Question

Which of the following expressions is correct for the rate of
reaction given below?
5Br⁻ (aq) + BrO₃⁻ (aq) + 6H⁺ (aq) → 3Br₂ (aq) + 3H₂O(l)
(a) ∆[Br⁻]/∆t = 5 ∆[H⁺]/∆t
(b) ∆[Br⁻]/∆t = 6/5 ∆[H⁺]/∆t
(c) ∆[Br⁻]/∆t = 5/6 ∆[H⁺]/∆t
(d) ∆[Br⁻]/∆t = 6 ∆[H⁺]/∆t

Answer 1

answer : option (c) ∆[Br⁻]/∆t = 5/6 ∆[H⁺]/∆t

rate of appearance or disappearance = ± 1/stoichiometric coefficient × d[product or reactant]/dt

for instance, aA + bB ⇒cC + dD

-1/a d[A]/dt = -1/b d[B]/dt = +1/c d[C]/dt = +1/d d[D]/dt

now come to the question, reaction is ....

BrO₃⁻ (aq) +5Br⁻ (aq) + 6H⁺ (aq) → 3Br₂(l) +3H₂O(l)

⇒-d[BrO₃-]/dt = -1/5 d[Br-]/dt = -1/6 d[H⁺]/dt = +1/3 d[Br₂]/dt = +1/3 d[H₂O]/dt

⇒-1/5 d[Br-]/dt =-1/6 d[H⁺]/dt

⇒d[Br-]/dt = 5/6 d[H⁺]/dt

hence option (c) is correct choice.

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