Biochem – Chapter 15 [Lipids and Proteins Are Associated in Biological Membranes] – Flashcards

Which of the following statements concerning the free energy change (DG) is false? A. The energy change for a reaction depends only on the initial and final states, and is independent of the path taken. B. The overall energy change for a reaction could be calculated by summing the energy changes for a series of separate reactions that could convert the reactants to the products. C. The rate of a reaction can be determined from the energy change. D. The energy change is a function of the concentrations of the products and reactants at start.

The standard state of a solution is taken as A. 1 atmosphere of pressure. B. the pure solute. C. 1 molar concentration. D. none of the above.

Consider this rxn which has a DG = +0.4 kJ/mol. A + B « C + D 1 M A, 1 M B, 0.1 M C and 0.1 M D are added to a container at room temperature. Which of the following statements is true? A. The reaction will proceed in the forward direction to reach equilibrium. B. The reaction will proceed in the backward direction to reach equilibrium. C. The reaction will not proceed in either direction; it is already at equilibrium. D. Cannot be determined from the information provided.

Consider this rxn which has a DG = +0.4 kJ/mol. succinate + FAD « fumarate + FADH2 1 mM of each compound are mixed & the reaction is allowed to come to equilibrium. Which statement is correct about the resulting concentration of FAD at equilibrium? A. [FAD] > [FADH2] B. [FAD] < [FADH2] C. [FAD] = [FADH2] D. Cannot be determined from the information provided.

Consider this rxn which has a DG = +0.4 kJ/mol. A + B « C + D 1 M A, 1 M B, 0.1 M C and 0.1 M D are added to a container at room temperature. Which of the following statements is true? A. DG < 0 (i.e., it's negative) B. DG = 0 C. DG > 0 (i.e., it's positive) D. Cannot be determined from the information provided.

Which of the following is not true concerning standard states? A. For pure liquids, the standard state is 1M B. For pure solids, the standard state is the pure solid itself C. For gases, the standard state is 1 atmosphere D. For solutes, the standard state is 1M

I am performing a reaction, A ® B, with DG' = -0.3 kJ/mol. I start the reaction with 10 mM A and no B. After allowing the reaction to proceed for 24 hrs at room temperature and atmospheric pressure, I analyze a sample of the reaction mix to find I now have 1 mM A and 9 mM B. Which of the following conclusions should I make? A. The reaction has reached equilibrium. B. I should come back again later; equilibrium has not yet been reached. C. The formation of B from A is thermodynamically unfavorable, so I should find another starting material to make B. D. I must've screwed up; there's no way I could get that result with that DG'

I am performing a reaction, A ® B, with DG' = -5000 kJ/mol. I start the reaction with 10 mM A and no B. After allowing the reaction to proceed for 24 hrs at room temperature and atmospheric pressure, I analyze a sample of the reaction mix to find I now have 8 mM A and 2 mM B. Which of the following conclusions should I make? A. The reaction has reached equilibrium. B. I should come back again later; equilibrium has not yet been reached. C. The formation of B from A is thermodynamically unfavorable, so I should find another starting material to make B. D. I must've screwed up; there's no way I could get that result with that DG'

Biochemists use a modified value for standard DG values because A. all reagents are not at a 1 molar concentration. B. the pH in living systems is seldom, if ever, near 0. C. the concentration of water is not at 1 molar concentration. D. the reagents are not one molar and the pH = 7. E. All of these justify why biochemists use a special DG value.

Which best describes the DG for hydrolysis of creatine phosphate under cellular conditions in which the concentration of creatine phosphate, creatine, and phosphate all equal 1 mM at 25C. The DG for the hydrolysis of creatine phosphate at 25C is -43 kJ/mol. A. DG < -43 kJ/mol B. DG = -43 kJ/mol C. -43 kJ/mol < DG £ 0 kJ/mol D. DG > 0 kJ/mol

By definition, a spontaneous reaction is one in which A. energy is released. B. energy is absorbed. C. the energy change is zero. D. the reaction happens quickly E. energy is released and the reaction happens quickly

The standard state usually used in biochemistry (DG') includes A. all concentrations at 1 M. B. all concentrations at 1 M, except for [H+], which is 10-7 M. C. same as a), but at 25 C. D. same as b), but at 25 C.

"Metabolism" refers to A. the breakdown of larger molecules into smaller ones. B. the production of larger molecules from smaller ones. C. both of these D. none of these

The production of larger molecules from smaller ones is called A. metabolism. B. catabolism. C. anabolism. D. none of these

In general, catabolism A. releases energy. B. absorbs energy. C. neither absorbs nor releases energy.

In general, catabolism A. is an oxidative process that releases energy B. is a reductive process that releases energy C. is an oxidative process that requires energy D. is a reductive process that requires energy E. none of these

Which of the following statements apply to anabolism? A. proceeds in stages B. requires energy C. requires reducing agents D. all of these

"Oxidation" refers to A. the loss of oxygen. B. the gain of oxygen. C. the loss of electrons. D. the gain of electrons.

An oxidizing agent A. loses oxygen. B. gains oxygen. C. loses electrons. D. gains electrons.

Exhibit 15A Consider the reaction of alcohol dehydrogenase. Refer to Exhibit 15A. Which is the oxidizing agent? A. Ethanol B. NAD+ C. Acetaldehyde D. NADH E. H+

Exhibit 15A Consider the reaction of alcohol dehydrogenase. Refer to Exhibit 15A. Which molecule is reduced? A. Ethanol B. NAD+ C. Acetaldehyde D. NADH E. H+

Exhibit 15A Consider the reaction of alcohol dehydrogenase. Refer to Exhibit 15A. Which molecule loses electrons? A. Ethanol B. NAD+ C. Acetaldehyde D. NADH E. H+

During reduction A. electrons are lost. B. electrons are gained. C. electrons may either be lost or gained. D. hydrogen is formed.

In general, the anabolic pathways tend to involve oxidation reactions.

Which of the following is not true? A. Molecular oxygen is always a substrate in oxidation reactions. B. Oxidation reactions involve the movement of electrons from one molecule to another C. When a molecule is oxidized, it loses electrons D. Reduction involves the gain of electrons

Which of the following coenzymes is not a carrier of electrons in biological redox reactions? A. Coenzyme A B. Niacin. C. Riboflavin. D. Transition metal ions, such as those of iron or copper. E. All of these can be intermediate electron carriers.

In biological redox reactions, hydrogen ions are usually transferred along with electrons.

Which of the following coenzymes is derived from riboflavin? A. Coenzyme A B. NAD+. C. FAD D. All of the above. E. None of the above.

Which of the following is not a part of FAD? A. Ribitol B. isoalloxazine C. adenine D. ribose E. nicotinamide

The conversion of NAD+ to NADH is an example of reduction because A. the pyridine ring loses electrons (and a hydrogen) B. the pyridine ring gains electrons (and a hydrogen) C. the adenine ring loses electrons D. the adenine ring gains electrons

In the coenzyme FAD the site to which electrons are transferred is A. the ribose moiety of the molecule B. a purine ring system C. a pyrimidine ring system D. a nitrogen-containing ring system

What happens to the entropy when ATP is hydrolysed to ADP? A. Entropy increases B. Entropy decreases. C. Entropy doesn't change. D. ATP has no entropy.

The oxidation of nutrients supplies the energy to produce ATP.

In order to drive the synthesis of ATP, the hydrolysis of an organic phosphate A. must have a higher free energy change. B. must have a lower free energy change. C. must have a free energy change equal to that of ATP.

Consider these reactions: ATP ® ADP + Pi DG' = -31 kJ/mol glucose-6-phosphate ® glucose + Pi DG' = -13 kJ/mol glucose + ATP ® glucose-6-phosphate + ADP DG' = ? What is the DG' of the last reaction? A. -44 kJ/mol B. -18 kJ/mol C. +18 kJ/mol D. +44 kJ/mol E. Cannot be determined from the information provided.

ATP is a good source of energy to run metabolic reactions for all the following reasons, except: A. The pyrophosphate bond has a high energy of hydrolysis. B. The sugar group is very reactive. C. The bonds between the phosphates are acid anhydrides. D. The phosphate groups can combine readily with other molecules. E. All of these explain why ATP is a good energy source.

The body allows energy consuming reactions to occur by coupling them with reactions which have a negative DG.

The number of degrees of freedom a molecule has is related to the numbers of resonant structures it has.

What happens to the entropy of a molecule as the number of resonance structures increases? A. Entropy also increases. B. Entropy decreases. C. Entropy has no relationship to the number of resonance

Many cells oxidize fatty acids to produce ATP. If no ATP were produced, the DG' of this process would be A. unchanged B. a larger positive number C. a larger negative number D. impossible to determine

When we say that the efficiency of glycolysis is about 33% we mean that A. 2 ATP are produced and 6 ATP are involved in the overall process B. 2 ATP are produced in the oxidation of glucose, which contains six carbon atoms C. the energy used to phosphorylate 2 ATP is 33% of the energy released in the process D. all of these

The energy released during metabolism of nutrients can be used to synthesize ATP from ADP and phosphate.

In order to initiate many metabolic pathways it is necessary to activate the starting materials.

If the reaction A ® B has DG = +25 Joule/mol and the reaction B ® C has DG = -15 Joule/mol, the overall energy change A ® C will be A. -40 Joule/mol. B. -15 Joule/mol. C. +10 Joule/mol. D. +40 Joule/mol. E. You cannot determine the overall reaction from the given data.

Which of the following are examples of endergonic processes? A. protein synthesis and active transport B. protein synthesis and oxidation of carbohydrates C. active transport and oxidation of carbohydrates D. oxidation of fats and of carbohydrates

Which of the following are examples of exergonic processes? A. protein synthesis and active transport B. protein synthesis and oxidation of carbohydrates C. active transport and oxidation of carbohydrates D. oxidation of fats and of carbohydrates

The phosphorylation of ADP to produce ATP is endergonic because A. a negatively charged ion is bonded to a molecule that already carries a negative charge B. ATP is more stable than ADP C. the entropy of the products is less than that of the reactants D. polyphosphate chains are the storage form of phosphorus in living organisms

Spontaneous reaction always occurs at a relatively fast rate.

The efficiency of aerobic metabolism is greater than that of anaerobic metabolism even though much more energy is released in aerobic than in anaerobic metabolism because A. aerobic metabolism is linked to oxygen, which is a more powerful oxidizing agent than those in anaerobic metabolism B. aerobic metabolism produces carbon dioxide and water C. aerobic metabolism traps much more energy in the form of ATP than does anaerobic metabolism D. anaerobic metabolism produces two- and three-carbon compounds

The hydrolysis of ATP can be used to drive reactions that have a DG' that is A. greater than +5 kJ/mol B. less than +5 kJ/mol C. between +20 and +40 kJ/mol D. not possible to determine from the information in this chapter

The linking of an exergonic reaction to drive an endergonic reaction is called: A. coupling B. a state function C. resonance D. catabolsim

What happens to the entropy when ATP is hydrolysed to ADP? A. Entropy increases B. Entropy decreases. C. Entropy doesn't change. D. ATP has no entropy.

In metabolism the term "activation" refers to A. conversion of a component of a metabolic pathway into a reactive compound. B. addition of a catalyst. C. bypassing endergonic reactions in a pathway. D. bypassing the unreactive components of a pathway.

An example of an activation step in metabolism is A. the hydrolysis of a triacylglycerol. B. the cis-trans isomerization of retinal. C. the formation of an acyl derivative of coenzyme A. D. the formation of the peptide bond.

Which of the following is NOT a mechanism used to activate substrates for further metabolism? A. Addition of a phosphate group. B. Combination with a vitamin, such as coenzyme A. C. Hydrolyzing a polymer into its component monomers. D. Addition of a phosphate group or combining with a vitamin. E. All of these processes activate substrates.

Metabolism takes place in stages A. because enzymes cannot catalyze the process efficiently B. and allows for efficient production and use of energy C. because large free energy changes cannot occur in living organisms D. to use highly unreactive compounds