Question

The rate of reaction for the reaction $2A+B\to C$ is $k\left[A\right]\left[B\right]$. The correct statement in relation to this reaction is :

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

Answer 1

The correct option is B the value of $k$ is independent of the initial concentration of A and B

For a second order reaction, the unit of k is $M^{-1}{s}^{-1}.$
The value of k is constant at a given temperature and is independent of the initial concentration of A and B.
The rate of formation of C is the half of the rate of disappearance of A.
For a second order reaction, the half-life period is inversely proportional to concentration. Hence, half-life period is not constant.