Question

For a reaction 1/2 A → 2B, rate of disappearance of ‘A’ is
related to the rate of appearance of ‘B’ by the expression
(a) – d[A]/dt = 1/2 d[B]/dt
(b) – d[A]/dt = 1/4 d[B]/dt
(c) – d[A]/dt = d[B]/dt
(d) – d[A]/dt = 4 d[B]/dt

Answer 1

(d) – d[A]/dt = 4 d[B]/dt is the correct answer

Answer 2

answer : option (b) -d[A]/dt = 1/4 d[B]/dt

This question is based on kinetic equation of chemical reactions.

if a chemical reaction, aA + bB ⇒cC + dD is given then,

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

using this application here,

we get, -1/(1/2) d[A]/dt = 1/2 d[B]/dt

⇒-2 d[A]/dt = 1/2 d[B]/dt

⇒- d[A]/dt = 1/4 d[B]/dt

hence option (b) is correct choice.

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