Consider the interconversion shown, which occurs in glycolysis. Fructose 6-phosphate glucose 6-phosphate The equilibrium constant, K'eq, is 1.97 at 25.0 °C. Calculate AG'° for the reaction. AG" = kJ/ma If the concentration of fructose 6-phosphate is adjusted to 1.5 M and that of glucose 6-phosphate is adjusted to 0.50 M, what is AG? AG = kJ/ma

A healthful diet should have a distribution of macronutrients. In the following, match the caloric content with a healthful diet's macronutrients.     Protein Fats Carbohydrates   highest caloric content intermediate caloric content lowest caloric content

The reaction of gaseous H2H2 and liquid Br2Br2 to give gaseous HBrHBr has ΔHΔH = -17.4 kcal/molkcal/mol (-72.8 kJ/molkJ/mol) and ΔSΔS = 27.2 (cal/mol⋅K)(cal/mol⋅K) (114 J/(mol⋅K)J/(mol⋅K)). What is the value of ΔGΔG (in kcalkcal and kJkJ) for the reaction at 280 KK ?         Enter your answers numerically separated by a comma.

Many metabolites are maintained at steady-state concentrations that are far from equilibrium. A comparison of Keg and Q, the mass-action ratio, can determine whether a metabolic reaction is far from equilibrium. The equation for this equilibrium is, fructose 6-phosphate + ATP = fructose 1,6-bisphosphate + ADP Calculate Keg for this reaction at T = 25.0 °C. AG' = -14.2 kJ/mol Keg = Calculate the mass-action ratio, Q, from the approximate physiological concentrations for rat heart tissue shown in the table. Metabolite Concentration (µM) fructose 6-phosphate 82.0 Q = fructose 1,6-bisphosphate 31.0 АТР 12,900 ADP 1,390

Which aqueous solution has the highest ΔTf value? Kf = 0.51 °C m-1.   ​​​a.​0.200 m KCl(aq) ​​​​ ​​​b.  0.200 m C3H8O3 (aq), glycerol

What is the AH for the following reaction: IF5 (8)→ IF 3 (g) + F₂ (g) Given: IF (g) + F2 (g) → IF 3 (g) IF (g) + 2F2 (g) → IFs (g) +1135 kJ -35 kJ +355 kJ -1135 kJ +35 kJ ΔΗ = -390 kJ ΔΗ = -745 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

Formation of glycerol 3-phosphate is a model reaction for many metabolic processes. The ΔG˚’ for phosphorylating glycerol is +9.2 kJ/mol. Calculate the equilibrium constant for the phosphorylation of glycerol.

Using the following equations, N,0(g)– 2NO2(g) AH° = +57.93 kJ 2NO(g) + O(g) 2NO,(g) AH° = -113.14 kJ %3D calculate the AH° for the following reaction: 2NO(g) + O2(g)– N,0,(g) AH° = kJ

QUESTION 1 Consider the formation of a dimeric protein below. 2P → P2 AH° = 17.0 kJ/mol and AS° = 65.0 J/Kmol This reaction is spontaneous at body temperature (37 °C). Calculate the temperature (in units of °C) below which it becomes nonspontaneous. Enter a numeric answer with the correct sign and no units.