Download CHAPTER 10 REVIEW SHEET Briefly describe metabolism. What

CHAPTER 10 REVIEW SHEET
1. Briefly describe metabolism. What governs its processes?
2. What are metabolites?
3. Differentiate between anabolic and catabolic reactions.
4. Summarize the common metabolic themes that all organisms demonstrate.
5. How is a metabolic pathway similar to a synthesis scheme in organic chemistry?
6. Exemplify a linear, cyclic and spiral metabolic pathway.
7. The fact that pathways proceed via multiple steps helps to control what? How do they
adjust to changing environmental conditions?
8. Describe the steady state of metabolic reactions.
9. Draw diagrams that exemplify the difference between feedback inhibition and feedforward activation.
10. Briefly describe the major roles of anabolism and catabolism.
11. Differentiate between autotrophs and heterotrophs.
12. For what does compartmentation of metabolism allow? Where does it occur?
Match the location of the metabolic processes.
_____ 13. Cytosol
A. Nucleic acid synthesis
_____ 14. Mitochondrion
B. Delivery of proteins, synthesis of lipids for
membranes
_____ 15. Endoplasmic reticulum
_____ 16. Nucleus
C. Fatty acid synthesis, glycolysis,
gluconeogenesis, pentose phosphate pathway, etc.
_____ 17. Golgi apparatus
D. Sorting and secretion of some proteins
E. Citric acid cycle, oxidative phosphorylation,
fatty acid degradation
18. What is the equation that relates standard Gibbs free energy to actual Gibbs free energy?
19. What is the equation that relates Gibbs free energy to the equilibrium constant?
20. What is the main condition that changes most cellular free energies from being
nonspontaneous to being spontaneous?
21. If Q and K are close, the metabolic reaction is __________-_______________. If they
are far apart, then the reaction is _______________, and is usually _______________ in
some way as a __________ point in the pathway.
22. Predict the products:
a. ATP + H2O 
G° = –32 kJ/mol
b. ATP + H2O 
G° = –45 kJ/mol
23. Which complex is favored in aqueous solution: the  complex of MgATP or the 
complex of MgATP?
24. What three reasons explain why a large amount of energy is released during the
hydrolysis of the phosphoanhydride linkages of ATP?
25. A series of __________ (or phosphotransferases) catalyze interconversions of nucleoside
mono-, di- and triphosphates. Predict the products:
a. GMP + ATP
guanylate kinase
b. GDP + ATP
nucleoside diphosphate kinase
26. Intracellular ATP concentrations is maintained by the following two reactions. Predict
the products:
a. AMP + ATP
, which is then converted to ATP.
adenylate kinase
b. The overall process is shown here: AMP + ATP + 2 Pi
27. Exemplify how the Gibbs free energy change for ATP hydrolysis in vivo is greater than
the standard Gibbs free energy change given [ATP] = 3.8 mM, [ADP] = 0.9 mM and [Pi]
= 5.2 mM for a particular organism. Assume 25°C and pH = 7.0.
ATP  ADP + Pi
G° = –32 kJ/mol
28. Calculate the equilibrium constant for the hydrolysis of ATP under standard conditions
and in the cellular situation in #27.
29. Show using reaction equations the coupling a nonspontaneous reaction with the
hydrolysis of ATP to drive the reaction.
30. Exemplify the use of phosphoryl-group transfer from ATP to synthesize glutamine from
glutamate.
31. Describe the activity of phosphagens in muscles.
32. Exemplify ATP’s ability to transfer a nucleotidyl group by showing the synthesis of
acetyl CoA. What side reaction contributes to the negative Gibb’s free energy?
33. Exemplify the action of phosphoenolpyruvate with pyruvate kinase to produce ATP.
How are almost –30 kJ/mol released during the process?
34. Identify an example of a thioester. What two processes are driven by the release of
energy from the hydrolysis of this molecule? Write an equation for this process.
35. Molecule A donates a H– ion or a H atom to molecule B. Which is oxidized? Which is
reduced? Which is the oxidizing agent? Which is the reducing agent?
36. What is the equation that relates Gibbs free energy to cell potential?
37. Calculate the standard Gibbs free energy change for the following reaction using the table
of reduction potentials. Is the reaction spontaneous or nonspontaneous?
EtOH + oxaloacetate  acetaldehyde + malate
38. What is the equation that relates standard cell potential to actual cell potential?
39. Using the standard cell potential from #37 and the given concentrations under cellular
conditions, calculate the cellular cell potential assuming 25°C and pH = 7.0.. Is the
reaction under cellular conditions more or less spontaneous?
[EtOH] = 1.01 mM
[oxaloacetate] = 0.75 mM
[acetaldehyde] = 4.97 mM
[malate] = 3.78 mM
40. Describe the classical approach to studying a metabolic pathway. How can NMR be
used in the process? How are the steps verified?
41. How are mutations in single genes used to study a metabolic pathway? What if natural
mutations are not available? What process can be used to modify enzymes in a pathway
to study them?
42. How can inhibitory drugs be used to study a metabolic pathway?