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Cards for exam 3

First Law of Thermodynamics Energy is conserved
Second law of Thermodynamics Any system NOT at equilibrium has an inherent direction in which it will move in order to reach equilibrium *This is called a spontaneous reaction
Third law of Thermodynamics The Entropy of a pure crystalline solid is equal to zero at absolute zero (i.e. there is no disorder)
Factors determining Spontaneity 1) Exothermic reactions have a strong tendency to be spontaneous 2) The greater disorder of the system, the greater system entropy, therefore high spontaneity
Gibbs free energy change(equation) delta_g=delta_h-[(t(kelvin))(delta_s)] delta_g(rxn)=delta_g(prod)-delta_g(react) *State function
Gibbs free energy change and reaction spontaneity delta_g,negative= Occurs in forward direction delta_g,positive= Occurs in reverse direction delta_g,0= Equilibrium
Standard Conditions solids exist as pure solids liquids exist as pure liquids gases exist at 1 atm pressure solutions have all solutes present at a concentration of 1 mol/l 25 degrees Celsius
Gibbs free energy change Measure of the maximum amount of usable work that can be done by the system on the surroundings by a spontaneous process at constant pressure * Tells us nothing about the speed of the reaction
Gibbs free energy change under non-standard conditions delta_g=delta_g(std)-(R)(T)(ln(Q))
delta_g to K delta_g=-(R)(T)(ln(K))
Created by: Whatx



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