finals review Flashcards
(349 cards)
energy
capacity to cause change, especially to do work (move matter against an opposing force)
kinetic energy
energy associated witht eh relative motion of objects
thermal energy
kinetic energy due to the random motion of atoms and molecules (heat)
chemical energy
energy available in molecules for release in a chemical reaction
potential energy
energy that matter possesses as a result of its location or spatial arrangement
first law of thermodynamics
the total amount of energy in the universe must always be the same
what is the ultimate source of energy
the sun
what is photosynthesis
converts electromagnetic energy in sunlight to chemical-bond energy in organic molecules
ANABOLIC
what is cellular respiration
extracts energy from organic molecules (food) by gradual oxidation
CATABOLIC
second law of thermodynamics
the degree of entropy (disorder) in the universe can only increase
how do cells not defy the second law of thermodynamics
increased order inside cell = increased disorder in cell’s surroundings
free energy (energy that could do work) is dissipated as heat
what is free energy (G)
amt of energy available in a molecule to do work in a system when the temp and pressure are uniform
units: joules or kcal/mole
where is free energy stored
in the bonds between individual atoms of a molecule
what does free energy cause
vibration, rotation and movement of the molecule through space
how can chemical reactions produce disorder
- reactions can decrease order in the cell (ex. preventing an interaction that prevents bond rotations)
- changes of bond energy of reacting molecules can cause heat to be released –> disorders environment
equation for free energy
A + B –> C + D
(delta)G = free energy (C + D) - free energy (A + B)
when is G negative
if the disorder of the universe increases
a chemical reaction that occurs spontaneously
when is deltaG 0
at chemical equilibrium
standard free energy skin
gain or loss of free energy as one mole of reactant is converted to one mole of product under “standard conditions”
used to predict the outcome of a reaction
coupled reactions
coupling energetically unfavourable reactions with energetically favourable ones makes life possible
exergonic vs. endergonic reactions
exergonic: reaction with negative change in free energy
endergonic: reaction with positive change in free energy
exergonic reactions
releases energy into its surroundings, SPONTANEOUS
energetically favourable
lower free energy level (more stable)
release free energy in bonds
endergonic reactions
require energy, NON-SPONTANEOUS
energetically unfavourable reactions
higher free energy level than substrate
can store energy in molecules
activated carriers
store energy as a readily TRANSFERABLE CHEMICAL GROUP or as READILY TRANSFERABLE ELECTRONS