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### 27 Cards in this Set

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 1st law of Thermodynamics Energy of the universe is constant; Energy can never be created or destroyed 2nd law of Thermodynamics System spontaneously move toward disorder(high entropy) ΔE:? ΔE= q + E w= -pΔV +w = V is - -w = V is + Locked piston ΔE = q Unlocked piston: When heat piston Volume increases Work is - PE increases so ΔE decreases " Expanding gases cool" Unlocked piston: Put weight on piston Work is + Temp increases "compressed gases warm" Isobaric Pressure constant area= work done by gas Isochoric Volume constant Area= 0 so work= 0 Isothermal Temp constant ΔE=0 so q=-w Adiabatic no heat transfer q=0 ΔE=w "perfectly insulated system" Entropy Amount of disorder Increasing entropy means: 1) Phase change 2) Increasing # of moles of gas dissolved; the side with the more mol of gas has more entropy Enthalpy amount of heat gained or lost when bonds are formed or broken Bond breaking requires energy Bond forming releases energy (-)ΔH exothermic heat is product product have stronger bond that the reactant (+)ΔH endothermic heat is reactant reactant have stronger bonds Hf=0 when? when elements are in their natural state ΔG Gibbs free energy Energy evolved or absorbed as the rxn goes from rxn to product (-)ΔG product have less energy more stable spontaneous exergonic(energy is given off) (+)ΔG Product have more energy less stable nonspontaneous endergonic ΔG=0 prod and reac have same energy rxn is @ equilibrium Low temperature ΔH dominated if ΔH and ΔS are both (-):spon High temperature ΔS dominates Kinetics rates, activation Energy, catalyst, temp Thermodynamics ΔG, H, S, Equilibrium, Temperature