Use the following information (T = 37°C) ADP + H2O ATP + H2O AMP + Pi + H+ AG°=-35.7 kJ/mol ADP + Pi + H+ = AGO -30.5 kJ/mol What is the AG' for the following reaction? AMP + ATP <--- 2ADP Type your answer...

Find AH°, for the reaction rxn 2Na(s) + 2H20(1) → 2NaOH(aq) + 2H2(g). [AH°t (NaOH(aq)) = -426.8 kJ/mol; AH°t (H2O(1)) = -285.5 kJ/mol] -284.6 kJ -282.6 kJ -280.6 kJ O-278.6 kJ

The hydrolysis of ATP to form ADP requires energy to break the bonds initially, but releases moreenergy as bond are remade making the reaction exothermic overall. The Gibbs free energy for thisreaction is -30.5 kJ/mole, meaning that it is also exergonic (ΔG=-). This energy can be used by otherbiological systems if this reaction is coupled with another less favorable one. In this case, the creation ofglucose-6-phosphate, C6H10O9P, this is a pivotal intermediate in many biochemical pathways. PO43- + C6H12O6 ⇌ H2O + C6H10O9P           ΔG° = +13.8 kJ/moleATP + H2O ⇌ ADP + PO43-                            ΔG° = -30.5 kJ/mole A) What is the overall reaction that takes place? B) Calculate the ΔG° for this reaction C) Will this be a successful coupled reaction?

23 Use the following information to answer the next question. 4 Q(9) +2₂(B) + 100.0 kJ → 2 QzZ(6) The AH value for the reverse reaction would be A. -100.0 kJ B. -50.0 kJ C. +50,0 kJ D. +100.0 kJ AH = + 100.0 KJ

The conversion of glucose (C,H12O6) into lactic acid (2CH3CH(OH)COOH) drives the phosphorylation of 2 moles of ADP to ATP and has a AG° = -135 kJ/mol. CH,0,(aq) + 2HPO? (aq) + 2ADP³3- (aq) +2H*(aq) –→ 2CH,CH(OH)COOH(aq) +2ATPª¯(ag) + 2H,0(1) The conversion of ATP to ADP has a AG° = -30.5 kJ/mol. ATP4 (ag)+H,0(1) –→ ADP³-(aq) + HPO? (aq) + H*(aq) 1st attempt See Periodic Tabl O See Hint What is AG° for the conversion of glucose into lactic acid? CH1206(aq) → 2CH,CH(OH)COOH(aq) A SUBMIT ANSWER

5. Using given information, calculate AG of this reaction at 37°C ATP"+H,O 6, 5.6, 5.6 mM, respectively, 2- ADP*+HPO,+H¨ The concentrations of ATP", ADP , HPO, , H¨ are 8, 4 4 Given: ATP"+H,O ADP'+HPO, AG," = -41.0kJ/mol ² 2- 3- '0 ADP ADP +H" AG," = -20 kJ/mol 2

Which of the reactions are spontaneous (favorable)? DHAP = glyceraldehyde-3-phosphate AG = 3.8 kJ/mol L-malate + NAD+ → oxaloacetate + NADH + H+ AG = 29.7 kJ/mol C,H¸O; C,H,O, + H,0 AG= 3.1 kJ/mol Rh(I) C,H, + H, C,H, AG = -150.97 kJ/mol C,H1,0,P O̟P + ATP C,H14012P2 + ADP AG = -14.2 kJ/mol glutamate + NAD+ + H,O → NH† + a-ketoglutarate + NADH + H* AG = 3.7 kcal/mol

18) What is AH°, for the following reaction? 18) rxn 2H2O2(1) → 2H2O(1) + O2(g) AH°f(H2O(1)) =-285.8 kJ/mol, AH°f(H2O2(1)) =-187.6 kJ/mol A) 98.2 kJ/mol B) -946.8 kJ/mol C) –196.4 kJ/mol D) –473.4 kJ/mol E) -98.2 kJ/mol

13. Calculate AH for the reaction NO + Og) O NO2(8) Given the following information: As part of your answer, show how the equations can be added together to give the overall or net equation. + Oig) AH = -427 Kj AH = +495 Kj %3D 203(e) O 302(3) Ozle) O 20) + O318) (g) AH = -199 Kj NOe) + O3(2) O NO218) + O213)

at 25oC, Ka for aspirin (C9H8O4) is 3.0 x 10-4.  Calculate Δ Go (kJ/mol) for the reaction:            C9H8O4(aq)  +  H2O(l)  =  H3O+(aq)  +  C9H7O4-(aq)