SnO2 (s)+2CO (g) →Sn (s, white) + 2CO2 (g) Round your answer to zero decimal places. tab, calculate the standard reaction free energy of the following chemica OkJ x10

One of the important reactions in the biochemical pathway glycolysis is the reaction of glucose-6-phosphate (G6P) to form fructose-6-phosphate (F6P): G6PF6PG298=1.7kJ (a) Is the reaction spontaneous or nonspontaneous under standard thermodynamic conditions?. (b) Standard thermodynamic conditions imply the concentrations of G6P and F6P to be 1 M, however, in a typical cell, they are not even Close to these values. Calculate G when the concentrations of G6P and F6P are 120 M and 28 M respectively, and discuss the spontaneity of the forward reaction under these conditions. Assume the temperature is 37 C.

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.

Yeast can produce ethanol by the fermentation of glucose (C6H12O6), which is the basis for the production of most alcoholic beverages. C6H12O6(aq) 2 C2H5OH() + 2 CO2(g) Calculate rH, rS, and rG for the reaction at 25 C. Is the reaction product- or reactant-favored at equilibrium? In addition to the thermodynamic values in Appendix L, you will need the following data for C6H12O6(aq): fH = 1260.0 kl/mol; S = 289 J/K mol; and fG = 918.8 kl/mol.

Using values of fH and S, calculate rG for each of the following reactions at 25 C. (a) 2 Na(s) + 2 H2O() 2 NaOH(aq) + H2(g) (b) 6 C(graphite) + 3 H2(g) C6H6() Which of these reactions is (are) predicted to be product-favored at equilibrium? Are the reactions enthalpy- or entropy-driven?

Predict whether each reaction is reactant-favored or product-favored at 298 K and 1 bar, and calculate the minimum work that would have to be done to force it to occur, or the maximum work that could be done by the reaction. (a) 2 CO2(g) 2 CO(g) + O2(g) (b) 4 Fe(s) + 3 O2(g) 2 Fe2O3(s)

Without looking up their standard entropies in reference tables, identify which of the following lists the materials in order of increasing entropy. (a) H2O() NaCl(s) NH3(g) (b) H2O() NH3(g) NaCl(s) (c) NaCl(s) H2O() NH3(g) (d) NH3(g) H2O() NaCl(s)

a Calculate K1, at 25C for sulfurous acid: H2SO3(aq)H+(aq)+HSO3(aq) b Which thermodynamic factor is the most significant in accounting for the fact that sulfurous acid is a weak acid? Why?

Using values of fH and S, calculate the standard molar free energy of formation, fG, for each of the following compounds: (a) CS2(g) (b) NaOH(s) (c) ICl(g) Compare your calculated values of fG with those listed in Appendix L Which of these formation reactions are predicted to be product-favored at equilibrium at 25 C?

For the reaction NO(g)+NO2(g)N2O3(g) , use tabulated thermodynamic data to calculate H and S. Then use those values to answer the following questions. (a) Is this reaction spontaneous at 25°C? Explain your answer. (b) If the reaction is not spontaneous at 25°C, will it become spontaneous at higher temperatures or lower temperatures? (c) To show that your prediction is accurate, choose a temperature that corresponds to your prediction in part (b) and calculate G . (Assume that both enthalpy and entropy are independent of temperature.)