Life systems and their activity require energy and facilitate the flow of energy
Life needs to be ordered and structured due to to their ability to replicate, this requires energy, which means organisms release heat into the environment
Over 160 years ago, a term called energy was discovered, and it was surmised to be conserved
E is total internal energy
THERMODYNAMICS
Study of macroscopic states near equilibrium
Relaxation lifetimes
Time it takes for a system with various entities, interactions, and a number of energy states to reach thermal equilibrium
Every system differs
Long as most are composed of short metabolicprocesses and structures with long decay time
Living systems cannot have thermal equilibrium, there are processes that help us avoid reaching this
In physics, 2 bodies in thermal contact that do not exhibit macroscopic transfer of energy have the same temperature
Changes in temperature can cause change in volumes of certain materials (e.g. mercury thermometer)
Gases can also be used in measuring temperature, as changes in the temperature can cause changes in pressure, which can be monitored
Temperature is not equivalent to average kinetic energy, this only applies to systems which have no intermolecular interaction such as ideal gases
Temperature measures energies from both kinetic and potential energy
In temperature, the rate at which internal energy changes per unit change in the disorder of the system, while the volume and particle size of the unit are fixed
HEAT
Energy transferred between two bodies due to a difference in temperature
Energy transfer can lead to volume changes within systems
Heat Transfer
Causes a redistribution of the occupation numbers of the possible energy levels in the system without changing the energy levels in the microstates
Associated with change in disorder
Heat goes into a system (+)
When heat is absorbed by a system from its surroundings
E.g. When you place a pot of water on a stove, heat from the stove is transferred into the water, causing its temperature to rise
Heat goes out of a system (-)
When a system releases heat energy to its surroundings
E.g. When you turn off the stove and allow the pot of water to cool, heat is transferred from the water to the cooler surroundings
Adiabatic process - a change of a system involving no transfer of heat
Conduction
By means of molecular agitation within a material without any motion of the material as a whole
Convection
By mass motion of a fluid such as air or water when the heated fluid is caused to move away from the source of heat, carrying energy with it
Radiation
By EM waves such as visible light, UV and infrared radiation
HOMEOSTASIS
We maintain a temperature of 37°C through various means
Regulation of blood flow
Perspiration
Coverings
Hair erection
Shivering
Cell mitochondrial thermogenic control
Folding to reduce temperature
Exhalation
Our brain consumes 25 % of the energy present in blood, by product is heat
Zeroth Law of Thermodynamics
If two thermodynamic systems are in equilibrium with a third, then the two are in equilibrium with each other
First Law of Thermodynamics
The change in internal energy of a system equals to the heat added to the system minus the work done
Second Law of Thermodynamics
The entropy of any natural and spontaneous process either increases or remains constant
Third Law of Thermodynamics
Entropy of a pure crystal is zero as the temperature approaches absolute zero
ENTROPY
A measure of disorder in a system, defined by the second law of thermodynamics
The entropy change of a system from state A to state B will never be LESS than the change of entropy of a thermodynamic process that carries it from A to B
GIBBS FREE ENERGY
A value for isothermal and isobaric processes denoting the spontaneity of a system or an event
Minimized by systems at equilibrium
Applicable for most chemical and biological events
T or F. Living systems must have thermal equilibrium.