Chemistry - Chemical Kinetics Question with Solution | TestHub

For the reaction $4A+B\to 2C+2D$, the rate of reaction is given by:

$\text{Rate}=-\frac{1}{4}\frac{d[A]}{dt}=-\frac{d[B]}{dt}=\frac{1}{2}\frac{d[C]}{dt}=\frac{1}{2}\frac{d[D]}{dt}$

From this relation, we can analyze the given options:

$-\frac{d[B]}{dt}=\frac{1}{4}\left(-\frac{d[A]}{dt}\right)$, so the rate of consumption of B is one-fourth the rate of consumption of A.

$\frac{d[D]}{dt}=\frac{2}{4}\left(-\frac{d[A]}{dt}\right)=\frac{1}{2}\left(-\frac{d[A]}{dt}\right)$, so the rate of formation of D is half the rate of consumption of A.

$\frac{d[C]}{dt}=2\left(-\frac{d[B]}{dt}\right)$, so the rate of formation of C is twice the rate of consumption of B. The statement says it is half, which is incorrect.

$\frac{d[C]}{dt}=\frac{d[D]}{dt}$, so the rates of formation of C and D are equal.

Thus, the incorrect statement is that the rate of formation of C is half the rate of consumption of B.

Answer: The rate of formation of C is half the rate of consumption of B.