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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
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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 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
Transcribed Image Text: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
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