chapter 6 an introduction to metabolism n.
Download
Skip this Video
Loading SlideShow in 5 Seconds..
Chapter 6 An Introduction To Metabolism PowerPoint Presentation
Download Presentation
Chapter 6 An Introduction To Metabolism

Loading in 2 Seconds...

play fullscreen
1 / 43

Chapter 6 An Introduction To Metabolism - PowerPoint PPT Presentation


  • 195 Views
  • Uploaded on

Chapter 6 An Introduction To Metabolism. Metabolism/Bioenergetics. Metabolism : The totality of an organism’s chemical processes; managing the material and energy resources of the cell Catabolic pathways : degradative process such as cellular respiration; releases energy

loader
I am the owner, or an agent authorized to act on behalf of the owner, of the copyrighted work described.
capcha
Download Presentation

Chapter 6 An Introduction To Metabolism


An Image/Link below is provided (as is) to download presentation

Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author.While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server.


- - - - - - - - - - - - - - - - - - - - - - - - - - E N D - - - - - - - - - - - - - - - - - - - - - - - - - -
Presentation Transcript
metabolism bioenergetics
Metabolism/Bioenergetics
  • Metabolism: The totality of an organism’s chemical processes; managing the material and energy resources of the cell
  • Catabolic pathways: degradative process such as cellular respiration; releases energy
  • Anabolic pathways: building process such as protein synthesis; photosynthesis; consumes energy
thermodynamics
Thermodynamics
  • Energy (E)~ capacity to do work;
  • Kinetic energy~ energy of motion;
  • Potential energy~ stored energy
  • Thermodynamics~ study of E transformations
  • 1st Law: conservation of energy;

E transferred/transformed, not created/destroyed

  • 2nd Law: transformations increase entropy (disorder, randomness)
  • quantity of E is constant, quality is not
free energy
Free Energy
  • Free energy: portion of system’s E that can perform work (at a constant T)
  • Exergonic reaction: net release of free E to surroundings
  • Endergonic reaction: absorbs free E from surroundings
free energy equation
Free Energy Equation

Organisms live at the expense of free energy.

The amount of energy available to do work.

G = H - TS

G = free energy

H = enthalpy or total energy

T = temperature in 0K

S = entropy (disorder/randomness)

significance of free energy
Significance of Free Energy

Indicates whether a reaction will occur spontaneously

or not.

In a spontaneous reaction, G decreases, DG<0 (negative)

EXERGONIC REACTIONENDERGONIC REACTION

Products have less G Products have more G

Reaction is ‘downhill’ Reaction is ‘uphill’

Spontaneous Require energy input

DG is negative DG is positive

metabolic disequilibrium
Metabolic Disequilibrium

Many metabolic reactions are reversible and reach

equilibriuim.

At equilibrium a cell is dead!

Disequilibrium is maintained by the continual use/removal

of products e.g. respiration

energy coupling atp
Energy Coupling & ATP
  • E coupling: use of exergonic process to drive an endergonic one (ATP)
  • Adenosine triphosphate
  • ATP tail: high negative charge
  • ATP hydrolysis: release of free E
  • Phosphorylation (phosphorylated intermediate)~ enzymes
chemical reactions
Chemical Reactions

Animation 6.1.1

enzymes
Enzymes
  • Catalytic proteins: change the rate of reactions w/o being consumed
  • Free E of activation (activation E): the E required to break bonds
  • Substrate: enzyme reactant
  • Active site: pocket or groove on enzyme that binds to substrate
  • Induced fit modelbinding of substrate changes shape of the active site so that the substrate can bind
enzyme properties
Enzyme Properties
  • Are proteins
  • Lower the activation energy of a reaction –
  • transition state can be reached at cellular temperatures.
  • Do not change the nature of the reaction –
  • only speed up a reaction that would have occurred anyway.
  • Are very selective for which reaction they will catalyze
  • Substrate + enzyme
  • enzyme-substrate complex
  • product + enzyme
how an enzyme lowers activation energy
How an Enzyme Lowers Activation Energy
  • Active site holds 2 or more reactants.
  • Induced fit distorts bonds-less E required to break them.
  • Active site may produce a micro-environment.
  • Side chains of amino acids may participate.
how enzymes work
How Enzymes Work

Animation 6.1.6

http://www.chem.ufl.edu/~itl/2045/lectures/lec_m.html

initial substrate conc determines rate of an enzyme controlled reaction
Initial Substrate Conc. Determines Rate of an Enzyme-Controlled Reaction
  • The higher the substrate conc. the faster the reaction
  • If the substrate concentration is high enough –
  • the enzyme may become saturated, reaction will slow
  • Reaction rate may be increased by adding more enzyme.
effects on enzyme activity
Effects on Enzyme Activity
  • Temperature
  • pH
  • Cofactors:

inorganic, nonprotein

helpers;

e.g. zinc, iron, copper

  • Coenzymes:

organic helpers;

e.g. vitamins

enzyme inhibitors
Enzyme Inhibitors
  • Irreversible (covalent); Reversible (weak bonds)
  • Competitive: competes for active site (reversible); mimics the substrate
  • Noncompetitive: bind to another part of enzyme (allosteric site) altering its conformation (shape); poisons, antibiotics
allosteric regulation
Allosteric Regulation

Allosteric enzymes have two conformations, one

catalytically active, the other inactive.

Binding of an activator to the allosteric site stabilizes

the active conformation of the enzyme

Binding of an inhibitor to the allosteric site stabilizes

the inactive form of the enzyme (non-competitive)

cooperativity
Cooperativity

Binding at one site enhances binding at other sites

slide31

Each enzyme is specific for the reaction it will catalyze. In this laboratory,Enzyme = catalase Substrate = hydrogen peroxide (H2O2)Products = water and oxygen H2O2 H2O + O2

If a small amount of catalase is added to hydrogen peroxide, you will be able to observe bubbles of oxygen forming.

slide32
To determine the amount of hydrogen peroxide that remains after the reaction, you will do a titration with KMnO4.

In such a titration, you slowly add a chemical (KMnO4) that will cause a color change until a target is achieved.

slide33

To determine how much hydrogen peroxide (substrate) has been broken down by catalase at varying times, you measure the amount of peroxide remaining in each flask.

slide35
Analysis of ResultsEnzyme Action Over Time

We can calculate the rate of a reaction by measuring, over time, either the disappearance of substrate or the appearance of product.

For example, on the graph above, what is the rate, in moles/second, over the interval from 0 to 10 seconds?

Rate = Dx = 7-0 moles = 7 = 0.7 mols/sec

Dy 10-0 seconds 10

slide37
After 40 seconds there were no more substrate molecules. The curve becomes flat at this point, and the rate is zero.
slide38

During what time interval is the enzyme working at its maximum velocity?

a. 0–30 seconds

b. 60–120 seconds

c. 120–180 seconds

d. Over the entire time course

slide39

In order to keep the rate constant over the entire time course, which of the following should be done?

  • Add more enzyme.
  • Gradually increase the temperature after 60 seconds.
  • Add more substrate
  • Add H2SO4 after 60 seconds.
  • Remove the accumulating product.
slide40

Which of the following graphs represents the rate of the reaction shown above? Notice that in the graphs below, the y-axis is number of molecules/sec.

what is the role of sulfuric acid h2so4 in this experiment
What is the role of sulfuric acid (H2SO4) in this experiment?

a. It is the substrate on which catalase acts

b. It binds with the remaining hydrogen peroxide during titration

c. It accelerates the reaction between enzyme and substrate

d. It blocks the active site of the enzyme

e. It denatures the enzyme by altering the active site

slide42

A student was performing a titration for this laboratory, and accidentally exceeded the endpoint. What would be the best step to obtain good data for this point?

a. Estimate the amount of KMnO4 that was in excess, and subtract this from the result

b. Repeat the titration using the reserved remaining sample.

c. Obtain data for this point from another lab group

d. Prepare a graph of the data without this point, and then read the estimated value from the graph.