Consider the complex generic reaction mechanism taking place in two explicit sequential steps: Step — Chemical Kinetics Chemistry Question

💡 Solution & Explanation

Statement A is true as the slow step dictates the rate. Statement B represents standard kinetics protocol where unmeasurable intermediates in rate laws are substituted via preceding fast equilibria. Applying this, $K_c = \frac{[I]}{[A][B]} \Rightarrow [I] = K_c[A][B]$. Substituting $I$ into the slow step rate law yields $\text{Rate} = k_2 K_c [A][B][C]$, proving C is correct and the effective constant $k_{eff} = k_2 K_c$, validating D.