Equilibria - Copy - Copy - Copy

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  Equilibria Introduction Many reactions do not go to complete because the reaction is reversible. As the reaction is dependent on the concentration of the reactants, the reaction will proceed up to the point at which the rate of the forward reaction equals the rate of the reverse reaction.    Equilibria Things to learn ã  At equilibrium, the rate of forward reaction equals the rate of the reverse reaction. ã Both products and reactants are constantly being made and used up, but their concentrations do not change. ã In a static equilibrium all the processes which might disturb the equilibrium have stopped.   Equilibria ã Static equilibrium can be demonstrated by two children on a see-saw. They are balancing each other so no movement of the see-saw takes place. ã Dynamic equilibrium can be demonstrated by using isotopes. For example: CH 3 COOH(l) + C 2 H 5 OH(l) CH 3 COOC 2 H 5 (l) + H 2 O(l)   ã Mix the four substances in their equilibrium concentrations, but have the water made from the isotopes 18 O. After some time the 18 O isotope will be found (by means of a  Equilibria mass spectrometer) in both the ethanoic acid and the water, but the concentrations of the four substances will not have changed.
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