FULL CHAPTERS TESTBANK For Biochemistry An Integrative Approach with Expanded Topics 1st Edition John T. Tansey

, Testbank For Biochemistry An Integrative
Approach with Expanded Topics 1st Edition
John T. Tansey
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,Tansey Test Bank, Chapter 1: The Chemical Foundations of Biochemistry

MULTIPLE CHOICE
1. If a reaction at 37C has a H of 23 kJ/mol and a S of 337 J/K•mol, what is the G for the reaction?
A) 65 kJ/mol
B) –42 kJ/mol
C) 18 kJ/mol
D) –19 kJ/mol
E) none of the above
Answer: D
Difficulty: Moderate
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
2. The second law of thermodynamics states ______.
A) that spontaneous processes are characterized by the overall conversion of order to disorder
B) that spontaneous processes are characterized by the conversion of work to force
C) that nonspontaneous processes are characterized by the conversion of order to disorder
D) that spontaneous processes are characterized by the conversion of heat to pressure
E) none of the above
Answer: A
Difficulty: Easy
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
3. Change in enthalpy (H) is best defined as ______.
A) the sum of heat absorbed and work done
B) the heat transferred at constant pressure
C) the pressure change at constant temperature
D) the measure of disorder in a system
E) none of the above
Answer: B
Difficulty: Easy
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
4. A reaction with a ______ H and a ______ S will never be spontaneous.
A) positive, positive
B) positive, negative
C) negative, positive
D) negative, negative
E) none of the above
Answer: B
Difficulty: Moderate
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
5. Calculate the G for a reaction with H = 20. kJ/mol and S = 20. J/K•mol that is carried out at 27°C.
A) 14 J/mol

,B) 140 J/mol
C) 1,400 J/mol
D) 14,000 J/mol
E) none of the above
Answer: D
Difficulty: Moderate
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
6. A spontaneous process ______.
A) occurs without the addition of free energy
B) has a G < 0
C) is exergonic
D) is all of the above
E) is none of the above
Answer: D
Difficulty: Easy
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MATCHING:
A) phylogenetic
B) negative
C) H2O
D) H°
E) H – TS
F) halobacteria
G) open
H) entropy
I) flux
J) polymers
K) G°ꞌ
L) thermophiles
M) nitrogen
N) positive

7. The term used to indicate the degree of randomness within a system is ______.
Answer: H
Difficulty: Easy
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

8. Spontaneous processes are characterized by a change in Gibbs free energy that is ______.
Answer: B
Difficulty: Easy
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

9. Gibbs free energy is defined as G = ______.
Answer: E
Difficulty: Easy
Section: 1.1

,Learning objective: Basic principles of thermodynamics describe all systems

10. The symbol for free energy under standard biochemical conditions is ______.
Answer: K
Difficulty: Easy
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

11. Living creatures can be described thermodynamically as ______ systems.
Answer: G
Difficulty: Easy
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
12. An endergonic reaction with a ______ H and a ______ S can be changed into an exergonic reaction by decreasing
the temperature.
A) positive, positive
B) positive, negative
C) negative, positive
D) negative, negative
Answer: D
Difficulty: Moderate
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
13. For a reaction with H = 23 kJ/mol and S = 22 J/K•mol, at 2°C, the reaction is ______.
A) spontaneous
B) nonspontaneous
C) at equilibrium
D) impossible to determine reactivity
E) none of the above
Answer: B
Difficulty: Moderate
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
14. An increase in disorder in the system ______.
A) is required for a process to be spontaneous
B) results in a decrease in entropy
C) is characteristic of a system increasing in enthalpy
D) results in the factor TS being positive
E) is found in every exergonic process
Answer: D
Difficulty: Moderate
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

SHORT ANSWER
15. Consider a reaction in which H = -20. kJ/mol and S = 10. J/mol · K.
a. Calculate the G for this reaction at 25°C.

, b. Is the reaction spontaneous (explain your answer)?
Answer: a. G = H − TS  G = –20,000 J/mol – (298 × 10 J/mol) = −23,000 J/mol
b. The reaction is spontaneous because the G is negative.
Difficulty: Moderate
Section 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
16. Of the following amino acids, which contains an alcohol?




A B C D
A) A
B) B
C) C
D) D
E) all of the above
Answer: A
Difficulty: Easy
Section: 1.1
Learning Objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
17. What functional groups are present in the following molecule?




A) amine and carboxylic acid
B) amine, ketone, and carboxylic acid
C) amine, amide, and carboxylic acid
D) alcohol, amine, amide, and carboxylic acid
E) none of the above are correct
Answer: C
Difficulty: Medium
Section: 1.1
Learning Objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
18. Keq can be determined from the change in standard free energy using the equation ______.
A) Keq = e−G°/RT
B) Keq = ln e−G°/TS
C) Keq = e−H/RT

,D) Keq = e−G°/TS
E) Keq = log e−G°/RT
Answer: A
Difficulty: Easy
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
19. Consider the reaction A + B  C + D. After reaching equilibrium at 25°C, the following concentrations of reactants
and products were measured: [A] = 10 µM, [B] = 15 µM, [C] = 10 µM, [D] = 10 µM. Calculate ∆G°ꞌ for this reaction.
A) 1,000 J/mol
B) 10 kJ/mol
C) 1 J/mol
D) insufficient data to determine answer
E) none of the above
Answer: A
Difficulty: Moderate
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

SHORT ANSWER
20. Consider the isomerization reaction R  P, in which R is converted to P. The G°ꞌ for this reaction is −10. kJ/mol.
Calculate the [P]/[R] at equilibrium at 25°C.
Answer: At equilibrium [P]/[R] = Keq = e−G°/RT  [P]/[R] = e− -(−-10000 J/mol)/8.3145 × 298 J/mol =
e10000/8.3145 × 298 = 57
Difficulty: Moderate
Section 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

SHORT ANSWER
21. Phosphoglucomutase catalyzes the reaction in which a phosphate group is transferred from the C-1 of glucose to the
C-6 of glucose (G1P  G6P). A student incubates a 0.2 M solution of glucose-1-phosphate overnight with a small amount
of the enzyme. At equilibrium the concentration of glucose-1-phosphate is 9.0 × 10−3 M and the concentration of
glucose-6-phosphate is 19.1 × 10−2 M.
Calculate the equilibrium constant (Keq) and the standard state free energy (∆G°ꞌ) for this reaction at 25°C.
Answer: The equilibrium constant Keq = [G6P]eq/[G1P]eq = 19.1 × 10−2 M/ 9.0 × 10−3 M = 21.
G°ꞌ = −RTlnKeq = −8.3145 × 298 J/mol × ln 21.2 = −7,600 J/mol.
Difficulty: Difficult
Section 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

MULTIPLE CHOICE
22. Enzymes accelerate biochemical reactions by ______.
A) decreasing the ∆G for the reactions
B) increasing the ∆G for the reactions
C) establishing a “closed system” for each reaction
D) promoting reaction pathways associated with a positive ∆G
E) providing a more favorable pathway for the reactions
Answer: E
Difficulty: Moderate
Section: 1.1
Learning objective: Apply the basic principles of thermodynamics, equilibrium, and kinetics to biological systems.

,For questions 23–26, consider the structure of the coenzyme NADP.

O
B
O NH 2


O P O N

A H
O
H
O
H H
OH OH NH2
O P O
N
C
N
O
N
N


H
O
H
D
H H
OH O
E
O P O

O

MULTIPLE CHOICE
23. Which arrow points at a phosphoester bond?
A) A
B) B
C) C
D) D
E) E
Answer: E
Difficulty: Easy
Section: 1.2
Learning objective: Describe biological molecules and processes using the tools of organic chemistry.

MULTIPLE CHOICE
24. Which arrow points at an amide bond?
A) A
B) B
C) C
D) D
E) E
Answer: B
Difficulty: Easy
Section: 1.2
Learning objective: Describe biological molecules and processes using the tools of organic chemistry.

MULTIPLE CHOICE
25. Which arrow points at a phosphoanhydride bond?
A) A
B) B
C) C

,D) D
E) E
Answer: A
Difficulty: Moderate
Section: 1.2
Learning objective: Describe biological molecules and processes using the tools of organic chemistry.

MULTIPLE CHOICE
26. In a water molecule, hydrogens are partially _____; oxygens are partially _____.
A) negative; negative
B) negative; positive
C) positive; positive
D) positive; negative
E) none of the above
Answer: D
Difficulty: Easy
Section: 1.3
Learning Objective: Perform basic calculations pertaining to the chemistry of water and aqueous systems.

MULTIPLE CHOICE
27. Due to the formation of hydrogen bonds, _____ is highly soluble in water.
A) carbon dioxide
B) sodium chloride
C) methanol
D) octane
E) cholesterol
Answer: C
Difficulty: Medium
Section: 1.3
Learning Objective: Perform basic calculations pertaining to the chemistry of water and aqueous systems.

MULTIPLE CHOICE
28. Which of the following explains the interactions that occur between the atoms of water molecules and the ions that
form when sodium chloride dissolves in water?
A) Hydrogens interact with the sodium ion; oxygens interact with the chloride ion.
B) Hydrogens interact with the chloride ion; oxygens interact with the sodium ion.
C) Hydrogens interact with the sodium ion and the chloride ion.
D) Oxygens interact with the sodium ion and the chloride ion.
E) none of the above
Answer: B
Difficulty: Medium
Section: 1.3
Learning Objective: Perform basic calculations pertaining to the chemistry of water and aqueous systems.

TEXT ENTRY
29. The 104.5° bond angle in the water molecule is the result of the ______ of electron orbitals around oxygen.
Answer: tetrahedral arrangement
Difficulty: Easy
Section: 1.3
Learning objective: Perform basic calculations pertaining to the chemistry of water and aqueous systems.

TEXT ENTRY
30. The polarity of the O–H bond is caused by the ______ of oxygen relative to that of hydrogen.

, Answer: higher electronegativity
Difficulty: Easy
Section: 1.3
Learning objective: Perform basic calculations pertaining to the chemistry of water and aqueous systems.

MULTIPLE CHOICE
31. Which of the following statements about water is not true?
A) It has a high dielectric constant.
B) It dissolves salts and polar substances.
C) It can form two hydrogen bonds per water molecule.
D) It packs in a hexagonal- (honeycomb-) shaped lattice when the temperature falls below 0°C.
E) In the liquid state it is only 15% less hydrogen bonded than in the solid state at 0°C.
Answer: C
Difficulty: Easy
Section: 1.3
Learning objective: Perform basic calculations pertaining to the chemistry of water and aqueous systems.

MULTIPLE CHOICE
32. In a hydrogen bond between a water molecule and another biomolecule, _____.
A) a hydrogen ion on the water molecule forms an ionic bond with a hydride ion on the other molecule
B) the hydrogen bond will typically form between a hydrogen atom and either a nitrogen, sulfur, or oxygen atom
C) the partial charge on a hydrogen of the water interacts with the partial charge on a hydrogen of the other molecule
D) a hydrogen on the water molecule forms a covalent bond to an oxygen or nitrogen atom on the other molecule
E) the hydrogen atom is located between an oxygen atom of the water and a carbon atom of the other molecule
Answer: B
Difficulty: Medium
Section: 1.3
Learning Objective: Perform basic calculations pertaining to the chemistry of water and aqueous systems.

MULTIPLE CHOICE
33. Which of the following is a physical property of water that results from hydrogen bonding?
A) a high boiling point relative to molecular weight
B) a solid state that is less dense than the liquid state
C) high surface tension
D) the ability to solubilize polar molecules
E) all of the above
Answer: E
Difficulty: Medium
Section: 1.3
Learning Objective: Perform basic calculations pertaining to the chemistry of water and aqueous systems.

MULTIPLE CHOICE
34. Which of the following functional groups has two hydrogen bond donors and one hydrogen bond acceptor?
A) alcohol
B) ester
C) thiol
D) amine
E) amide
Answer: D
Difficulty: Difficult
Section: 1.3
Learning Objective: Perform basic calculations pertaining to the chemistry of water and aqueous systems.