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Chapter 2: Physical Biochemistry: Energy Conversion, Water, and Membranes
Learning Objectives
2.1 Energy Conversion in Biological Systems 2.2 Water Is Critical for Life Processes
2.1.a. Describe how sunlight is the source of all energy on 2.2.a. Identify hydrogen bond donors and hydrogen bond
Earth. acceptors.
2.1.b. Differentiate between autotrophs and heterotrophs. 2.2.b. Describe how an antifreeze protein functions.
2.1.c. Explain the role of oxidation-reduction reactions in 2.2.c. Differentiate among hydrogen bonds, ionic
biological systems. interactions, and van der Waals interactions.
2.1.d. Differentiate between a system and its surroundings. 2.2.d. State the concept of the hydrophobic effect and how
it impacts protein folding.
2.1.e. Differentiate among open, closed, and isolated
systems. 2.2.e. Explain the impacts of hypotonic, isotonic, and
hypertonic solutions on cells.
2.1.f. Explain the first law of thermodynamics as it applies
to biological systems. 2.2.f. Identify the important aspects of plant, fungi, and
bacterial cells that allow them to survive in a hypotonic
2.1.g. Differentiate between endothermic and exothermic environment.
reactions.
2.2.g. Calculate the concentration of H+ or OH– given the
2.1.h. State the second law of thermodynamics as it applies OH– or H+ concentration.
to biological systems.
2.2.h. Relate pH to the concentration of H+ or OH–.
2.1.i. Explain the concept of entropy and its role in
biological systems. 2.2.i. Differentiate between weak acids and strong acids
and between weak bases and strong bases.
2.1.j. Define Gibbs free energy, its relation to enthalpy and
entropy, and its relation to equilibrium. 2.2.j. Relate pH to pKa using the Henderson-Hasselbalch
equation.
2.1.k. Identify the impacts of enthalpy, entropy, and
temperature on free energy. 2.3 Cell Membranes Function as Selective Hydrophobic
Barriers
2.1.l. Differentiate between standard state condition and the
biochemical standard state. 2.3.a. Identify the characteristics of a phospholipid that
contribute to membrane formation.
2.1.m. Differentiate between exergonic and endergonic
reactions and explain how such reactions are coupled in 2.3.b. Relate the degree of saturation in phospholipids to
biological systems. the fluidity of the membrane.
2.1.n. Identify the characteristics of the ATP molecule 2.3.c. Explain the various ways cholesterol impacts
that provide such a large standard free energy change for membrane structure.
phosphoanhydride bond cleavage.
2.3.d. Differentiate among the different types of membranes
2.1.o. Describe the relationship between energy charge and found in a eukaryotic cell.
concentrations of ATP, ADP, and AMP.
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Chapter 2: Physical Biochemistry: Energy Conversion, Water, and Membranes 6. Which of the following correctly describes the relationship between an ice cube melting on the
table and the air surrounding it?
a. The ice cube is the system and the air is the surroundings.
MULTIPLE CHOICE b. The air is the system and the ice cube is the surroundings.
c. The ice cube is the system and only the air is the universe.
1. Energy conversion in living systems is required for what three types of work? d. The air is the system and only the ice cube is the universe.
a. osmotic work, chemical work, mechanical work ANS: A DIF: Medium REF: 2.1
b. osmotic work, chemical work, potential work OBJ: 2.1.d. Differentiate between a system and its surroundings.
c. kinetic work, chemical work, mechanical work MSC: Evaluating
d. osmotic work, photosynthetic work, mechanical work
ANS: A DIF: Easy REF: 2.1 7. Which of the following is an example of a system?
OBJ: 2.1.a. Describe how sunlight is the source of all energy on Earth. a. the universe
MSC: Remembering b. the air
c. a test tube with reaction components
2. What chemical process is able to take place in the presence of solar energy? d. outer space
a. anaerobic respiration ANS: C DIF: Easy REF: 2.1
b. photosynthesis OBJ: 2.1.d. Differentiate between a system and its surroundings.
c. hydrogenation MSC: Understanding
d. hydrolysis
ANS: B DIF: Medium REF: 2.1 8. A hot pack on your arm is an example of what kind of system?
OBJ: 2.1.a. Describe how sunlight is the source of all energy on Earth. a. open
MSC: Remembering b. closed
c. isolated
3. Which of the following is the correct solar energy reaction that takes place on the sun? d. surroundings
a. 4 He → 4 He ANS: B DIF: Medium REF: 2.1
b. 4 He → 4 He OBJ: 2.1.e. Differentiate among open, closed, and isolated systems.
c. 4 H → 4 He MSC: Applying
d. 4 H → 4 H
9. Which of the following best describes an open system?
ANS: C DIF: Medium REF: 2.1 a. Matter and energy are freely exchanged with the surroundings.
OBJ: 2.1.a. Describe how sunlight is the source of all energy on Earth. b. Energy is exchanged with the surroundings but matter is not.
MSC: Understanding c. Matter is exchanged with the surroundings but energy is not.
d. Neither matter nor energy is exchanged with the surroundings.
4. What is the final molecule made from the oxidation of H2 O by solar energy?
a. ozone ANS: A DIF: Easy REF: 2.1
b. glucose OBJ: 2.1.e. Differentiate among open, closed, and isolated systems.
c. fructose MSC: Understanding
d. carbon dioxide
10. Which of the following best defines the first law of thermodynamics?
ANS: B DIF: Medium REF: 2.1 a. All spontaneous processes in the universe tend toward dispersal of energy.
OBJ: 2.1.c. Explain the role of oxidation-reduction reactions in biological systems. b. Total amount of energy in the universe is a constant.
MSC: Understanding c. There is no entropy at zero Kelvin.
d. Entropy is a measure of disorder.
5. The difference between an oxidation reaction and a reduction reaction is that oxidation is the
__________ and reduction is the __________. ANS: B DIF: Medium REF: 2.1
a. loss of electrons; gain of electrons OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems.
b. gain of electrons; loss of electrons MSC: Understanding
c. loss of protons; gain of protons
d. gain of protons; loss of protons
ANS: A DIF: Medium REF: 2.1
OBJ: 2.1.c. Explain the role of oxidation-reduction reactions in biological systems.
MSC: Analyzing
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11. Energy conversion in a biological system operates under constant __________ and 16. In the figure below, which state of matter has the highest entropy?
constant __________.
a. heat; pressure
b. work; heat
c. pressure; volume
d. volume; heat
ANS: C DIF: Medium REF: 2.1
OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems.
MSC: Applying
12. Given a biological system at 1 atm with ∆H = 16 kJ/g, what is the internal energy of the
system?
a. 15 kJ/g
b. 16 kJ/g
c. 14 kJ/g
d. Not enough information is given to calculate the answer.
ANS: B DIF: Difficult REF: 2.1
OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems.
MSC: Applying a. solid phase
b. liquid phase
13. The combustion of gasoline is considered exothermic because heat is c. gas phase
a. transferred from the surroundings to the system. d. all are equal entropy.
b. transferred from the system to the surroundings.
ANS: C DIF: Easy REF: 2.1
c. transferred to the universe.
OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems.
d. not transferred.
MSC: Remembering
ANS: B DIF: Medium REF: 2.1
OBJ: 2.1.g. Differentiate between endothermic and exothermic reactions. 17. For a reaction to be spontaneous, the change in the entropy of the universe must be
MSC: Understanding a. greater than zero.
b. less than zero.
14. Given 80 grams of water, how many calories are required to raise the temperature 1°C? c. equal to zero.
a. 4.184 calories d. equal to 1.
b. 15.7 calories
ANS: A DIF: Easy REF: 2.1
c. 80 calories
OBJ: 2.1.i. Explain the concept of entropy and its role in biological systems.
d. Not enough information is given to calculate the answer.
MSC: Understanding
ANS: C DIF: Medium REF: 2.1
OBJ: 2.1.g. Differentiate between endothermic and exothermic reactions. 18. The example of water freezing into ice shows
MSC: Applying a. an increase in entropy of the system.
b. a decrease in entropy of the system.
15. The oxidation of glucose releases 15.7 kJ/g. Is this reaction spontaneous? c. no change in the entropy of the system.
a. Yes, because it is exothermic. d. a decrease in the entropy of the surroundings.
b. No, because it is exothermic.
ANS: B DIF: Medium REF: 2.1
c. Yes, because it is endothermic.
OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems.
d. The answer cannot be determined.
MSC: Applying
ANS: D DIF: Difficult REF: 2.1
OBJ: 2.1.g. Differentiate between endothermic and exothermic reactions.
MSC: Analyzing
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19. The change in entropy of a system is a function of a change in 24. If a reaction has a ∆H < 0 and ∆S < 0, under which conditions would the reaction be
a. temperature and pressure. spontaneous in the forward direction?
b. volume and pressure. a. low temperatures
c. enthalpy and pressure. b. high temperatures
d. enthalpy and temperature. c. high pressure
d. low pressure
ANS: D DIF: Difficult REF: 2.1
OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems. ANS: A DIF: Medium REF: 2.1
MSC: Understanding OBJ: 2.1.k. Identify the impacts of enthalpy, entropy, and temperature on free energy.
MSC: Evaluating
20. Gibbs free energy can best be defined as the
a. difference between the enthalpy and entropy of a system at a given temperature. 25. The standard free energy change is defined under what set of conditions?
b. difference between exothermic and endothermic energy of a system at a given a. 1 atm, 298 K, 1 M
temperature. b. 1 atm, 273 K, 1 M
c. addition of enthalpy and entropy of a system at a given temperature. c. 100 kPa, 273 K, 1 M
d. difference between pressure and volume at a given temperature. d. 100 kPa, 298 K, 1 M
ANS: A DIF: Difficult REF: 2.1 ANS: A DIF: Difficult REF: 2.1
OBJ: 2.1.j. Define Gibbs free energy, its relation to enthalpy and entropy, and its relation to OBJ: 2.1.l. Differentiate between standard state condition and the biochemical standard state.
equilibrium. MSC: Understanding MSC: Understanding
21. For a given reaction with a ∆G < 0, the reaction is 26. If the equilibrium constant (Keq) is greater than 1, which direction will the reaction proceed?
a. favorable in the reverse direction. a. spontaneously to products
b. favorable in the forward direction. b. spontaneously to reactants
c. unfavorable in both directions. c. neither direction
d. favorable in both directions. d. Not enough information is given to determine the direction of reaction.
ANS: B DIF: Medium REF: 2.1 ANS: A DIF: Easy REF: 2.1
OBJ: 2.1.j. Define Gibbs free energy, its relation to enthalpy and entropy, and its relation to OBJ: 2.1.l. Differentiate between standard state condition and the biochemical standard state.
equilibrium. MSC: Understanding MSC: Applying
22. If a reaction has a ∆H > 0 and a ∆S < 0, then __________ and the reaction is __________ at 27. If the equilibrium constant (Keq) is greater than 1, what is the value of ∆G°?
all temperatures. a. ∆G° > 0
a. ∆G < 0; spontaneous b. ∆G° = 0
b. ∆G > 0; spontaneous c. ∆G° < 0
c. ∆G < 0; nonspontaneous d. ∆G° > 1
d. ∆G > 0; nonspontaneous
ANS: C DIF: Difficult REF: 2.1
ANS: D DIF: Medium REF: 2.1 OBJ: 2.1.l. Differentiate between standard state condition and the biochemical standard state.
OBJ: 2.1.j. Define Gibbs free energy, its relation to enthalpy and entropy, and its relation to MSC: Applying
equilibrium. MSC: Applying
28. Under what conditions could a biological reaction spontaneously proceed to reactants if the
23. If ∆G = 0 for a reaction, then this reaction ∆G° > 0?
a. is favorable in the forward direction. a. Reactant concentrations are greater than product concentrations.
b. is favorable in the reverse direction. b. Product concentrations are greater than reactant concentrations.
c. is at equilibrium. c. Reactant concentrations are equal to product concentrations.
d. cannot occur. d. There are no conditions where this could happen.
ANS: C DIF: Medium REF: 2.1 ANS: B DIF: Difficult REF: 2.1
OBJ: 2.1.j. Define Gibbs free energy, its relation to enthalpy and entropy, and its relation to OBJ: 2.1.l. Differentiate between standard state condition and the biochemical standard state.
equilibrium. MSC: Analyzing MSC: Evaluating
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Chapter 2: Physical Biochemistry: Energy Conversion, Water, and Membranes
Learning Objectives
2.1 Energy Conversion in Biological Systems 2.2 Water Is Critical for Life Processes
2.1.a. Describe how sunlight is the source of all energy on 2.2.a. Identify hydrogen bond donors and hydrogen bond
Earth. acceptors.
2.1.b. Differentiate between autotrophs and heterotrophs. 2.2.b. Describe how an antifreeze protein functions.
2.1.c. Explain the role of oxidation-reduction reactions in 2.2.c. Differentiate among hydrogen bonds, ionic
biological systems. interactions, and van der Waals interactions.
2.1.d. Differentiate between a system and its surroundings. 2.2.d. State the concept of the hydrophobic effect and how
it impacts protein folding.
2.1.e. Differentiate among open, closed, and isolated
systems. 2.2.e. Explain the impacts of hypotonic, isotonic, and
hypertonic solutions on cells.
2.1.f. Explain the first law of thermodynamics as it applies
to biological systems. 2.2.f. Identify the important aspects of plant, fungi, and
bacterial cells that allow them to survive in a hypotonic
2.1.g. Differentiate between endothermic and exothermic environment.
reactions.
2.2.g. Calculate the concentration of H+ or OH– given the
2.1.h. State the second law of thermodynamics as it applies OH– or H+ concentration.
to biological systems.
2.2.h. Relate pH to the concentration of H+ or OH–.
2.1.i. Explain the concept of entropy and its role in
biological systems. 2.2.i. Differentiate between weak acids and strong acids
and between weak bases and strong bases.
2.1.j. Define Gibbs free energy, its relation to enthalpy and
entropy, and its relation to equilibrium. 2.2.j. Relate pH to pKa using the Henderson-Hasselbalch
equation.
2.1.k. Identify the impacts of enthalpy, entropy, and
temperature on free energy. 2.3 Cell Membranes Function as Selective Hydrophobic
Barriers
2.1.l. Differentiate between standard state condition and the
biochemical standard state. 2.3.a. Identify the characteristics of a phospholipid that
contribute to membrane formation.
2.1.m. Differentiate between exergonic and endergonic
reactions and explain how such reactions are coupled in 2.3.b. Relate the degree of saturation in phospholipids to
biological systems. the fluidity of the membrane.
2.1.n. Identify the characteristics of the ATP molecule 2.3.c. Explain the various ways cholesterol impacts
that provide such a large standard free energy change for membrane structure.
phosphoanhydride bond cleavage.
2.3.d. Differentiate among the different types of membranes
2.1.o. Describe the relationship between energy charge and found in a eukaryotic cell.
concentrations of ATP, ADP, and AMP.
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Chapter 2: Physical Biochemistry: Energy Conversion, Water, and Membranes 6. Which of the following correctly describes the relationship between an ice cube melting on the
table and the air surrounding it?
a. The ice cube is the system and the air is the surroundings.
MULTIPLE CHOICE b. The air is the system and the ice cube is the surroundings.
c. The ice cube is the system and only the air is the universe.
1. Energy conversion in living systems is required for what three types of work? d. The air is the system and only the ice cube is the universe.
a. osmotic work, chemical work, mechanical work ANS: A DIF: Medium REF: 2.1
b. osmotic work, chemical work, potential work OBJ: 2.1.d. Differentiate between a system and its surroundings.
c. kinetic work, chemical work, mechanical work MSC: Evaluating
d. osmotic work, photosynthetic work, mechanical work
ANS: A DIF: Easy REF: 2.1 7. Which of the following is an example of a system?
OBJ: 2.1.a. Describe how sunlight is the source of all energy on Earth. a. the universe
MSC: Remembering b. the air
c. a test tube with reaction components
2. What chemical process is able to take place in the presence of solar energy? d. outer space
a. anaerobic respiration ANS: C DIF: Easy REF: 2.1
b. photosynthesis OBJ: 2.1.d. Differentiate between a system and its surroundings.
c. hydrogenation MSC: Understanding
d. hydrolysis
ANS: B DIF: Medium REF: 2.1 8. A hot pack on your arm is an example of what kind of system?
OBJ: 2.1.a. Describe how sunlight is the source of all energy on Earth. a. open
MSC: Remembering b. closed
c. isolated
3. Which of the following is the correct solar energy reaction that takes place on the sun? d. surroundings
a. 4 He → 4 He ANS: B DIF: Medium REF: 2.1
b. 4 He → 4 He OBJ: 2.1.e. Differentiate among open, closed, and isolated systems.
c. 4 H → 4 He MSC: Applying
d. 4 H → 4 H
9. Which of the following best describes an open system?
ANS: C DIF: Medium REF: 2.1 a. Matter and energy are freely exchanged with the surroundings.
OBJ: 2.1.a. Describe how sunlight is the source of all energy on Earth. b. Energy is exchanged with the surroundings but matter is not.
MSC: Understanding c. Matter is exchanged with the surroundings but energy is not.
d. Neither matter nor energy is exchanged with the surroundings.
4. What is the final molecule made from the oxidation of H2 O by solar energy?
a. ozone ANS: A DIF: Easy REF: 2.1
b. glucose OBJ: 2.1.e. Differentiate among open, closed, and isolated systems.
c. fructose MSC: Understanding
d. carbon dioxide
10. Which of the following best defines the first law of thermodynamics?
ANS: B DIF: Medium REF: 2.1 a. All spontaneous processes in the universe tend toward dispersal of energy.
OBJ: 2.1.c. Explain the role of oxidation-reduction reactions in biological systems. b. Total amount of energy in the universe is a constant.
MSC: Understanding c. There is no entropy at zero Kelvin.
d. Entropy is a measure of disorder.
5. The difference between an oxidation reaction and a reduction reaction is that oxidation is the
__________ and reduction is the __________. ANS: B DIF: Medium REF: 2.1
a. loss of electrons; gain of electrons OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems.
b. gain of electrons; loss of electrons MSC: Understanding
c. loss of protons; gain of protons
d. gain of protons; loss of protons
ANS: A DIF: Medium REF: 2.1
OBJ: 2.1.c. Explain the role of oxidation-reduction reactions in biological systems.
MSC: Analyzing
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11. Energy conversion in a biological system operates under constant __________ and 16. In the figure below, which state of matter has the highest entropy?
constant __________.
a. heat; pressure
b. work; heat
c. pressure; volume
d. volume; heat
ANS: C DIF: Medium REF: 2.1
OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems.
MSC: Applying
12. Given a biological system at 1 atm with ∆H = 16 kJ/g, what is the internal energy of the
system?
a. 15 kJ/g
b. 16 kJ/g
c. 14 kJ/g
d. Not enough information is given to calculate the answer.
ANS: B DIF: Difficult REF: 2.1
OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems.
MSC: Applying a. solid phase
b. liquid phase
13. The combustion of gasoline is considered exothermic because heat is c. gas phase
a. transferred from the surroundings to the system. d. all are equal entropy.
b. transferred from the system to the surroundings.
ANS: C DIF: Easy REF: 2.1
c. transferred to the universe.
OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems.
d. not transferred.
MSC: Remembering
ANS: B DIF: Medium REF: 2.1
OBJ: 2.1.g. Differentiate between endothermic and exothermic reactions. 17. For a reaction to be spontaneous, the change in the entropy of the universe must be
MSC: Understanding a. greater than zero.
b. less than zero.
14. Given 80 grams of water, how many calories are required to raise the temperature 1°C? c. equal to zero.
a. 4.184 calories d. equal to 1.
b. 15.7 calories
ANS: A DIF: Easy REF: 2.1
c. 80 calories
OBJ: 2.1.i. Explain the concept of entropy and its role in biological systems.
d. Not enough information is given to calculate the answer.
MSC: Understanding
ANS: C DIF: Medium REF: 2.1
OBJ: 2.1.g. Differentiate between endothermic and exothermic reactions. 18. The example of water freezing into ice shows
MSC: Applying a. an increase in entropy of the system.
b. a decrease in entropy of the system.
15. The oxidation of glucose releases 15.7 kJ/g. Is this reaction spontaneous? c. no change in the entropy of the system.
a. Yes, because it is exothermic. d. a decrease in the entropy of the surroundings.
b. No, because it is exothermic.
ANS: B DIF: Medium REF: 2.1
c. Yes, because it is endothermic.
OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems.
d. The answer cannot be determined.
MSC: Applying
ANS: D DIF: Difficult REF: 2.1
OBJ: 2.1.g. Differentiate between endothermic and exothermic reactions.
MSC: Analyzing
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19. The change in entropy of a system is a function of a change in 24. If a reaction has a ∆H < 0 and ∆S < 0, under which conditions would the reaction be
a. temperature and pressure. spontaneous in the forward direction?
b. volume and pressure. a. low temperatures
c. enthalpy and pressure. b. high temperatures
d. enthalpy and temperature. c. high pressure
d. low pressure
ANS: D DIF: Difficult REF: 2.1
OBJ: 2.1.f. Explain the first law of thermodynamics as it applies to biological systems. ANS: A DIF: Medium REF: 2.1
MSC: Understanding OBJ: 2.1.k. Identify the impacts of enthalpy, entropy, and temperature on free energy.
MSC: Evaluating
20. Gibbs free energy can best be defined as the
a. difference between the enthalpy and entropy of a system at a given temperature. 25. The standard free energy change is defined under what set of conditions?
b. difference between exothermic and endothermic energy of a system at a given a. 1 atm, 298 K, 1 M
temperature. b. 1 atm, 273 K, 1 M
c. addition of enthalpy and entropy of a system at a given temperature. c. 100 kPa, 273 K, 1 M
d. difference between pressure and volume at a given temperature. d. 100 kPa, 298 K, 1 M
ANS: A DIF: Difficult REF: 2.1 ANS: A DIF: Difficult REF: 2.1
OBJ: 2.1.j. Define Gibbs free energy, its relation to enthalpy and entropy, and its relation to OBJ: 2.1.l. Differentiate between standard state condition and the biochemical standard state.
equilibrium. MSC: Understanding MSC: Understanding
21. For a given reaction with a ∆G < 0, the reaction is 26. If the equilibrium constant (Keq) is greater than 1, which direction will the reaction proceed?
a. favorable in the reverse direction. a. spontaneously to products
b. favorable in the forward direction. b. spontaneously to reactants
c. unfavorable in both directions. c. neither direction
d. favorable in both directions. d. Not enough information is given to determine the direction of reaction.
ANS: B DIF: Medium REF: 2.1 ANS: A DIF: Easy REF: 2.1
OBJ: 2.1.j. Define Gibbs free energy, its relation to enthalpy and entropy, and its relation to OBJ: 2.1.l. Differentiate between standard state condition and the biochemical standard state.
equilibrium. MSC: Understanding MSC: Applying
22. If a reaction has a ∆H > 0 and a ∆S < 0, then __________ and the reaction is __________ at 27. If the equilibrium constant (Keq) is greater than 1, what is the value of ∆G°?
all temperatures. a. ∆G° > 0
a. ∆G < 0; spontaneous b. ∆G° = 0
b. ∆G > 0; spontaneous c. ∆G° < 0
c. ∆G < 0; nonspontaneous d. ∆G° > 1
d. ∆G > 0; nonspontaneous
ANS: C DIF: Difficult REF: 2.1
ANS: D DIF: Medium REF: 2.1 OBJ: 2.1.l. Differentiate between standard state condition and the biochemical standard state.
OBJ: 2.1.j. Define Gibbs free energy, its relation to enthalpy and entropy, and its relation to MSC: Applying
equilibrium. MSC: Applying
28. Under what conditions could a biological reaction spontaneously proceed to reactants if the
23. If ∆G = 0 for a reaction, then this reaction ∆G° > 0?
a. is favorable in the forward direction. a. Reactant concentrations are greater than product concentrations.
b. is favorable in the reverse direction. b. Product concentrations are greater than reactant concentrations.
c. is at equilibrium. c. Reactant concentrations are equal to product concentrations.
d. cannot occur. d. There are no conditions where this could happen.
ANS: C DIF: Medium REF: 2.1 ANS: B DIF: Difficult REF: 2.1
OBJ: 2.1.j. Define Gibbs free energy, its relation to enthalpy and entropy, and its relation to OBJ: 2.1.l. Differentiate between standard state condition and the biochemical standard state.
equilibrium. MSC: Analyzing MSC: Evaluating
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