Reactant A converts to product D through the given mechanism (with the net evolution of heat):

$A \to B (slow); Δ H = + ve$

$B \to C (fast); Δ H = - ve$

$C \to D (fast); Δ H = - ve$

Which of the following represents the above reaction mechanism [2025]

Question

Reactant A converts to product D through the given mechanism (with the net evolution of heat):

$A \to B (slow); Δ H = + ve$

$B \to C (fast); Δ H = - ve$

$C \to D (fast); Δ H = - ve$

Which of the following represents the above reaction mechanism? [2025]

Smart Achievers · Accepted Answer

(1)

$As A \to B is an endothermic reaction, E_{B} > E_{A}$

$As B \to C is an exothermic reaction, E_{C} < E_{B}$

$As C \to D is an exothermic reaction, E_{D} < E_{C}$

$As net reaction is exothermic, E_{D} < E_{A}$

$Only option (1) satisfies these conditions.$

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