Exam 3: The Energetics of Life

Calculate the $\Delta$ G ^$\circ$ 'for the oxidation of succinate to fumarate, a step in the citric acid cycle. FAD + 2H⁺ + 2e^- $\rarr$ FADH₂ E ^$\circ$ ' = - 0.22 V fumarate + 2H⁺ + 2e^- $\rarr$ succinate E ^$\circ$ ' = + 0.03 V

Which of the following conditions will produce a non-spontaneous reaction?

In the study of thermodynamics, which of the following could be examined as a system?

Based on the half reactions given below, which of the following reactants is the strongest reducing agent?

Which of the following represents an apparent violation of the second law of thermodynamics?

Which of the following is true regarding a spontaneous reaction?

Which of the following best describes the relationship between the oxidation of glucose in a cell versus the oxidation of glucose in a bomb calorimeter?

The biochemical standard state differs from standard state conditions in what way?

In a resting muscle cell at 37 ^$\circ$ C, what is the $\Delta$ G for the phosphorylation of ADP by creatine phosphate (CP)given the following concentrations: CP, 25 mM; ATP, 5 mM; ADP, 0.1 mM and creatine, 1 mM? creatine phosphate + H₂O $\rarr$ creatine + P_i $\Delta$ G ^$\circ$ ' = -43.1 kJ/mol ATP + H₂O $\rarr$ ADP + P_i $\Delta$ G ^$\circ$ ' = -30.5 kJ/mol

Which of the following compounds contains a phosphate ester as its most energetically labile bond?

Which of the following best describes biochemical systems with respect to the first law of thermodynamics?

Which of the following correctly relates the relative entropies?

What is the E ^$\circ$ ' for the spontaneous reaction that would result if the following reactions were coupled? NAD⁺ + H⁺ + 2e^- $\rarr$ NADH E ^$\circ$ ' = -0.32 V Pyruvate + 2H⁺ + 2e^- $\rarr$ 0 lactate E ^$\circ$ ' = -0.19 V

Which of the following would be considered a closed system?

The typical concentration of glucose-6-phosphate (G6P)in a cell is 1 mM. What concentration of glucose-1-phosphate (G1P)would be required to make the interconversion of G6P and G1P freely reversible at 37 ^$\circ$ C? G1P + H₂O $\rarr$ glucose + P_i $\Delta$ G ^$\circ$ ' = -20.9 kJ/mol G6P + H₂O $\rarr$ glucose + P_i $\Delta$ G ^$\circ$ = -13.8 kJ/mol

The formation of glucose-1-phosphate from glucose and orthophosphate has a $\Delta$ G ^$\circ$ ' of + 20.9 kJ/mol. If this reaction were coupled to another reaction in order to produce an exergonic reaction, which of the following would produce an overall endergonic reaction and therefore not be suitable for coupling?

If acetyl phosphate is made from the combination of ATP and acetate, what is the $\Delta$ G ^$\circ$ '? How would this reaction proceed within a typical cell? acetyl phosphate + H₂O $\rarr$ acetate + P_i + H⁺ $\Delta$ G ^$\circ$ '= -43.1 kJ/mol ATP + H₂O $\rarr$ ADP + P_i + H⁺ $\Delta$ G ^$\circ$ ' = -30.5 kJ/mol

The conversion of glucose-6-phosphate to fructose-6-phosphate has a $\Delta$ G°´ of +1.7 kJ/mol but within a typical cell, the $\Delta$ G is -2.9 kJ/mol. What can be said about the value of K_eq and Q?

The highly exergonic nature of ATP hydrolysis is explained by which of the following?

If the $\Delta$ G ^$\circ$ ' for ATP hydrolysis is -31 kJ/mol and the $\Delta$ G ^$\circ$ ' for phosphoenolpyruvate hydrolysis is -62 kJ/mol, what is the $\Delta$ G ^$\circ$ ' for the phosphorylation of ADP by phosphoenolpyruvate?