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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 the standard Gibbs free energy change, ∆Gorxn, for the following reaction at 25.0oC: Ca3(PO4)2(s) → 3Ca2+(aq) + 2PO43– (aq), Ksp = 2.07×10–33 Calculate it with correct units and significant figures.
- Using the thermodynamic information, calculate the standard rection free energy of the following chemical reaction: N2(g)+O2(g) ---> 2NO(g) Round to zero decimal placesCalculate the free energy change that occurs when a reaction has an enthalpy of −315.2 kJ mol−1 and an entropy change of 224.7 J mol−1 K−1 at 211.3 ∘C. What is the equilibrium constant for this reaction at this temperature? Will that constant increase or decrease as the temperature is increased?Calculate the standard Gibbs free energy of the reaction, ΔG∘rxn. The standard enthalpy of the reaction, ΔH∘rxn, is −44.2 kJ⋅mol−1. C2H4(g)= 68.4 H2O(l)= -237.1 C2H5OH(l)= -166.6
- Calculate the standard Gibbs free energy in kJ mol–1.If Gibbs free energy (at standard conditions) of a reaction is -22.8 kj/mol, what is the equilibrium constant of the reaction?The acid dissociation constant for a weak acid HX at 25°C is 1.9 10–6. Calculate the free energy of formation for X–(aq) at 25°C. The standard free energies of HX(aq) and H+(aq) at 25°C are –245.4 kJ/mol and 0, respectively.
- Use the thermodynamic data below to answer the following questions regarding this chemical reaction: CH4(g) + H2O(g) ® 3 H2(g) + CO(g) DfG° [CH4(g)] = –50.8 kJ/mol, DfG° [H2O(g)] = –228.6 kJ/mol, DfG° [H2(g)] = 0.0 kJ/mol, and DfG° [CO(g)] = –137.2 kJ/mol; Calculate the standard net Gibbs free energy change for the reaction as written. 2. Calculate the equilibrium constant in terms of Kp and Kc. (Note: DfG°’s given above relate to Kp, not Kc. (R = 8.314 J/mol K = 0.08206 L atm/mol K) 3. Estimate the mol fraction of carbon monoxide (CO) at equilibrium?A reaction has a standard free‑energy change of −18.20 kJ (−4.350 kcal mol−1). Calculate the equilibrium constant for the reaction at 25 °C. Keq =What is the relationship between the standard free energy change and the equilibrium constant of the reaction?