7. Equilibria Flashcards
(13 cards)
reversible reaction
dynamic equilibrium and closed system
why closed system
rate of forward and reverse
reactions being equal and the concentration of reactants and products remaining constant
Le Chatelier’s principle
if a change is made to a system at dynamic equilibrium, the position of
equilibrium moves to minimise this change
effects of changes in temperature, concentration, pressure or presence of a catalyst on a system at equilibrium
temperature-
concentration-
pressure-
equilibrium constants in terms of concentrations, Kc.
mole fraction and partial pressure
equilibrium constants in terms of partial pressures, Kp
changes in temperature, concentration or pressure or the presence of a catalyst affect the
value of the equilibrium constant for a reaction
ONLY temperature affects K.
conditions used in the Haber process and the Contact process
common acids and alkalis
hydrochloric acid, HCl, sulfuric acid, H2SO4, nitric acid, HNO3, ethanoic acid, CH3COOH
sodium hydroxide, NaOH, potassium hydroxide, KOH, ammonia, NH3
Brønsted–Lowry theory of acids and bases
strong and weak acids and bases
fully/partially dissociated in aqueous solution
differences in behaviour between strong and weak acids
reaction with a reactive metal and difference in pH values by use of a pH meter, universal indicator or conductivity
neutralisation
H+(aq) and OH–(aq) form H2O(l)
salt always forms
pH titration curves using combination of strong and weak acids and bases and suitable indicators
