Answer:
(i) Large value of equilibrium constant \[(>{{10}^{3}})\] shows that forward reaction is favoured, i,e., concentration of products is much larger than that of the reactants at equilibrium.
(ii) Intermediate value of \[K\,({{10}^{-3}}\,\text{to}\,{{10}^{3}})\] shows that the concentration of the reactants and products are comparable.
(iii) Low value of \[K(<{{10}^{-3}})\] shows that backward reaction is favoured, i.e., concentration of reactants is much larger than that of the products.
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