H_2(g) + Cl_2(g) → 2HCl_(g) ...... rate = r₁
D_2(g) + Cl_2(g) → 2DCl_(g) ..... rate = r₂.
The value of r₁ > r₂. Then the correct statement among the following is

detailed solution

Correct option is C

The order of bond dissociation energy (BDE): The order of bond lengths (B.L):  → The bond dissociation energy of heavier isotopes is greater than that of lighter isotopes.→ As the bond dissociation energy increases the time required to break the bond in the reaction increases, therefore rate of reaction (r) decreases. i.e,. The reaction which involes heavier isotopes proceeds with slower rate (r1) than the reaction which involes lighter isotopes(r1)  (1) B.L  : H-H ≈ D-D→  Correct but it is not correct explaination for the rates of above reaction(2) B.L (or) B.D.E: D-D > H-H(3)                ⇒ [Ea]2 > [Ea]1 and    Activation Energy:(Ea)The energy difference between the Activated complex and reactants is called Activation  energy.The reaction with high activation  energy proceeds with slow rate