Calculate the standard free energy change (ΔG°') for the reaction catalyzed by the enzyme aspartate amino transferase (K'eq = 6.8) using the given equilibrium constant for the reactions at 25°C and pH 7.0.

A student determines the value of the equilibrium constant to be 2.22x10 2 for the following reaction. CH (g) + H,O(g) →3H2(g) + CO(g) Based on this value of Keg AG° for this reaction is expected to be (greater, less) than zero. Calculate the free energy change for the reaction of 2.05 moles of CH,(g) at standard conditions at 298K. AG°. Ixn kJ

In glycolysis, glucose is broken down to yield energy. If the equilibrium constant of the isomerization of glucose-6-phosphate to fructose-6-phosphate is 0.5, would this reaction proceed in the forward or reverse direction? What is the free energy of the reaction? Using standard conditions (1 M) as an initial state, what are the equilibrium concentrations?

6) If we represent protein folding with the following equilibrium expression: Unfolded protein z folded protein The values of AH and AS° for the folding of lysozyme protein are -280 kJ/mol and -790 J/mol-K, respectively. a) Based on these values, calculate AG° for the folding process at 25 °C. b) At what temperature would you expect the unfolding process to become unfavorable?

Cl₂ is a stable diatomic molecule. It can be decomposed to form two CI atoms as shown below. Cl₂ → 2Cl(g) Predict the change in free energy (AG) of this reaction. A) AG is (-); endergonic B) AG is (+); endergonic C) AG is (-); exergonic D) AG is (+); exergonic E) AG is dependent upon the temperature of the reaction

Nitesh

The oxidation of glucose 1C6H12O62 in body tissue produces CO2 and H2O. In contrast, anaerobic decomposition, which occurs during fermentation, produces ethanol 1C2H5OH2 and CO2. (a) Using data given in Appendix C,compare the equilibrium constants for the following reactions:C6H12O61s2 + 6 O21g2 ∆ 6 CO21g2 + 6 H2O1l2C6H12O61s2 ∆ 2 C2H5OH1l2 + 2 CO21g2

A student determines the value of the equilibrium constant to be 1.39x1025 for the following reaction. 2502(g) + O2(8)2S03(g) Based on this value of Keg: AG° for this reaction is expected to be (greater,less) than zero. Calculate the free energy change for the reaction of 1.84 moles of SO2(g) at standard conditions at 298K. AG° rxn kJ

A student determines the value of the equilibrium constant to be 5.14×1091 for the following reaction.H2CO(g) + O2(g)CO2(g) + H2O(l)Based on this value of Keq:G° for this reaction is expected to be (greater, less) fill in the blank 1 than zero.Calculate the free energy change for the reaction of 2.29 moles of H2CO(g) at standard conditions at 298K.    G°rxn = ____________  kJ

The combustion of hydrazine, N₂H4(1), with O₂(g) produces N₂(g) and H₂O(g). Using free energies of formation, what is AG (in kJ) for hydrazine?