metabolism an introduction. energy every reaction that occurs in a living organism requires the use...
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MetabolismMetabolismAn Introduction
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EnergyEnergy
Every reaction that occurs in a living organism requires the use of Energy◦Energy = ability to do work
Metabolism: capture and use of energy through catabolic and anabolic reactions ◦ Catabolic reaction = breaking apart molecules into
simpler compounds Eg. Protein amino acids
◦ Anabolic reaction = building complex molecules out of smaller compounds
Eg. Glucose + glucose maltose
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Energy cont’dEnergy cont’d
Cells need a constant supply of energy in order to live
The nature of energy is important when considering metabolism
In metabolism, ATP molecules are the cell’s source of energy ATP = energy currency
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What does Energy look What does Energy look like?like?
Energy used to do work takes on many forms ◦ Electrical, kinetic, thermal, light,
sound
The types of energy fall into 2 categories:1.Kinetic energy- energy in
MOVING objects thermal (heat), mechanical,
electrical
2.Potential energy- STORED energy gravitational, chemical
Ex. Roller coaster car Top: potential
energy As drops: kinetic
energy
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Laws of thermodynamics Laws of thermodynamics (I)(I)
1st law:◦Total energy in a system always
remains constant ◦Energy is converted from on form to
another
• Metabolism- in the context of biochemical reactions in living cells, energy is constantly changing form and thermal energy is generally lost from the organism
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An interactive exampleAn interactive example
http://www.wiley.com/legacy/college/boyer/0470003790/animations/catalysis_energy/catalysis_energy.htm
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Free energy diagram
#1
Energy changes are what drive all chemical reactions
Free energy ( G) is the potential energy in a chemical reaction energy available to do work
#1- the reactants have a higher level of free energy than the products
Glucose
Carbon dioxide + water
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Free energy diagram
#2- a temporary state where both reactant bonds are breaking and product bonds are forming *intermediary step
The activation energy (Eact)is the jumpstart needed for reactions to proceed Needed to strain/break bonds
#2
Ex. Racket ball turning inside out
Glucose
Carbon dioxide + water
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http://www.wiley.com/legacy/college/boyer/0470003790/animations/catalysis_energy/catalysis_energy.htm
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Free energy diagram
#3- Decline in overall free energy as the free energy decreases in the reactants as they become products.
#3
Glucose
Carbon dioxide + water
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Free energy diagram
#4- Products have formed, the reaction is complete, the overall free energy has decline
#4
G is negative
Glucose
Carbon dioxide + water
An exothermic reaction
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In a living organism/cell, G < 0 in a reaction is harnessed to do useful work, leaving less free energy available & more entropy
What is entropy?
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What are some words you would use to describe the change in this room?
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Laws of thermodynamics Laws of thermodynamics (II)(II)2nd law:
◦The universe is constantly increasing in disorder As energy changes forms, it becomes more
disordered
◦Entropy is a measure of disorder Increased entropy = increase in disorder
When thinking of chemical reactions, we must consider both energy AND entropy◦Text pg 61
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Spontaneous vs Non-Spontaneous vs Non-Spontaneous ReactionsSpontaneous Reactions
◦Chemical reactions occur spontaneously when both energy & entropy are favoured
◦Chemical reactions may not occur spontaneously if energy is favoured but entropy is not
◦In summary- cells favour spontaneous reactions
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• Less entropy• More free energy
• More entropy• Less free energy
ATP ↔ ADP + Pi
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HomeworkPg 68 #1, 2, 3, 5, 6
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ResourcesResources
http://www.accessexcellence.org/RC/VL/GG/ecb/ecb_images/03_32_ATP_and_ADP_cycle.jpg