Biochemistry quize on Bioenergetics
1. The biochemical reactions that result in loss of free energy are known as
a. Exergonic
b. Endergonic
c. Endothermic
d. Metabolic
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2. The biochemical reactions that result in the gain of free energy are known as
a. Exergonic
b. Endergonic
c. Endothermic
d. Metabolic
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3. The biological vital processes obtain energy for oxidative reactions by
a. Chemical linkage
b. Linkage equilibrium
c. Linkage disequilibrium
d. Equilibrium
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4. The biochemical exergonic reactions are termed
a. Metabolic reactions
b. Anabolic reactions
c. Catabolic reactions
d. Endothermic reactions
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5. The energy rich compound in living cells is
a. ATP
b. ADP
c. NADP
d. DNA
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6. Life forms that obtain free energy by simple exergonic processes are termed
a. Heterotrophic
b. Herbivores
c. Benthic
d. Autotrophic
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7. Life forms that obtain free energy by breakdown of complex organic
molecules are termed
a. Heterotrophic
b. Herbivores
c. Benthic
d. Autotrophic
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8. ATP has an important role in obtaining free energy in
a. Heterotrophs
b. Herbivores
c. Plankton
d. Autotrophs
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9. In cellular reactions, ATP complexes with
a. Fe2+
b. Fe3+
c. Mg2+
d. Mg3+
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10. Which of the following is not a high-energy compound
a. Adenosine Tri-Phosphate
b. Acetyl-CoA
c. Adenosine Mono-Phosphate
d. Active methionine
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11. Which of the following is a low-energy compound
a. Adenosine Tri-Phosphate
b. acetyl-CoA
c. Adenosine Mono-Phosphate
d. Active methionine
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12. A process that is not a source of high energy phosphate is
a. Glycolysis
b. Photosynthesis
c. Oxidative phosphorylation
d. Citric acid cycle
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13. High energy phosphate storage forms are known as
a. Phosphagens
b. Phosphanogens
c. Pyruvates
d. Pyrinogens
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14. Many activation reactions are
a. Endergonic
b. Exergonic
c. Neither endergonic nor exergonic
d. Coupled endergonic and exergonic
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15. The free energy of biochemical reactions is denoted by
a. B
b. G
c. H
d. S
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16. The change in free energy as a result of a reaction is denoted by
a. ∆B
b. ∆K
c. ∆H
d. ∆G
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17. Reactions at equilibrium with respect to their free energies are denoted by
a. ∆G > 0
b. ∆G = 0
c. ∆G < 0
d. ∆G / 0
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18. Exergonic reactions with respect to their free energies are denoted by
a. ∆G > 0
b. ∆G = 0
c. ∆G < 0
d. ∆G / 0
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19. Endergonic reactions with respect to their free energies are denoted by
a. ∆G > 0
b. ∆G = 0
c. ∆G < 0
d. ∆G / 0
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20. The unit of energy is
a. kcal
b. mol
c. calories/mol
d. cal
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21. The useful energy that can be obtained from a reaction is termed
a. Entropy
b. Free energy
c. Enthalpy
d. Etrophy
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22. The net energy amount available from bonding changes of the reactants and
products is termed as
a. Entropy
b. Free energy
c. Enthalpy
d. Etrophy
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23. The change in the amount of order during a reaction is termed
a. Entropy
b. Free energy
c. Enthalpy
d. Etrophy
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24. Enthalpy is denoted by
a. ∆B
b. ∆K
c. ∆H
d. ∆G
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25. Entropy is denoted by
a. ∆B
b. ∆S
c. ∆H
d. ∆G
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26. The energy that a molecule must gain to undergo a reaction is called
a. Entropy
b. Enthalpy
c. Transition state
d. Free energy of activation
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27. A reaction with atom arrangement of reactants and products with highest
energy is termed
a. Free energy of activation
b. Transition state
c. Free energy
d. Equilibrium
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28. The first-order rate constant is represented by
a. k = v
b. v = k
c. v = k [A]
d. v = k [A][B]
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29. The second-order rate constant is represented by
a. k = v
b. v = k
c. v = k [A]
d. v = k [A][B]
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30. The zero-order rate constant is represented by
a. k = v
b. v = k
c. v = k [A]
d. v = k [A][B]
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31. The rate of reaction which depends on the substrate concentration is given by
a. First law of thermodynamics
b. Second law of thermodynamics
c. Rate law
d. Coulomb’s law
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32. The rate of first order reactions depend on
a. Concentration of substrate
b. Concentration of reactants
c. Concentration of both substrate and reactants
d. Concentration of neither the substrate nor reactants
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33. The rate of second order reactions depend on
a. Concentration of substrate
b. Concentration of reactants
c. Concentration of both substrate and reactants
d. Concentration of neither the substrate nor reactants
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34. The energy-rich state of ATP is due to the presence of
a. One phosphoanhydride bond in its triphosphate unit
b. Absence of phosphoanhydride bond in its triphosphate unit
c. Two phosphoanhydride bonds in its triphosphate unit
d. Three phosphoanhydride bond in its triphosphate unit
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35. The principle biological energy exchange mode is
a. GTP-CDP cycle
b. GTP-UDP cycle
c. CDT-CTP cycle
d. ATP-ADP cycle
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36. The hydrolysis of ATP to ADP yields
a. -14.8 kcal mol-1
b. -7.3 kcal mol-1
c. -5.0 kcal mol-1
d. -3.3 kcal mol-1
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37. The important source of cellular energy is
a. Oxidation of nitrogenous compounds
b. Reduction of nitrogenous compounds
c. Oxidation of carbon containing molecules
d. Reduction of carbon containing molecules
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38. The process where the exergonic clevage of ATP is used for the endergonic
biochemical processes is called
a. Catabolism
b. Anabolism
c. Energetic uncoupling
d. Energetic coupling
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39. One compound not similar to ATP is
a. GTP
b. MTP
c. CTP
d. UTP
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40. The membrane potential of resting cells is
a. -0.5 to -0.9 V
b. -0.03 to -0.07 V
c. -0.005 to -0.009 V
d. -0.05 to -0.09 V
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41. Proton gradient which is important for ATP synthesis is developed by
a. Hydroxyl ions
b. Hydronium ions
c. Carboxyl ions
d. Sodium ions
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42. The proton gradient across the inner mitochondrial membrane provides close
to
a. 24 kj/mol H+
b. 2.4 kj/mol H+
c. 0.24 kj/mol H+
d. 0.024 kj/mol H+
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43. The relationship between changes in free energy and entropy is expressed by
the equation
a. ∆G = ∆H + T∆S
b. ∆G = ∆H * T∆S
c. ∆G = ∆H-T∆S
d. ∆G = ∆H / T∆S
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44. The pH of biochemical reactions in a standard state of free energy change is
a. 9
b. 7
c. 5
d. 11
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45. The standard state free energy change is denoted by
a. kal
b. mol
c. ∆G0
d. ∆H
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46. The equilibrium constant from which the standard free energy change can be
calculated is denoted by
a. Keq
b. Eeq
c. Geq
d. Heq
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47. The standard free energy of hydrolysis of ADP is
a. -27.6 kj/mol
b. -27.6 kj/mol
c. -27.6 kj/mol
d. -27.6 kj/mol
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48. The standard free energy of hydrolysis of creatinine phosphate is
a. -4.31 kj/mol
b. -0.431 kj/mol
c. -43.1 kj/mol
d. -431 kj/mol
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49. The standard free energy of hydrolysis of pyrophosphate is
a. -51.4 kj/mol
b. -61.9 kj/mol
c. -43.1 kj/mol
d. -27.6 kj/mol
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50. The standard free energy of hydrolysis of glucose 1-phosphate is
a. -9.2 kj/mol
b. -20.9 kj/mol
c. -43.1 kj/mol
d. -13.8 kj/mol
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51. The standard free energy of hydrolysis of fructose 6-phosphate is
a. -9.2 kj/mol
b. -20.9 kj/mol
c. -15.9 kj/mol
d. -13.8 kj/mol

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52. The standard free energy of hydrolysis of AMP is
a. -14.2 kj/mol
b. -20.9 kj/mol
c. -43.1 kj/mol
d. -13.8 kj/mol
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53. The standard free energy of hydrolysis of glucose 6-phosphate is
a. -9.2 kj/mol
b. -20.9 kj/mol
c. -43.1 kj/mol
d. -13.8 kj/mol
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54. The standard free energy of hydrolysis of glycerol 3-phosphate is
a. -9.2 kj/mol
b. -20.9 kj/mol
c. -43.1 kj/mol
d. -13.8 kj/mol
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55. “High energy bond” is also refered to as
a. Action potential
b. Transfer potential
c. Group transfer potential
d. Action transfer potential
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56. The amount of heat required to raise the temperature of 1 gm of water from
14.5 °C to 15.5 °C is termed
a. Kilojoule (kJ)
b. Joule (J)
c. Calorie (cal)
d. Kilocalorie (kcal)