A)Consider these hypothetical chemical reactions: A⇌B,ΔG=A⇌B,ΔG= 13.5 kJ/molkJ/mol B⇌C,ΔG=B⇌C,ΔG= -27.6 kJ/molkJ/mol C⇌D,ΔG=C⇌D,ΔG= 9.90 kJ/molkJ/mol What is the free energy, ΔGΔGDelta G, for the overall reaction, A⇌DA⇌D?   B)Firefly luciferase is the enzyme that allows fireflies to illuminate their abdomens. Because this light generation is an ATP-requiring reaction, firefly luciferase can be used to test for the presence of ATP. In this way, luciferase can test for the presence of life. The coupled reactions are: luciferin+O2ATP⇌oxyluciferin+light ATP⇌AMP+PPi If the overall ΔGDelta G of the coupled reaction is -9.00 kJ/mol , what is the equilibrium constant, KKK, of the first reactions at 13 ∘C ? The ΔGDelta for the hydrolysis of ATP to AMP is −31.6 kJ/mol. Express your answer numerically.

Using the equation, ΔG=ΔH−TΔS, explain when will ΔG<0, ΔG>0 and ΔG=0

What is the reaction that represents ΔHf° for Al2O3 (s)?

Given the following data, what is the value of ΔGf° (CH3OH(ℓ) at 25°C?CO(g) + 2 H2(g) ⇄ CH3OH(ℓ)   K = 1.081 × 10-40ΔGf°(CO) = -137.2 kJ/mol

What is the free energy change for the reaction below, if the reaction quotient, Q, at 25.0oC is equal to 5.95e-5?5C2H2(g) + 6 H2(g) → C10H22(g) ΔGo = -1.01e3 kJ. a) ΔG = -1.036e3 kJ b) ΔG = -1.010e3 kJ c) ΔG = -1.014e3 kJ d) ΔG = 1.057e3 kJ

a) As stated in question 5a, glucose (C6H12O6(s)) is a source of cellular energy. Calculate the standard free energy for the metabolism of glucose: Given ΔG°C6H12O6(s) =  -911kJ/mol; ΔG°O2(g) = 0kJ/mol; ΔG°CO2 = -394kJ/mol; ΔG°H2O(l) = -237kJ/molC6H12O6(s) + 6O2(g) ➝ 6CO2(g) + 6H2O(l)  b) Cells couple the hydrolysis of adenosine triphosphate (ATP) into adenosine diphosphate (ADP) andinorganic phosphate (PO43–) to drive chemical reactions (i.e. as a source of chemical energy). The reaction is: ATP(aq) + H2O(l) ➝ ADP(aq) + PO43–(aq) Calculate K for this reaction if ΔG° = –30.5 kJ/mole. c) If all of the energy from glucose metabolism went into ATP synthesis from ADP and inorganicphosphate, how many molecules of ATP could be generated from each molecule of glucose?

A student determines the value of the equilibrium constant to be 2.33×1016 for the following reaction.Ca(OH)2(aq) + 2HCl(aq) ----> CaCl2(s) + 2H2O(l)Based on this value of Keq:ΔG° for this reaction is expected to be (greater, less) ____ than zero.Calculate the free energy change for the reaction of 2.34 moles of Ca(OH)2(aq) at standard conditions at 298K.ΔG°rxn = _______ kJ

How many Calories should there be in three grams of pure sucrose?A.4B. 12C. 18D. 8E. None of the above.