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equilibrium position
used to determine if a reaction has reached equilibrium
law of chemical equilibrium
states that every reaction proceeds to an equilibrium state with a specific Keq
reaction quotient
depends on the initial concentrations of the substances in a reaction
homogenous equilibria
equilibrium condition for reactions in which products and reactants are in the same state
law of mass action
expresses the relative concentration of reactants and products at equilibrium in terms of an equilibrium constant
heterogenous equilibria
equilibrium condition for a chemical reaction involving substances in more than one state
equilibrium constant
the ratio of product concentration to reactant concentration of equilibrium
Keq >>> 1
shifts towards products
Keq <<< 1
shifts towards reactants
Keq = 1
equilibrium
Q > Keq
shifts towards reactants
Q < Keq
shifts towards products
Q = Keq
equilibrium
le chatelier principle
factors affecting chemical equilibrium: changes in concentration, pressure, temperature
concentration: reactant is added
shifts towards products
concentration: reactant is removed
shifts towards reactants
concentration: product is added
shifts towards reactants
concentration: product is removed
shifts towards products
pressure: increase in pressure
shifts towards side with least number of moles of gas
pressure: decrease in pressure
shifts towards side with most number of moles of gas
temperature: endothermic, increase in temperature
shifts towards products
temperature: endothermic, decrease in temperature
shifts towards reactants
temperature: exothermic, increase in temperature
shifts towards reactants
temperature: exothermic, decrease in temperature
shifts towards products
ΔS+, ΔH-, ΔG-
spontaneous at all T
ΔS+, ΔH+, ΔG+/-
spontaneous at high T, at low T rxn will go in reverse
ΔS-, ΔH-, ΔG+/-
spontaneous at low T, at high T rxn will go in reverse
ΔS-, ΔH+, ΔG+
non-spontaneous at all T
enthalpy of formation (remember formula!)
energy change when one mol of a substance is formed from its elements at standard conditions; unit Kj/mol
entropy (remember formula!)
measurement of disorder, randomness; unit J/K*mol
gibbs free energy
the energy available to do work; energy stored in chemical bonds; temperature dependent
ΔG<0
forward reaction
ΔG>0
reverse reaction
ΔG=0
equilibrium
equilibrium temperature
set ΔG to 0
the equilibrium concentration of products is much greater than that of reactants
Keq is much greater than 1
the equilibrium concentration of products is much less than that of reactants
Keq is much less than 1
there is a considerable amount of both reactants and products at equilibrium
Keq is about equal to 1
Note
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