Chapter 11: Thermodynamics
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Last updated 7:40 PM on 4/3/23
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22 Terms
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System
part of universe what you are studying
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surroundings
anything and everything not under study
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open system
transfer energy and matter to surroundings
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closed system
transfer only energy to surroundings
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isolated system
transfers nothing to surroundings
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state functions
describes an aspect of a chemical system (such as pressure, volume)
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extensive properties
the matter changes as the initial sample change
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standard state
1 atm, 25 celsius, 1 mol of compound present
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exothermic
energy lost to surroundings
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ΔH sign for exothermic
negative
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endothermic
energy gained from surroundings
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ΔH symbol for endothermic
positive
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law of conservation of energy
energy cannot be created or destroyed
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kinetic energy
energy in motion
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potential energy
stored and released under certain conditions
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specific heat
amount of energy needed to cause 1 g of substance to increase in 1 degree celsius (or kelvin)
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first law of thermodynamics
energy is always conserved
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work
force applied to an object as it moved a certain distance
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enthalpy
H
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formation reactions
only one mole of products and reactants in standard states
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entropy
S
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Gibbs Free Energy
G
