer to 2 significant digits. kg x10The decomposition of a generic diatomic element in its standard state is represented by the equation X,(g) → X(g) Assume that the standard molar Gibbs energy of formation of X(g) is 4.94 kJ - mol-1 at 2000. K and -62.81 kJ mol at 3000. K. Determine the value of the thermodynamic equilibrium constant, K, at each temperature. At 2000. K, AG = 4.94 kJ mol. What is K at that temperature? K at 2000. K = At 3000. K, AG = -62.81 kJ - mol. What is K at that temperature? K at 3000. K =Calculate 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