kinetics and equilibrium Flashcards
what does kinetics study
the rates of chemical reactions
what must particles do to react
collide
effective reaction leads to a
reaction
ineffective reaction leads to
no reactions
what conditions must be met to have an effective collision
particles collide with enough energy and particles must have proper orientation
if particles must collide to react, then more collisions equal
faster reaction rate
increased temperature in a reaction causes
increased average kinetic energy = particles move faster
increased concentration in reactions mean
more molecules present in the same amount of space
increased pressure in reactions causes
gas molecules to become closer together
what 4 conditions lead to a fast reaction rate
increased temperature, increased concentration, increased surface area, increased pressure
when bonds are broken energy is
absorbed
when bonds are formed energy is
released
what do chemical bonds contain
potential chemical energy
what is heat of reaction formula
Hproducts - Hreactants
exothermic equals
release energy
endothermic equals
absorb energy
what does a catalyst do
speeds up the rate of reaction but doesn’t affect the number of collisions
a catalyst provides
alternate pathway for a reaction with a lower activation energy
enthalpy is
energy
entropy is
randomness or disorder
when does enotropy increase
when gas is formed and when molecules break apart
what do systems in nature favor
low enthalpy and high entropy
what is equilibrium
when the rate of the forward reaction equals the rate of the reverse reaction
what are the three types of equilibrium
phase, solutions, chemical
