Studied by 12 peopleSystem
part of universe what you are studying
surroundings
anything and everything not under study
open system
transfer energy and matter to surroundings
closed system
transfer only energy to surroundings
isolated system
transfers nothing to surroundings
state functions
describes an aspect of a chemical system (such as pressure, volume)
extensive properties
the matter changes as the initial sample change
standard state
1 atm, 25 celsius, 1 mol of compound present
exothermic
energy lost to surroundings
ΔH sign for exothermic
negative
endothermic
energy gained from surroundings
ΔH symbol for endothermic
positive
law of conservation of energy
energy cannot be created or destroyed
kinetic energy
energy in motion
potential energy
stored and released under certain conditions
specific heat
amount of energy needed to cause 1 g of substance to increase in 1 degree celsius (or kelvin)
first law of thermodynamics
energy is always conserved
work
force applied to an object as it moved a certain distance
enthalpy
H
formation reactions
only one mole of products and reactants in standard states
entropy
S
Gibbs Free Energy
G
Note
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