Consider the following statements related to temperature dependence of rate constants. Identify the correct statements, A. The Arrhenius equation holds true only for an elementary homogenous reaction. B. The unit of A is same as that of k in Arrhenius equation. C. At a given temperature, a low activation energy means a fast reaction. D. A and Ea as used in Arrhenius equation depend on temperature. E. When Ea >> RT, A and Ea become interdependent. Choose the correct answer from the options given below:

### Related Formula Arrhenius equation is given by: k = A e^-fracE_aR T$$k = A e^{-\frac{E_a}{R T}}$$ where: - k$k$ is the rate constant - A$A$ is the pre-exponential factor (frequency factor) - E_a$E_a$ is the activation energy ### Core Logic Evaluate each statement: - **A**: Arrhenius equation is an empirical relation that works well for both elementary and complex homogeneous reactions rightarrow$\rightarrow$ *Incorrect*. - **B**: Since the exponential term e^-E_a/RT$e^{-E_a/RT}$ is dimensionless, the pre-exponential factor A$A$ has the exact same unit as the rate constant k$k$ rightarrow$\rightarrow$ *Correct*. - **C**: For low E_a$E_a$, the term e^-E_a/RT$e^{-E_a/RT}$ is large, giving a high rate constant k$k$ and a fast reaction rightarrow$\rightarrow$ *Correct*. - **D**: A$A$ and E_a$E_a$ are assumed to be independent of temperature over a narrow range rightarrow$\rightarrow$ *Incorrect*. - **E**: A$A$ and E_a$E_a$ remain independent parameters of the system, not interdependent rightarrow$\rightarrow$ *Incorrect*. ### Step 1: Select correct statements Statements B and C are correct, matching Option (3). ### Pattern Recognition The exponential factor e^-E_a/RT$e^{-E_a/RT}$ represents the fraction of collisions with energy greater than the activation barrier. As E_a$E_a$ decreases, this fraction grows exponentially, explaining why low-activation pathways (like catalyzed reactions) run much faster. ### Evaluation Rubric / Model Answer null ### Chapter Mix Class 12 Chemistry: Chemical Kinetics