Question 1

Which of the following is an example of a system?

Accepted Answer

A)  the universe 
B)  the air 
C)  a test tube with reaction components 
D)  outer space 
A)  the universe 
B)  the air 
C)  a test tube with reaction components 
D)  outer space C

Question 2

The oxidation of glucose releases 15.7 kJ/g. Is this reaction spontaneous?

Accepted Answer

A)  Yes, because it is exothermic. 
B)  No, because it is exothermic. 
C)  Yes, because it is endothermic. 
D)  The answer cannot be determined. 
A)  Yes, because it is exothermic. 
B)  No, because it is exothermic. 
C)  Yes, because it is endothermic. 
D)  The answer cannot be determined. D

Question 3

Using the figure below, which of the following best describes the titration curve?

Accepted Answer

A)  The equivalence point for the titration is pH = 7. 
B)  The midpoint of the titration is pH = 7. 
C)  The pKa for this weak acid is 4.76. 
D)  This is a titration of a weak base by NaOH. 
A)  The equivalence point for the titration is pH = 7. 
B)  The midpoint of the titration is pH = 7. 
C)  The pKa for this weak acid is 4.76. 
D)  This is a titration of a weak base by NaOH. C

Question 4

Which of the following best describes an open system?

Accepted Answer

A)  Matter and energy are freely exchanged with the surroundings. 
B)  Energy is exchanged with the surroundings but matter is not. 
C)  Matter is exchanged with the surroundings but energy is not. 
D)  Neither matter nor energy is exchanged with the surroundings. 
A)  Matter and energy are freely exchanged with the surroundings. 
B)  Energy is exchanged with the surroundings but matter is not. 
C)  Matter is exchanged with the surroundings but energy is not. 
D)  Neither matter nor energy is exchanged with the surroundings.

Question 5

Differentiate between autotrophs and heterotrophs.

Accepted Answer

Autotrophs convert s

Question 6

If a reaction has a $\Delta$H $\gt$ 0 and a $\Delta$S $\lt$ 0, then __________ and the reaction is at all temperatures.

Accepted Answer

A)  "$\Delta$G $\lt$ 0; spontaneous" 
B)  "$\Delta$G $\gt$ 0; spontaneous" 
C)  "$\Delta$G$\lt$ 0; nonspontaneous" 
D)  "$\Delta$G $\gt$ 0; nonspontaneous" 
A)  "$\Delta$G $\lt$ 0; spontaneous" 
B)  "$\Delta$G $\gt$ 0; spontaneous" 
C)  "$\Delta$G$\lt$ 0; nonspontaneous" 
D)  "$\Delta$G $\gt$ 0; nonspontaneous"

Question 7

The interaction between an amino group and a carboxylate group is best characterized as

Accepted Answer

A)  hydrogen bonds. 
B)  ionic interactions. 
C)  van der Waals interactions. 
D)  a covalent bond. 
A)  hydrogen bonds. 
B)  ionic interactions. 
C)  van der Waals interactions. 
D)  a covalent bond.

Question 8

How are polar molecules like glucose transported across a membrane?

Accepted Answer

A)  There are holes in the membrane. 
B)  There are proteins that allow the transportation of polar molecules across the membrane. 
C)  Polar molecules cannot ever enter the cell. 
D)  Polar molecules diffuse across the hydrophobic barrier. 
A)  There are holes in the membrane. 
B)  There are proteins that allow the transportation of polar molecules across the membrane. 
C)  Polar molecules cannot ever enter the cell. 
D)  Polar molecules diffuse across the hydrophobic barrier.

Question 9

Calculate the concentration of pH of a 0.023 M HCl solution.

Accepted Answer

A)  12.36 
B)  3.68 
C)  1.64 
D)  2.30 
A)  12.36 
B)  3.68 
C)  1.64 
D)  2.30

Question 10

The example of water freezing into ice shows

Accepted Answer

A)  an increase in entropy of the system. 
B)  a decrease in entropy of the system. 
C)  no change in the entropy of the system. 
D)  a decrease in the entropy of the surroundings. 
A)  an increase in entropy of the system. 
B)  a decrease in entropy of the system. 
C)  no change in the entropy of the system. 
D)  a decrease in the entropy of the surroundings.

Question 11

Limonene is a nonpolar molecule. The water molecules around it forms

Accepted Answer

A)  hydrogen bonds with itself and entropy decreases. 
B)  ionic bonds with itself and the entropy decreases. 
C)  hydrogen bonds with limonene and the entropy increases. 
D)  covalent bonds with limonene and entropy increases. 
A)  hydrogen bonds with itself and entropy decreases. 
B)  ionic bonds with itself and the entropy decreases. 
C)  hydrogen bonds with limonene and the entropy increases. 
D)  covalent bonds with limonene and entropy increases.

Question 12

Compare the reaction conditions for $\Delta$G$\degree$ and $\Delta$G$\degree$ ' .

Accepted Answer

@#LAT-DLM&G@#LAT-DLM& is the standard free energy change and

Question 13

If a reaction has a $\Delta$ H $\lt$ 0 and $\Delta$ S $\lt$ 0, under which conditions would the reaction be spontaneous in the forward direction?

Accepted Answer

A)  low temperatures 
B)  high temperatures 
C)  high pressure 
D)  low pressure 
A)  low temperatures 
B)  high temperatures 
C)  high pressure 
D)  low pressure

Question 14

If the equilibrium constant (Keq) is greater than 1, which direction will the reaction proceed?

Accepted Answer

A)  spontaneously to products 
B)  spontaneously to reactants 
C)  neither direction 
D)  Not enough information is given to determine the direction of reaction. 
A)  spontaneously to products 
B)  spontaneously to reactants 
C)  neither direction 
D)  Not enough information is given to determine the direction of reaction.

Question 15

The transfer of a phosphate from ATP to another molecule produces a(n)

Accepted Answer

A)  low-energy intermediate. 
B)  highly reactive intermediate. 
C)  neutral energy intermediate. 
D)  It is not possible to transfer a phosphate to another molecule. 
A)  low-energy intermediate. 
B)  highly reactive intermediate. 
C)  neutral energy intermediate. 
D)  It is not possible to transfer a phosphate to another molecule.

Question 16

The interaction between nonpolar molecules is best characterized as

Accepted Answer

A)  a hydrogen bond. 
B)  ionic interactions. 
C)  van der Waals interactions. 
D)  a covalent bond. 
A)  a hydrogen bond. 
B)  ionic interactions. 
C)  van der Waals interactions. 
D)  a covalent bond.

Question 17

A solution of which of the following would be a good buffer system?

Accepted Answer

A)  HCl and NaOH 
B)  HCl and H2O 
C)  CH3COOH and NaCH3COO 
D)  NaOH and KOH 
A)  HCl and NaOH 
B)  HCl and H2O 
C)  CH3COOH and NaCH3COO 
D)  NaOH and KOH

Question 18

Osmosis occurs when water diffuses through a

Accepted Answer

A)  semipermeable membrane from high water to low water concentration. 
B)  nonpermeable membrane from high water to low water concentration. 
C)  semipermeable membrane from low water to high water concentration. 
D)  semipermeable membrane from high solute to low solute concentration. 
A)  semipermeable membrane from high water to low water concentration. 
B)  nonpermeable membrane from high water to low water concentration. 
C)  semipermeable membrane from low water to high water concentration. 
D)  semipermeable membrane from high solute to low solute concentration.

Question 19

If serum pH falls blow pH 7.4, a condition called acidosis, how does the body respond?

Accepted Answer

The equilibrium of the carbonic acid-bic

Question 20

Given a biological system at 1 atm with $\Delta$ H = 16 kJ/g, what is the internal energy of the system?

Accepted Answer

A)  15 kJ/g 
B)  16 kJ/g 
C)  14 kJ/g 
D)  Not enough information is given to calculate the answer. 
A)  15 kJ/g 
B)  16 kJ/g 
C)  14 kJ/g 
D)  Not enough information is given to calculate the answer.

Exam 2: Physical Biochemistry: Energy Conversion, Water, and Membranes

Which of the following is an example of a system?

The oxidation of glucose releases 15.7 kJ/g. Is this reaction spontaneous?

Using the figure below, which of the following best describes the titration curve?

Which of the following best describes an open system?

Differentiate between autotrophs and heterotrophs.

If a reaction has a Δ\DeltaΔ H >\gt> 0 and a Δ\DeltaΔ S <\lt< 0, then __________ and the reaction is at all temperatures.

The interaction between an amino group and a carboxylate group is best characterized as

How are polar molecules like glucose transported across a membrane?

Calculate the concentration of pH of a 0.023 M HCl solution.

The example of water freezing into ice shows

Limonene is a nonpolar molecule. The water molecules around it forms

Compare the reaction conditions for Δ\DeltaΔ G °\degree° and Δ\DeltaΔ G °\degree° ' .

If a reaction has a Δ\DeltaΔ H <\lt< 0 and Δ\DeltaΔ S <\lt< 0, under which conditions would the reaction be spontaneous in the forward direction?

If the equilibrium constant (Keq) is greater than 1, which direction will the reaction proceed?

The transfer of a phosphate from ATP to another molecule produces a(n)

The interaction between nonpolar molecules is best characterized as

A solution of which of the following would be a good buffer system?

Osmosis occurs when water diffuses through a

If serum pH falls blow pH 7.4, a condition called acidosis, how does the body respond?

Given a biological system at 1 atm with Δ\DeltaΔ H = 16 kJ/g, what is the internal energy of the system?

Principles of Biochemistry

Nucleic Acid Structure and Function

Protein Structure

Methods in Protein Biochemistry

Protein Function

Enzyme Mechanisms

Cell Signaling Systems

Glycolysis: a Paradigm of Metabolic Regulation

The Citrate Cycle

Oxidative Phosphorylation

Photosynthesis

Carbohydrate Structure and Function

Carbohydrate Metabolism

Lipid Structure and Function

Lipid Metabolism

Amino Acid Metabolism

Nucleotide Metabolism

Metabolic Integration

DNA Replication, Repair, and Recombination

RNA Synthesis, Processing, and Gene Silencing

Protein Synthesis, Posttranslational Modification, and Transport

Gene Regulation

Filters

If a reaction has a $\Delta$ H $\gt$ 0 and a $\Delta$ S $\lt$ 0, then __________ and the reaction is at all temperatures.

Compare the reaction conditions for $\Delta$ G $\degree$ and $\Delta$ G $\degree$ ^' .

If a reaction has a $\Delta$ H $\lt$ 0 and $\Delta$ S $\lt$ 0, under which conditions would the reaction be spontaneous in the forward direction?

If the equilibrium constant (K_eq) is greater than 1, which direction will the reaction proceed?

Given a biological system at 1 atm with $\Delta$ H = 16 kJ/g, what is the internal energy of the system?