Consider a hypothetical chemical reaction: A + B ⇌ C + D. The reaction is carried out in a closed container at a constant temperature. Initially, only reactants A and B are present. As the reaction progresses, the concentrations of A and B decrease, while the concentrations of C and D increase. In this system, the forward reaction rate is faster than the reverse reaction rate at the beginning. However, as the reaction proceeds, the reverse reaction rate gradually catches up and eventually becomes equal to the forward reaction rate. Explain the factors that contribute to this change in reaction rates and discuss how this phenomenon relates to the concept of chemical equilibrium

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