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Equilibrium/rxn rate

collision theory atoms, ions, and molecules can react to form products when they have collided, provided that the particles have enough KE
reaction properties particles collide enough KE right orientation
activation energy minimum amount of energy particles must have to react
activated complex/transition state arrangement of atoms at peak of activation energy
rate measures the speed of any change that occurs within an interval of time
rate equation x y Rate=[reactant] [reactant]
factors affecting reaction rates temperature: higher temps = faster rates concentration: higher concentration = faster rates
catalysts substance that increases rate of reaction without being used up by allowing the reaction to occur at lower temps
inhibitor substance that interferes with the actions of the catalyst; slows reaction
reversible reaction reaction occur simultaneously in both directions
equilibrium forward and reverse reaction occurs at the same rate and the same time
le chateliers principle is stress is applied to a system in equilibrium, the system changes to relieve that stress
equilibrium constant(Keq) ratio of product concentrations to reactant concentrations at equilibrium with each concentration raised to the power equal to their coefficients
Keq > 1 product favored
Keq < 1 reactant favored
Keq used for any reactions
Ka used for acids
Kb used for bases
Ksp solubility product(for things that are dissolving in solutions)
Kp used when pressure is used instead of concentration
Kc used when concentration in used
rate laws expressions relating rate of reaction to concentration of reactants
K specific rate constant
[] molar concentration
P and Q determined experimentally (usually 0, 1, 2)
free energy energy available to do work
spontaneous reaction reaction that occurs naturally and favors formation of products at specific conditions
non-spontaneous reaction reaction that doesn't favor the formation of products at specified conditions
entropy measure of disorder of a system; influences spontaneity of reaction
particle size smaller particles = more surface area = faster rates
reactant form products forward reaction
products form reactant reverse reaction
Created by: neisha0501