spontaneous reaction
A process that occurs naturally without external energy. Often exothermic with increasing entropy.
non-spontaneous reaction
A process that requires continuous external energy to proceed.
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spontaneous reaction
A process that occurs naturally without external energy. Often exothermic with increasing entropy.
non-spontaneous reaction
A process that requires continuous external energy to proceed.
Gibbs Free Energy (DeltaG)
DeltaG = DeltaH - TDeltaS. Determines if a process is spontaneous. If DeltaG < 0, the process is spontaneous.
negative DeltaG
The process is spontaneous.
positive DeltaG
The process is non-spontaneous.
endothermic reaction
Absorbs heat (DeltaH > 0).
exothermic reaction
Releases heat (DeltaH < 0).
entropy (DeltaS)
A measure of disorder. Higher entropy means more disorder.
factors increasing entropy
Phase changes to gas, more product particles than reactants, mixing substances.
enthalpy (DeltaH)
The total heat content of a system. Determines heat flow during reactions.
rate of a chemical reaction
Affected by concentration, temperature, surface area, catalysts, and nature of reactants.
activation energy
The minimum energy needed for a reaction to occur.
catalysts
They lower activation energy and speed up the reaction without being used up.
rate law
An expression that relates reaction rate to the concentration of reactants.
general form of a rate law
Rate = k[A]^m[B]^n, where m and n are reaction orders.
determining rate law experimentally
By measuring how rate changes with varying reactant concentrations.
equilibrium constant (K)
K = [products]^coeff / [reactants]^coeff at equilibrium.
K > 1
Products are favored at equilibrium.
K < 1
Reactants are favored at equilibrium.
Le Châtelier's Principle
If a system at equilibrium is disturbed, it will shift to counteract the disturbance.
temperature effect on equilibrium
Endothermic: heat is a reactant; Exothermic: heat is a product. Raising temp shifts equilibrium away from heat.