1. Chapter 8: Metabolism

2. Metabolism Metabolism: The totality of an organisms chemical reactions
Manages the material and energy resources of the cell
Begin with molecule and end with product
Catabolic pathway:
Release of energy by breakdown of complex molecules to simpler compounds
When digestive enzymes break down food
Anabolic pathway:
Consume energy to build complex molecules from simpler ones
Building muscle fibers from amino acids in response to exorcise

3. Complexity of Metabolic Pathways

4. Anabolic vs Catabolic

5. Energy Energy is the capacity to do work
Objects in motion possess kinetic energy
Objects at rest possess potential energy
Chemical energy: potential energy stored in the form of chemical bonds

6. Energy Kinetic energy is energy associated with motion
Heat (thermal energy) is kinetic energy associated with random movement of atoms or molecules
Potential energy is energy that matter possesses because of its location or structure
Chemical energy is potential energy available for release in a chemical reaction

7. Energy

8. Thermo Dynamics
The study of energy transformations that occur in matter
Closed systems verses open systems
Organisms are open systems
The two laws
NUMERO UNO: principal of conservation of energy
Energy can be transferred and transformed, but it cannot be created or destroyed
NUMERO DOS:
Every energy transformation or transfer increases the entropy (disorder) of the universe

9. Thermodynamics
During energy transfer energy is often lost in the form of heat, sound, friction, and so on.
Think of all the energy lost as a car accelerates

10. Free Energy
Free energy: the part of a systems energy that is able to perform work when the temperature of a system is uniform.
EXERgonic reaction: Energy is released
Energy is released
Occur spontaneously
Release free energy into the system
ENDERgonic reaction: Requires energy
Absorbs free energy from the system

11. The change in free energy (∆G) during a process is related to the change in enthalpy, or change in total energy (∆H), change in entropy (∆S), and temperature in Kelvin (T):
∆G = ∆H – T∆S
Only processes with a negative ∆G are spontaneous
Spontaneous processes can be harnessed to perform work
Can use the free energy equation to determine if a reaction will occur spontaneously or not
Very important when studying metabolism and trying to determine which reactions will happen spontaneously.

12. Free Energy Free energy
measure of a system’s instability, tendency to change to more stable state
During a spontaneous change, free energy decreases and stability of system increases
Equilibrium: state of max stability
A process is spontaneous and can perform work only when it is moving toward equilibrium

13. Free Energy Changes
Processes are spontaneous and can do work only when they are moving toward equilibrium