Test Bank Essential Cell Biology 4th Edition Alberts

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The Use of Energy by Cells

3-1 Chemical reactions carried out by living systems depend on the ability of some organisms to capture and use atoms from nonliving sources in the environment. The specific subset of these reactions that break down nutrients in food can be described as _____________.
(a) metabolic.
(b) catabolic.
(c) anabolic.
(d) biosynthetic.

3-2 When there is an excess of nutrients available in the human body, insulin is released to stimulate the synthesis of glycogen from glucose. This is a specific example of a(n) __________ process, a general process in which larger molecules are made from smaller molecules.
(a) metabolic
(b) catabolic
(c) anabolic
(d) biosynthetic

3-3 The second law of thermodynamics states that the disorder in any system is always increasing. In simple terms, you can think about dropping NaCl crystals into a glass of water. The solvation and diffusion of ions is favored because there is an increase in _____________.
(a) pH.
(b) entropy.
(c) ions.
(d) stored energy.

3-4 The energy used by the cell to generate specific biological molecules and highly ordered structures is stored in the form of _____________.
(a) Brownian motion.
(b) heat.
(c) light waves.
(d) chemical bonds.

3-5 At first glance, it may seem that living systems are able to defy the second law of thermodynamics. However, on closer examination, it becomes clear that although cells create organization from raw materials in the environment, they also contribute to disorder in the environment by releasing _____________.
(a) water.
(b) radiation.
(c) heat.
(d) proteins.

3-6 If you weigh yourself on a scale one morning, then eat four pounds of food during the day, will you weigh four pounds more the next morning? Why or why not? (Hint: What happens to the atoms from the food you ingested?)

3-7 In the cytoplasm, materials are organized, separated, and sorted by membranes. Cells exploit the selective permeability of these membranes to partition populations of molecules and generate chemical energy for the cell. Use the principles of the first and second laws of thermodynamics to explain how membranes can be used to produce chemical energy.

3-8 Indicate whether the following statements are true or false. If a statement is false, explain why it is false.
A. The second law of thermodynamics states that the total amount of energy in the Universe does not change.
B. The ultimate source of energy for living systems is chlorophyll.
C. CO2 gas is fixed in a series of reactions that are light-dependent.
D. H2 is the most stable and abundant form of hydrogen in the environment.

3-9 Two college roommates do not agree on the best way to handle the clutter piled up in your dorm room. Roommate 1 explains that chaos is inevitable, so why fight it? Roommate 2 counters that maintaining an organized environment makes life easier in many ways, and that chaos is not inevitable. What law of thermodynamics drives the thinking of Roommate 1? What thermodynamic argument can be used to support Roommate 2?

3-10 Assume that the average human adult requires 2000 kilocalories per day to sustain all normal processes and maintain a constant weight. If manufactured solar panels could somehow provide power directly to the human body, what size solar panel would be required (in cm2)? Assume there are 10 hours of sunlight per day, and that the usable energy output for a typical solar panel is 850 kJ/ft2 per hour.
Note: 1 kcal = 4.184 kJ
1 ft2 = 929.03 cm2

3-11 In the first stage of photosynthesis, light energy is converted into what other form of energy?
(a) electrical
(b) chemical
(c) potential
(d) kinetic

3-12 Fill in the blanks, selecting from the choices below.

Light + _________ + _________  _________ + heat + sugars

CO, CO2, O2, H2, H2O, N2, NO

3-13 During respiration, energy is retrieved from the high-energy bonds found in certain organic molecules. Which of the following, in addition to energy, are the ultimate products of respiration?
(a) CO2, H2O
(b) CH3, H2O
(c) CH2OH, O2
(d) CO2, O2

3-14 Your body extracts energy from the food you ingest by catalyzing reactions that essentially “burn” the food molecules in a stepwise fashion. What is another way to describe this process?
(a) reduction
(b) oxidation
(c) dehydration
(d) solvation

3-15 Oxidation is a favorable process in an aerobic environment, which is the reason cells are able to derive energy from the oxidation of macromolecules. Once carbon has been oxidized to _______________, its most stable form, it can only cycle back into the organic portion of the carbon cycle through __________________.
(a) CO2, photosynthesis.
(b) CH3, combustion.
(c) CO2, respiration.
(d) CO, reduction.

3-16 For each of the pairs A–D in Figure Q3-16, pick the more reduced member of the pair.

Figure Q3-16

3-17 Oxidation is the process by which oxygen atoms are added to a target molecule. Generally, the atom that is oxidized will experience which of the following with respect to the electrons in its outer shell?
(a) a net gain
(b) a net loss
(c) no change
(d) an equal sharing

3-18 When elemental sodium is added to water, the sodium atoms ionize spontaneously. Uncharged Na becomes Na+. This means that the Na atoms have been _____________.
(a) protonated.
(b) oxidized.
(c) hydrogenated.
(d) reduced.

3-19 Indicate whether the following statements are true or false. If a statement is false, explain why it is false.
A. Photosynthetic organisms release only O2 into the atmosphere, while nonphotosynthetic organisms release only CO2.
B. The cycling of carbon through the biosphere first requires the incorporation of inorganic CO2 into organic molecules.
C. The oxidation of one molecule is always coupled to the reduction of a second molecule.
D. During cellular respiration, carbon-containing molecules become successively more oxidized until they reach their most oxidized form, as CO2.

3-20 Arrange the following molecules in order with respect to their relative levels of oxidation (assign 5 to the most oxidized and 1 to the most reduced).

_______ CH2O (formaldehyde)

_______ CH4 (methane)

_______ CHOOH (formic acid)

_______ CH3OH (methanol)

_______ CO2 (carbon dioxide)

3-21 Oxidation and reduction states are relatively easy to determine for metal ions, because there is a measurable net charge. In the case of carbon compounds, oxidation and reduction depend on the nature of polar covalent bonds. Which of the following is the best way to describe these types of bond?
(a) hydrogen bonds in a nonpolar solution
(b) covalent bonds in an aqueous solution
(c) unequal sharing of electrons across a covalent bond
(d) equal sharing of electrons across a covalent bond

3-22 Seed oils are often dehydrogenated and added back into processed foods as partly unsaturated fatty acids. In comparison with the original oil, the new fatty acids have additional double carbon–carbon bonds, replacing what were once single bonds. This process could also be described as _____________.
(a) isomerization.
(b) oxidation.
(c) reduction.
(d) protonation.

Free Energy and Catalysis

3-23 Chemical reactions that lead to a release of free energy are referred to as “energetically favorable.” Another way to describe these reactions is: _____________.
(a) uphill.
(b) uncatalyzed.
(c) spontaneous.
(d) activated.

3-24 Even though cellular macromolecules contain a large number of carbon and hydrogen atoms, they are not all spontaneously converted into CO2 and H2O. This absence of spontaneous combustion is due to the fact that biological molecules are relatively __________ and an input of energy is required to reach lower energy states.
(a) large
(b) polar
(c) stable
(d) unstable

3-25 ΔG° indicates the change in the standard free energy as a reactant is converted to product. Given what you know about these values, which reaction below is the most favorable?
(a) ADP + Pi  ATP ΔG° = +7.3 kcal/mole
(b) glucose 1-phosphate  glucose 6-phosphate ΔG° = –1.7 kcal/mole
(c) glucose + fructose  sucrose ΔG° = +5.5 kcal/mole
(d) glucose  CO2 + H2O ΔG° = –686 kcal/mole

3-26 Catalysts are molecules that lower the activation energy for a given reaction. Cells produce their own catalysts called _____________.
(a) proteins.
(b) enzymes.
(c) cofactors.
(d) complexes.

3-27 For each of the following sentences, fill in the blanks with the best word or phrase selected from the list below. Not all words or phrases will be used; each word or phrase should be used only once.

By definition, catalysis allows a reaction to occur more __________________. Chemical reactions occur only when there is a loss of __________________ energy. Enzymes act more __________________ than other catalysts. A catalyst decreases the __________________ energy of a reaction.

activation free selectively
chemical bond kinetic slowly
completely rapidly unfavorable

3-28 Figure Q3-28 is an energy diagram for the reaction XY. Which equation below provides the correct calculation for the amount of free-energy change when X is converted to Y?
(a) a + b – c
(b) a – b
(c) a – c
(d) c – a

Figure Q3-28

3-29 Enzymes facilitate reactions in living systems. Figure Q3-29 presents an energy diagram for the reaction XY. The solid line in the energy diagram represents changes in energy as the reactant is converted to product under standard conditions. The dashed line shows changes observed when the same reaction takes place in the presence of a dedicated enzyme. Which equation below indicates how the presence of an enzyme affects the activation energy of the reaction (catalyzed versus uncatalyzed)?
(a) d – c versus b – c
(b) d – a versus b – a
(c) a + d versus a + b
(d) d – c versus b – a

Figure Q3-29

3-30 The branched diagram in Figure Q3-30 represents several possible reaction pathways that substance X may follow. Each branch point represents two possible reactions, which would give rise to different products. Next to each of these points are values for the uncatalyzed activation energies and catalyzed activation energies (in kcal/mole), respectively.
A. Order the final products in the relative amounts you expect them to be produced in the absence of any enzymes (from greatest to least).
B. Order the final products in the relative amounts you expect them to be produced when enzymes for each reaction are present.
C. Compare your answers for parts A and B. How do you think the uncatalyzed reactions could influence the rates of catalyzed reactions inside the cell?

Figure Q3-30

3-31 A chemical reaction is defined as spontaneous if there is a net loss of free energy during the reaction process. However, spontaneous reactions do not always occur rapidly. Favorable biological reactions require ______________ to selectively speed up reactions and meet the demands of the cell.
(a) heat
(b) ATP
(c) ions
(d) enzymes

3-32 Which of the following statements are true or false? If a statement is false, explain why it is false.
A. Enzymes lower the free energy released by the reaction that they facilitate.
B. Enzymes lower the activation energy for a specific reaction.
C. Enzymes increase the probability that any given reactant molecule will be converted to product.
D. Enzymes increase the average energy of reactant molecules.

3-33 ΔG measures the change of free energy in a system as it converts reactant (Y) into product (X). When [Y] =[X], ΔG is equal to _____________.
(a) ΔG° + RT
(b) RT
(c) ln [X]/[Y]
(d) ΔG°

3-34 For the reaction YX at standard conditions with [Y] = 1 M and [X] = 1 M, ΔG is initially a large negative number. As the reaction proceeds, [Y] decreases and [X] increases until the system reaches equilibrium. How do the values of ΔG and ΔG° change as the reaction equilibrates?
(a) ΔG becomes less negative and ΔG° stays the same.
(b) ΔG becomes positive and ΔG° becomes positive.
(c) ΔG stays the same and ΔG° becomes less negative.
(d) ΔG reaches zero and ΔG° becomes more negative.

3-35 Which of the following is true for a reaction at equilibrium?
(a) ΔG = ΔG°
(b) ΔG° + RT ln [X]/[Y] = 0
(c) RT ln [X]/[Y] = 0
(d) ΔG + ΔG° = RT ln [X]/[Y]

3-36 The equilibrium constant (K) for the reaction YX can be expressed with respect to the concentrations of the reactant and product molecules. Which of the expressions below shows the correct relationship between K, [Y], and [X]?
(a) K = [Y]/[X]
(b) K = [Y] * [X]
(c) K = [X]/[Y]
(d) K = [X] – [Y]

3-37 Although the biochemical study of reaction rates and free energies is important for understanding each biological reaction individually, these studies do not provide an accurate picture of what is happening to reactants and products inside the cell. Why not?

3-38 Isomerization of glucose 1-phosphate to glucose 6-phosphate is energetically favorable. At 37°C, ΔG° = –1.42 log10K. What is the equilibrium constant for this reaction if ΔG° = –1.74 kcal/mole at 37°C?
(a) 16.98
(b) 0.09
(c) –0.09
(d) 0.39

3-39 On the basis of the two reactions below, decide which of the following statements are true and which are false. If a statement is false, explain why it is false.

1: ATP + Y  Y-P + ADP ΔG = –100 kcal/mole
2: Y-P + A  B ΔG = 50 kcal/mole

A. Reaction 1 is favorable because of the large negative ΔG associated with the hydrolysis of ATP.
B. Reaction 2 is an example of an unfavorable reaction.
C. Reactions 1 and 2 are coupled reactions, and when they take place together, reaction 2 will proceed in the forward direction.
D. Reaction 2 can be used to drive reaction 1 in the reverse direction.

3-40 The potential energy stored in high-energy bonds is commonly harnessed when the bonds are split by the addition of _______________ in a process called _____________.
(a) ATP, phosphorylation.
(b) water, hydrolysis.
(c) hydroxide, hydration.
(d) acetate, acetylation.

3-41 When the polymer X-X-X… is broken down into monomers, it is “phosphorylyzed” rather than hydrolyzed, in the following repeated reaction:

X-X-X… + P  X-P + X-X… (reaction 1)

Given the ΔG° values of the reactions listed in the following table, what is the expected ratio of X-phosphate (X-P) to free phosphate (P) at equilibrium for reaction 1?
(a) 1:106
(b) 1:104
(c) 1:1
(d) 104:1

Figure Q3-41

3-42 In the case of a simple conversion reaction such as XY, which value of ΔG° is associated with a larger concentration of X than Y at equilibrium? (Hint: How is ΔG° related to K?)
(a) ΔG° = –5
(b) ΔG° = –1
(c) ΔG° = 0
(d) ΔG° = 1

3-43 Consider the reaction XY in a cell at 37°C. At equilibrium, the concentrations of X and Y are 50 μM and 5 μM, respectively. Use this information and the equations below to answer questions A–E.

ΔG° = –0.616 ln Keq
ΔG = ΔG° + 0.616 ln [Y]/[X]

Recall that the natural log of a number z will have a negative value when z < 1, positive when z > 1, and 0 when z = 1.

A. What is the value of Keq for this reaction?
B. Is the standard free-energy change of this reaction positive or negative? Is the reaction XY an energetically favorable or unfavorable reaction under standard conditions?
C. What is the value of the standard free energy? Refer to Table 3–1 in the textbook or use a calculator.
D. Imagine circumstances in which the concentration of X is 1000 μM and that of Y is 1 μM. Is conversion of X to Y favorable? Will it happen quickly?
E. Imagine starting conditions in which the reaction XY is unfavorable, yet the cell needs to produce more Y. Describe two ways in which this may be accomplished.

3-44 Hydrolysis reactions are commonly used inside the cell to split high-energy covalent bonds. For each of the three reactions below, use the ΔG° for each reaction to determine the equilibrium constants (K). Assume that each reaction occurs independently of the other two.
ΔG° (kcal/mole)
Reaction 1: acetyl-P  actetate + P –10.3
Reaction 2: ATP  ADP + P –7.3
Reaction 3: glucose 6-P  glucose + P –3.3

3-45 If proteins A and B have complementary surfaces, they may interact to form the dimeric complex AB. Which of the following is the correct way to calculate the equilibrium constant for the association between A and B?
(a) kon/koff = K
(b) K = [A][B]/[AB]
(c) K = [AB]/[A][B]
(d) (a) and (c)

3-46 Match the following general equations with the energy diagram that best describes the free-energy transitions along the reaction pathway. Indicate your answer by filling in the equation number in the box under each respective curve. After you have identified a match for each equation, indicate the positions of A, B, and C (if applicable) on the free-energy curves. Not all of the energy diagrams will have a match.

Figure Q3-46

3-47 The equilibrium constant for complex formation between molecules A and B will depend on their relative concentrations, as well as the rates at which the molecules associate and dissociate. The association rate will be larger than the dissociation rate when complex formation is favorable. The energy that drives this process is referred to as ___________.
(a) dissociation energy.
(b) association energy.
(c) binding energy.
(d) releasing energy.

3-48 Which of the following statements would not be true of a favorable binding equilibrium?
(a) The free-energy change is negative for the system.
(b) The concentration of the complex remains lower than the concentration of the unbound components.
(c) The complex dissociation rate is slower than the rate for component association.
(d) The binding energy for the association is large and negative.

3-49 Indicate whether the following statements are true or false. If a statement is false, explain why it is false.
A. When two macromolecules form a complex, the free energy of the system increases because there is a net increase in the amount of order in the cell.
B. Sequential pathways can help drive unfavorable reactions by siphoning off the products into the next energetically favorable reaction in the series.
C. The cytosol is densely packed with molecules, creating what is more an aqueous gel than a solution.
D. The diffusion rates for smaller molecules in the cytosol are much lower than what is observed for the same molecules in water.

3-50 The net distance a molecule travels through the cytosol via diffusion is relatively short in comparison with the total distance it may need to travel. This is because movement governed by diffusion alone is a ________________ process that is most effective for the dispersion of small molecules over short distances.
(a) slow
(b) random
(c) regulated
(d) complicated

3-51 The small molecule cyclic AMP (cAMP) takes about 0.2 second to diffuse 10 μm, on average, in a cell. Suppose that cAMP is produced near the plasma membrane on one end of the cell; how long will it take for this cAMP to diffuse through the cytosol and reach the opposite end of a very large cell, on average? Assume that the cell is 200 μm in diameter.
(a) 4 seconds
(b) 16 seconds
(c) 80 seconds
(d) 200 seconds

3-52 The graph in Figure Q3-52 illustrates the relationship between reaction rates and substrate concentration for an enzyme-catalyzed reaction. What does the Km value indicate with respect to enzyme–substrate interactions?
(a) the maximum rate of catalysis
(b) the number of enzyme active sites
(c) the enzyme–substrate binding affinity
(d) the equilibrium rate of catalysis

Figure Q3-52

3-53 The graph in Figure Q3-53 illustrates the change in the rate of an enzyme-catalyzed reaction as the concentration of substrate is increased. Which of the values listed below is used to calculate the enzyme turnover number?
(a) ½Vmax
(b) Km
(c) Vmax
(d) Vmax – Km

Figure Q3-53

3-54 Protein E can bind to two different proteins, S and I. The binding reactions are described by the following equations and values:

E + S  ES Keq for ES = 10
E + I  EI Keq for EI = 2

Given the equilibrium constant values, which one of the following statements is true?
(a) E binds I more tightly than S.
(b) When S is present in excess, no I molecules will bind to E.
(c) The binding energy of the ES interaction is greater than that of the EI interaction.
(d) Changing an amino acid on the binding surface of I from a basic amino acid to an acidic one will probably make the free energy of association with E more negative.

3-55 The study of enzyme kinetics is usually performed with purified components and requires the characterization of several aspects of the reaction, including the rate of association with the substrate, the rate of catalysis, and _____________.
(a) the enzyme’s structure.
(b) the optimal pH of the reaction.
(c) the subcellular localization of the enzyme.
(d) the regulation of the enzyme activity.

3-56 Indicate whether the following statements about enzymes are true or false. If a statement is false, explain why it is false.
A. Enzymes alter the equilibrium point of a reaction.
B. Vmax can be determined by measuring the amount of product accumulated late in the reaction.
C. Competitive inhibitors bind irreversibly to the enzyme active site, lowering Vmax.

3-57 A. You are measuring the effect of temperature on the rate of an enzyme-catalyzed reaction. If you plot reaction rate against temperature, which of the graphs in Figure Q3-57 would you expect your plot to resemble?
B. Explain why temperature has this effect.

Figure Q3-57

3-58 Consider a description of an enzymatic reaction pathway that begins with the binding of substrate S to enzyme E, and ends with the release of product P from the enzyme.

E + S  ES  EP  E + P

In many circumstances,

Km = [E][S]/[ES]

A. What proportion of enzyme molecules is bound to substrate when [S] = Km?
B. Recall that when [S] = Km, the reaction rate is ½Vmax. Does your answer to part A make sense in the light of this rate information?

3-59 Figure Q3-59 illustrates the amount of energy per molecule for a population in a contained, controlled environment. Most molecules will have the average energy of the population, shown in region 1. The number of molecules in the population with enough energy to be converted to product is shown in region 2. The number of molecules with enough energy to react in the presence of enzyme is shown in region 3. Use this information to explain how enzymes catalyze reactions.

Figure Q3-59

3-60 Chemical reactions are reversible; they can proceed in both the forward and reverse directions. If the ΔG° for the reaction YX is energetically favorable, how can you explain the fact that not all of the Y molecules will be converted to X molecules?

3-61 The maximum velocity (Vmax) of an enzymatic reaction is an important piece of information regarding how the enzyme works. What series of measurements can be taken in order to infer the maximum velocity of an enzyme-catalyzed reaction?
(a) the rate of substrate consumption after the system reaches equilibrium, for several reactant concentrations
(b) the rate of product consumption shortly after mixing the enzyme and substrate
(c) the rate of substrate consumption at high levels of enzyme concentration
(d) the rate of substrate consumption shortly after mixing the enzyme and substrate, for several substrate concentrations

3-62 What information regarding an enzyme-catalyzed reaction is obtained in a plot of the inverse of the initial velocities against the inverse of the corresponding substrate concentrations?
(a) 1/Vmax and 1/Km
(b) 1/V and 1/[S]
(c) Vmax and Km
(d) V and [S]

3-63 Enzymes A and B catalyze different reactions, but use the same reactant molecule as a substrate. The graph in Figure Q3-63 presents the reaction rates observed when enzyme A and enzyme B are mixed together in a single test tube containing molecule X. What are the Vmax and the apparent Km values for each enzyme under these conditions? How might these values change for enzyme B if it were analyzed in the absence of enzyme A? Explain your answer.

Figure Q3-63

3-64 The study of enzymes also includes an examination of how the activity is regulated. Molecules that can act as competitive inhibitors for a specific reaction are often similar in shape and size to the enzyme’s substrate. Which variable(s) used to describe enzyme activity will remain the same in the presence and absence of a competitive inhibitor?
(a) Vmax
(b) V
(c) Vmax and Km
(d) Km

Activated Carriers and Biosynthesis

3-65 Activated carriers are small molecules that can diffuse rapidly and be used to drive biosynthetic reactions in the cell. Their energy is stored in a readily transferable form such as high-energy electrons or chemical groups. Which of the molecules below is the most widely used activated carrier?
(a) FADH2
(b) NADH
(d) ATP

3-66 Energy cannot be created or destroyed, but it can be converted into other types of energy. Cells use potential kinetic energy to generate stored chemical energy in the form of activated carrier molecules, which are often employed to join two molecules together in _____________ reactions.
(a) oxidation
(b) hydrolysis
(c) condensation
(d) reduction

3-67 Consider an analogy between reaction-coupling and money. In a simple economy, barter provides a means of direct exchange of material goods. For example, the owner of a cow may have excess milk and need eggs, whereas a chicken owner has excess eggs and needs milk. Provided that these two people are in close proximity and can communicate, they may exchange or barter eggs for milk. But in a more complex economy, money serves as a mediator for the exchanges of goods or services. For instance, the cow owner with excess milk may not need other goods until three months from now, or may want goods from someone who does not need milk. In this case, the “energy” from providing milk to the economy can be temporarily “stored” as money, which is a form of “energy” used for many transactions in the economy. Using barter and money as analogies, describe two mechanisms that can serve to drive an unfavorable chemical reaction in the cell.

3-68 You are studying a biochemical pathway that requires ATP as an energy source. To your dismay, the reactions soon stop, partly because the ATP is rapidly used up and partly because an excess of ADP builds up and inhibits the enzymes involved. You are about to give up when the following table from a biochemistry textbook catches your eye.

Figure Q3-68

Which of the following reagents are most likely to revitalize your reaction?
(a) a vast excess of ATP
(b) glucose 6-phosphate and enzyme D
(c) creatine phosphate and enzyme A
(d) pyrophosphate

3-69 The anhydride formed between a carboxylic acid and a phosphate (Figure Q3-69A) is a high-energy intermediate for some reactions in which ATP is the energy source. Arsenate can also be incorporated into a similar high-energy intermediate in place of the phosphate (Figure Q3-69B). Figure Q3-69C shows the reaction profiles for the hydrolysis of these two high-energy intermediates. What is the effect of substituting arsenate for phosphate in this reaction?

Figure Q3-69

(a) It forms a high-energy intermediate of lower energy.
(b) It forms a high-energy intermediate of the same energy.
(c) It decreases the stability of the high-energy intermediate.
(d) It increases the stability of the high-energy intermediate.

3-70 In general, there is a positive change in free energy associated with reduction reactions, and most of them are coupled with oxidation reactions. The last step in the biosynthesis of cholesterol involves the reduction of a carbon–carbon double bond. What activated carrier molecule is used in this reaction (and generally for the reduction of lipids) and how would this reaction be influenced by the levels of available ATP?

3-71 The synthesis of glutamine from glutamic acid requires the production of an activated intermediate followed by a condensation step that completes the process. Both amino acids are shown in Figure Q3-71.

Figure Q3-71

Which molecule is added to glutamic acid in the activation step?
(a) phosphate
(b) NH3
(c) ATP
(d) ADP

3-72 The synthesis of glutamine from glutamic acid requires the production of an activated intermediate followed by a condensation step that completes the process. Both amino acids are shown in Figure Q3-72.

Figure Q3-72

In the condensation step, _______________ is displaced by ________________.
(a) OH, NH3.
(b) ADP, NH2.
(c) ATP, NH3.
(d) phosphate, NH3.

3-73 NADH and NADPH are activated carrier molecules that function in completely different metabolic reactions. Both carry two additional ________ and one additional _____________. This combination can also be referred to as a hydride ion.
(a) protons, electron.
(b) electrons, phosphate.
(c) hydrogens, electron.
(d) electrons, proton.

3-74 Coenzyme A can be converted to acetyl CoA, which is an important activated carrier molecule that has a central role in metabolism and can be used to add two carbons in each successive cycle of fatty acid synthesis.
A. Identify the location and type of high-energy bond in the acetyl CoA molecule shown in Figure Q3-74.
B. How does the bond energy help promote the synthesis of fatty acids?
C. What function does the rest of the coenzyme A molecule serve in these reaction pathways?

Figure Q3-74

3-75 The addition of a new deoxynucleotide to a growing DNA chain requires more energy than can be obtained by the hydrolysis of ATP to ADP + Pi. What alternative series of reactions is used, and how does this help overcome the energy barrier for DNA synthesis?


3-1 (b)

3-2 (c)

3-3 (b)

3-4 (d)

3-5 (c)

3-6 No, you will not weigh four pounds more the next morning because only a small portion of the mass of the food will form components of the body. Much of the mass of food is either released as CO2 and H2O that are breathed out into the atmosphere or converted into materials excreted as waste products.

3-7 When one type of molecule accumulates at a higher concentration on one side of the membrane, the molecules become “organized” by having their movement limited to the space they occupy. The second law of thermodynamics indicates that, if allowed to do so, the molecules would move across the membrane until there is an equal distribution of molecules on either side. The accumulation of molecules on one side of the membrane represents a store of potential energy. The first law of thermodynamics tells us that this energy will not be lost, but rather converted into a different type of energy. First, when the molecules are then allowed to move across the membrane, this potential energy is converted into kinetic energy. The kinetic energy of molecules moving through a protein channel to cross the membrane is often linked to conformational changes in the protein, promoting specific chemical reactions.

3-8 A. False. The second law of thermodynamics states that components of any system move toward greater disorder. It is the first law of thermodynamics that states that energy is neither created nor destroyed.
B. False. The ultimate source of energy for living organisms is sunlight.
C. False. The fixation of carbon from CO2 occurs independently of light.
D. False. The most stable form of hydrogen is H2O.

3-9 The second law of thermodynamics supports Roommate 1’s view. It is favorable for a system to become less ordered. However, if the energy used to create an ordered environment in the room is accompanied by enough release of heat, the Universe will become more disordered as the room becomes more organized. Thus, while increasing chaos is inevitable, the room—like a cell—can be kept highly organized, by interconverting types of energy.

3-10 Conversion factors:
1 kcal = 4.184 kJ
1 ft2 = 929.03 cm2

If there are 10 hours of sunlight each day hitting the solar panel, there are 8500 kJ/ft2 produced per day. The average adult human requires 8368 kJ per day; thus, with a conventional solar panel, we would require a surface area of about a square foot, or more precisely in cm2:

8368 kJ/X = 8500 kJ/929.03 cm2

929.03 μltiply 8368/8500 = X

X = 914.57 cm2

3-11 (a) or (d)

3-12 Light + H2O + CO2  O2 + heat + sugars

3-13 (a)

3-14 (b)

3-15 (a)

3-16 A—ii; B—ii; C—i; D—ii. “More reduced” means having more electrons; gain of electrons can result in an increased negative charge or a decreased positive charge and can be due to an increase in the number of hydrogen atoms in a molecule.

3-17 (b)

3-18 (b)

3-19 A. False. Plants, as well as photosynthetic algae and bacteria, perform both photosynthesis and respiration. This means that photosynthetic organisms release both O2 and CO2 into the atmosphere.
B. True.
C. True. This forms the basis for redox pairs.
D. True.

3-20 __3__ CH2O (formaldehyde)

__1__ CH4 (methane)

__4__ CHOOH (formic acid)

__2__ CH3OH (methanol)

__5__ CO2 (carbon dioxide)

3-21 (c)

3-22 (b)

3-23 (c)

3-24 (c)

3-25 (d)

3-26 (b)

3-27 By definition, catalysis allows a reaction to occur more rapidly. Chemical reactions occur only when there is a loss of free energy. Enzymes act more selectively than other catalysts. A catalyst decreases the activation energy of a reaction.

3-28 (d)

3-29 (b)

3-30 The lower the activation energy, the larger the number of molecules that have the energy required to overcome the energy barrier. When no enzymes are present, the uncatalyzed activation energies will determine the relative rates at which the substrate undergoes either reaction.
A. Following this principle, the relative amounts of products in the absence of the necessary enzymes (from greatest to least) are: C, D, A, B, H, G, E, F.
B. In the presence of the enzymes required to catalyze the two different reactions represented by each branch, we should expect to see a different distribution of products: G, H, E, F, A, B, D, C.
C. Although we can make these predictions based on activation energies, there are many other factors that determine how fast a certain product will accumulate: reactant concentration, catalytic efficiency of the enzyme in question, and the relative reactivity of the product, to name a few. If a reaction has a very low uncatalyzed activation energy, it could occur spontaneously at a rapid rate, which would decrease the concentration of substrate available for the enzyme-catalyzed reaction. If this is the case, the relative abundances predicted in part B will change.

3-31 (d)

3-32 A. False. Enzymes do not affect the initial energy of the reactants nor the final energy of the products after the reaction is complete, which are the values that determine the change in free energy of a reaction.
B. True.
C. True.
D. False. By lowering the energy of activation, enzymes increase the number of molecules in a population that can overcome the activation barrier.

3-33 (d)

3-34 (a)

3-35 (b)

3-36 (c)

3-37 Chemical reactions inside the cell do not reach a state of equilibrium because both reactants and products are typically used in more than one set of reactions, which means their concentrations are constantly fluctuating. As a result, the forward and reverse reaction rates are almost never identical.

3-38 (a)

3-39 A. True.
B. True.
C. True.
D. False. This is false for two reasons: (1) reaction 2 is unfavorable, as indicated by the positive free-energy change associated with the reaction; (2) the reverse reaction, although possibly more favorable, will yield the product for reaction 1, not reactants to help drive it forward.

3-40 (b)

3-41 (c) Reaction 1 can be written as the sum of the three reactions given, because the ATP used in step 2 is restored in step 3.

X-X-X… + H2O  X + X-X… ΔG° = –4.5 kcal/mole
X + ATP  X-P + ADP ΔG° = –2.8 kcal/mole
ADP + P  ATP + H2O ΔG° = +7.3 kcal/mole

Because ΔG° values are additive, ΔG°total = 0, and if ΔG° = 0, Keq = 1, meaning that