Enthalpy - energy, standard enthalpy of formation - when one mole of a substance is prepared from elements in their standard states, Entropy - disorder in the system, second law of thermodynamics - total entropy of a system and its surroundings is always increasing, third law of thermodynamics - entropy of a perfect crystal at 0K is zero, Gibbs free energy - effect on the system - brings together enthalpy and entropy, feasible - if the change in free energy is negative, enthalpy of formation - energy to make a compound from elements in their natural state, order - can only be determined by experiment and is how many moles in the RDS, first order - as concentration doubles, rate doubles, second order - as concentration doubles, rate quadruples, rate constant - proportional factor for each set of conditions, rate determining step - slowest step in the reaction, will match the rate equation, equilibrium - rate of the forward and reverse reactions are equal, equilibrium constant - characterises the equilibrium composition (large K = more products), effect of temperature - only thing to change K, hydronium ions - H3O+ , ionic product - Kw = [H3O+][OH-] = 1x10-14 at stp, bronsted lowry acid - donates protons H+, bronsted lowry base - accepts protons H+, conjugate base - formed form loss of proton (from an acid), strong acid - fully dissociates (HCl, HNO3, H2SO4), weak acid - partially dissocaites (-oic acids, sulfurous), strong alkali - metal hydroxides (e.g. NaOH), buffer solution - pH remains approximately constant, weak acid and its salt, acidic salt - strong acid + weak base, basic salt - strong alkali + weak acid, acid buffer - weak acid supplies H+ when these are removed by base, conjugate reacts with any added acid, indicator - weak acid dissociation where two distinct colours of acid and the conjugate, indicator colur change - [H3O+] = Kin,

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