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Explanation:
Dynamic equilibrium in chemical reactions refers to a state in which the forward and reverse reactions occur at the same rate, and the concentrations of reactants and products remain constant over time. It's important to note that dynamic equilibrium does not imply that the reactions have stopped; rather, the rates of the forward and reverse reactions are equal.
Consider the general chemical reaction:
[tex]\[ aA + bB \rightleftharpoons cC + dD \][/tex]
where \(a\), \(b\), \(c\), and \(d\) are coefficients representing the stoichiometry of the reaction. At dynamic equilibrium, the rate of the forward reaction (\(aA + bB \rightarrow cC + dD\)) is equal to the rate of the reverse reaction (\(cC + dD \rightarrow aA + bB\)).
An example is the Haber-Bosch process for ammonia synthesis:
[tex]\[ N_2(g) + 3H_2(g) \rightleftharpoons 2NH_3(g) \][/tex]
In this reaction, nitrogen (\(N_2\)) reacts with hydrogen (\(H_2\)) to form ammonia (\(2NH_3\)). At dynamic equilibrium, the rate of the forward reaction (formation of ammonia) is equal to the rate of the reverse reaction (decomposition of ammonia back into nitrogen and hydrogen).
The dynamic equilibrium in this process is crucial for industrial-scale ammonia production, ensuring a steady yield of ammonia without the continuous consumption of reactants or the overaccumulation of products.