Chapter 6 - Equilibria
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what is a reversible reaction and how it is represented
a reaction in which the products are turned into the reactants and the reactants can be turned back into the products a double arrow is used to represent one
state the conditions of a reaction in dynamic equilibrium
the rates of the forward and backward reactions are the same the concentration of the reactants and the products stays constant the reaction occurs in a closed system
state Le Chatelier’s principle
If a system at equilibrium is subjected to a change, the position of equilibrium will shift to counteract said change
what changes will affect the position of equilibrium
temperature pressure concentration
state the effect on the yield of the products of increasing the temperature of a reaction in equilibrium (endo and exo)
endo: temp up, yield up exo: temp up, yield down
state the effect on the yield of the products of increasing the pressure of a reaction in equilibrium
if more moles on products side, yield decreases if more moles on reactants side, yield increases
how does using a catalyst affect the position of eqilibrium
it doesnt, only changes the rates of reaction
how to calculate Kc for aA + bB —-> cC + dD
[C]^c + [D]^d / [A]^a + [B]^b conc of products / conc of reactants
how will changing temp, press, or conc affect Kc
only temp will affect Kc in an endo reaction, change and Kc directly proportional in an exo reaction, change and Kc inversely proportional
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