Question

The rate equation for the reaction $2A+B\to C$ is found to be rate $=k[A][B]$ The correct statement in relation to this reaction is that the

• A. unit of k must be $s^{-1}$
• B. $t_{1/2}$ is a constant
• C. rate of formation of C is twice the rate of, disappearance of A
• D. value of k is independent of the initial concentrations of A and B

Answer 1

Answer: (C)

$2A+B\to C$ Rate $=k[A][B]$ It represents second-order reaction. Thus unit of k is $M^{-1}{s}^{-1}$ $\therefore$ is false $T_{50}$ is dependent of concentration but not constant $\therefore$ (a) is false $-\frac{1}{2}\frac{d[A]}{dt}=\frac{d[C]}{dt},$ thus (c) is correct