For the reaction A → B, the rate of reaction can be written as:
A$-d[A]/dt$ only
B$+d[B]/dt$ only
C$+d[A]/dt = -d[B]/dt$
D$-d[A]/dt = +d[B]/dt$
Answer & Solution
Correct answer: D. $-d[A]/dt = +d[B]/dt$
A is consumed → rate $= -d[A]/dt$ (negative because [A] decreases). B is formed → rate $= +d[B]/dt$. By stoichiometry (1:1), both are equal.
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