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APC: Equilibrium
Term | Definition |
---|---|
chemical equilibrium | state where the forward reaction rate is equal to the reverse reaction rate |
Why is it dynamic | each species is actively consumed and produced |
Criteria for an equilibrium system | 1. constant macroscopic properties(concentrations, pH, color, temperature) 2. closed system 3. shift in response to changes |
macroscopic property | property observed with the naked eye |
closed system | system where chemicals do not enter or leave |
steady state | system that appears to be at equilibrium but chemicals are entering and leaving the system at the same time |
Stage 1 | reactant concentrations are high, rf is at the highest A+B-> |
Stage 2 | concentrations of A, B, and rf decrease concentrations of C,D, and rr increase A+B<-C+D |
Stage 3 | concentrations of A,B,C,D are constant rf, rr are equal |
Le Chatelier's Principle | an equilibrium system will shift when subjected to stress will shift to alleviate the stress |
stress | any change that favors rf or rr |
if the concentration of a chemical species increases... | then the system will shift to consume that species |
if the concentration of a chemical species decreases... | the system will shift to produce that species |
when a system shifts to favor the products it... | shifts right |
when a system shifts to favor the reactants it... | shifts left |
adding a catalyst... | does not affect equilibrium, but the systems will alleviate the stresses applied faster |
equilibrium position | relative concentrations of chemical species in equilibrium expressed in percent yield |
percent yield | actual/theoretical x 100 |
if the percent yield is above 50%... | the products are favored |
if the percent yield is less than 50%... | the reactants are favored |
partial pressure | pressure exerted by an individual gas in a mixture |
partial pressure is to gaseous equilibria as... | osmotic pressure is to solution concentration |
gas pressure is directly proportional to... | gas concentration |
osmotic pressure is directly proportional to... | solution concentration |
the side of equilibrium with the greater sum of coefficients... | will be more sensitive to volume change |
if temperature is increased in a rigid container... | pressure increases, but will not affect equilibrium |
as temperature changes are gradual, a system in equilibrium will... | shift before the stress is fully applied |
when heat is added the | endothermic direction is favored due to activation energy requirements |
Haber Bosch Reaction | N2 + 3H2 = 2NH3 + 92.4 kJ |
Haber Reactor | -decrease temperature -catalyst is added -pressure increased to 3.5x10^4 kPa |
equilibrium expression | formula for finding the equilibrium constant in terms of concentrations of products and reactants |
equilibrium constant(keq) | numerical value that relates the concentrations of products to the concentration of reactants in equilibria -units vary and not expressed -temperature dependent |
keq>1 | products are favored |
keq<1 | reactants are favored |
equilibrium law | the expression of a balanced chemical equation and an equilibrium expression together |
reaction quotient(or trial keq) | numerical value calculated from taking any set of concentrations and plugging them in to an equilibrium expression |
if q>keq | proceed left |
if q<keq | proceed right |
if only one chemical species is present in an equilibrium expression... | the system will shift to completely alleviate the stress that affects its concentration |
ICE Box | table that is used to solve calculations in systems of equilibria |
mass action expression | equilibrium expressions in terms of concentration or partial pressure |
how many psi in 1 atm | 14.7psi |
how many mmHg in 1 atm | 760mmHg(torr) |
how many kPa in 1 atm | 101.3 kPa |
how many bar in 1 atm | 1.01 bar |
ideal gas constant | 0.08206 L x atm/(mol x K) |
Kp= | Kc(RT)^delta n |