Which of these statements concerning this reaction is true? acetaldehyde + NADH ↔ ethanol + NAD+   a)  Ethanol is more reduced than acetaldehyde.   b)  Acetaldehyde is more reduced than ethanol.   c)  NAD+ is more reduced than NADH.   d)  Ethanol is more oxidized than acetaldehyde.

Consider the following chemical equation whose delta(G) = 9kcal/mol: AC + BD ---> AB + CD    what are the reactants and what are the products  is this reaction spontaneous? How do you know?  Is energy released or consumed by this reaction?  If an enzyme, which catalyzes this reaction is added, what will happen to delta (G) If this reaction is coupled to another reaction, whose delta(G) is -12 kcal/mol, what will be the net delta(G) value? will the overall reaction be spontaneous

Carboxylic acids, such as the one shown below, can be difficult to reduce Provide the name of a reductant A. Explain why this reductant is able to react with the carboxylic acid whereas others cannot (Hint: Draw and discuss the potential reactive intermediates/transition states).

What are the expected results for the reactions: (a) CuSO4 with iron, (b) KMnO4 with ethanol, and (c) KMnO4 with acetaldehyde? Write the chemical equation of the reactions, and identify which substance is reduced and which is oxidized.

The following questions are based on the reaction A+ B ↔ C+D shown in Figure 8.1.   1. Which of the following terms best describes the progress of the reaction with respect to free energy change? a) endergonic, ∆G> 0 b) exergonic, ∆G> 0 c) exergonic, ∆G< 0 d) endergonic, ∆G< 0   2. Which of the following in Figure 8.1 remains unchanged by having an enzyme included? a) b b) d c) a       d) c   3. The part labeled “C” on the above graph represents a) Energy of activation without enzyme b) Energy of activation with enzyme c) Amount of free energy released d) amount of energy required for the reaction progress

What is the purpose of using excess alcohol in a Fischer Esterification? 1) Using excess alcohol pushes the equilibrium reaction to the left, increasing the production of isopentyl acetate via Le Chatelier's principle. 2) Using excess alcohol pushes the equilibrium reaction to the right, decreasing the production of isopentyl acetate via Le Chatelier's principle. 3) Using excess alcohol pushes the equilibrium reaction to the left, decreasing the production of isopentyl acetate via Le Chatelier's principle. 4) Using excess alcohol pushes the equilibrium reaction to the right, increasing the production of isopentyl acetate via Le Chatelier's principle.

Glyceraldehyde-3-phosphate (GAP) is converted to 1,3-bisphosphoglycerate (1,3-BPG) as shown. GAP + P + NAD+ 1,3-BPG + NADH Is this reaction spontaneous? How do you know? AG = 6.7 kJ mol-¹ The reaction shown above is coupled to the following reaction in which 1,3-BPG is converted to 3-phosphoglycerate (3-PG): GAP + P + NAD+ + ADP3-PG + NADH + ATP AG = -18.8 kJ mol-¹ 1,3-BPG+ADP3-PG+ATP Write the equation for the overall conversion of GAP to 3PG. Is the coupled reaction favorable? How do you know?