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Expression for equilibrium constant, (K_c = {left [ C right ]^r left [ D right ]^s over {left [ A right ]^m left [ B right ]^n} }) is applicable only when the reaction has achieved equilibrium i.e. concentrations of reactants and products have attained constant values.- The value of equilibrium constant (K_c) does not depend on initial concentrations of reactants and products.
- Equilibrium constant (K_c) depends on temperature. Its value is unique for a particular reaction and at a given temperature.
- Equilibrium constant (K_c(r))for reverse reaction is inverse of equilibrium constant (K_c (f))for forward reaction i.e. (K_c(r)) = (1 over {K_c (f)})
- Equilibrium constant (K_c) depends on stoichiometric coefficients of a balanced chemical equation.
- For a reaction that happens in steps,[ (ce{A + B<=>C + D, $K_c = K_1$}) ] and [ (ce{C + E<=>F + G, $K_c = K_2$}) ];
net reaction being $$ce{A + B +E <=> D + F + G }$$, then equilibrium constant for the reaction (K_c = K_1 times K_2 )
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