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Chapter 8 - Coggle Diagram
Chapter 8
Free energy change
Free energy
energy available to do work
At constant temp/pressure
-ΔG
spontaneous reaction
releases free energy
system becomes more stable
Free energy equation
ΔG = ΔH – TΔS
ΔH = enthalpy (total energy)
ΔS = entropy (disorder)
T = temperature (Kelvin)
+ΔG
nonspontaneous reaction
requires energy
stabiltity
higher ΔG
unstable
Lower ΔG
more stable
Equilibrium
forward = reverse reaction
max stability
no net charge
Exergonic reactions
Energy outward
products have less energy
endergonic reactions
energy inward
products have more energy
Enzymes
Catalyst
Speeds reactions
Enzyme
proteiin that is a catalyst
specific reaction
Lowers activation enegy
Speed up chemical reactions
reusable
enzyme changes shape to bond
EA
Enegy required to start reacton
reach transition state
Substate
Reactant molecule
Binds to enzyme
Active site
where substate binds./ specific shape
Enzyme substrate complex
temporary binding
product fomation
Factors effecting enzyme
Substrate concetration
increase rate
until saturation
temperature
increase rate
high temperature cause denaturation
ph
optimal ph required
high ph can cause denaturation
Regulation
Cofactors
non protein helpers
inorgainc
organinc= coenzymes
Enzyme Inhibitors
Noncompetitive Inhibitors
bind elsewhere
change enzyme shape
cannot overcome
lowers enzyme activity
competitive inhibitors
bind active site
resemble substrate
can overcome
Allosteric Regulation
regulator binds different site
changes enzyme activity
active or inactive form
Cooperativity
one sibstrate bind helps others
increase activity
Feedback Inhibition
end product inhibits pathway
prevents overproduction
energy conservation
location
Helps bring order to metabolic pathways
Compartmentalization
enzymes in specific locations
increases efficiency
ex. mitochondria
Multienzyme Complex
enzymes grouped together
sequential reactions
faster processing
Thermodynamics laws
thermodynamics
study of energy transformations/ in a collection of matter
In sytems
System types
open sytem
exchanges energy/matter
ex. living organism
Isolated system
no exchange of energy/matter
ex. liquid in thermos
First law
Conservation of energy
energy cannot be created/destroted
only transformed
ex. food to heat to work
second law
increase entrophy in universe
entropy= chaos
heat released reduces usable enegy
universe becomes more disorded
Spontaneous process
no enegy
increase entropy
can be slow or fast
ex. diffusion
Nonspontaneous process
require energy input
Decrese entropy
must be with spontaneous
Cellular energy
ATP
Energy molecule
adenine/ribose/3 phosphates
ATP hydrolysis
ATP breakdown
ADP/ Pi
Release energy
Exergonic reaction
Phosphate bonds
High potential energy
Energy coupling
ATP provide enegy
Exergonic/endergonic reactions
Types of cellular work
Chemical work
Synthesis of molecules/endorgonic
Transport work
pumping across membrane/ against gradient
Mechanical. work
Movement/ muscle contratctions
Phosphorylation
transger of phsphate group
atp to another molecule
Receipt molecule
phosphorylated intermiedate
more reactive
Atp regeneration
ADP/PI to ADP
Need energy
ATPacyvle
Forms of energy
Energy
Capacity to do work
move objects perform work
Kinetic
Energy of motion
ex. water turning turbine
moving objects perform work
Heat
Kinetic energy of molecules
increase molecular movement
transfer of energy is called heat
Potential
Energy of position(location)
Chemical bonds store energy
ex. rock in a cliff
Chemical
Energy released in reactions
Potential enegy in molecules
Ex. glucose breakdown
metabolism
metabolic
stepwise chemical reactions
starting molecule to intermediate to product
each step catalyzed by enzy,e
specific enzyme for each reaction
anabolic
synthesis of molecules
simple to complex
need atp
endergonic process
Ex. protein synthesis
catabolic
breakdown of big molecules
complex to simple
release energy
exergonic process
ex. cellular respiration
total chemical reactions
emergent property of life
interactions of molecules