Which of the reactions are spontaneous (favorable)?DHAP = glyceraldehyde-3-phosphate AG = 3.8 kJ/molL-malate + NAD+→ oxaloacetate + NADH + H+AG = 29.7 kJ/molC,H¸O;C,H,O, + H,0 AG= 3.1 kJ/molRh(I)C,H, + H,C,H, AG = -150.97 kJ/molC,H1,0,PO̟P + ATPC,H14012P2 + ADPAG = -14.2 kJ/molglutamate + NAD+ + H,O → NH† + a-ketoglutarate + NADH + H*AG = 3.7 kcal/mol

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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 O C,H,O5 C,H,O, + H,0 AG= 3.1 kJ/mol Rh(I) O C,H, + H2 C,H. AG = -150.97 kJ/mol O C,H130,P + ATP C,H4012P, + ADP AG = –14.2 kJ/mol 12 2 O glutamate + NAD+ + H,O – NH + a-ketoglutarate + NADH + H* AG = 3.7 kcal/mol

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 O C,H,O5 C,H,O, + H,0 AG= 3.1 kJ/mol Rh(I) O C,H, + H2 C,H. AG = -150.97 kJ/mol O C,H130,P + ATP C,H4012P, + ADP AG = –14.2 kJ/mol 12 2 O glutamate + NAD+ + H,O – NH + a-ketoglutarate + NADH + H* AG = 3.7 kcal/mol

Chemistry & Chemical Reactivity

9th Edition

ISBN:9781133949640

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions

Section5.5: Enthalpy Changes For Chemical Reactions

Problem 1RC: 1. For the reaction 2 Hg(l) + O2(g) → 2 HgO(s), ∆rH° = 181.6 kJ/mol-rxn. What is the enthalpy change...

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