Question

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

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

Answer 1

The correct option is D value of k is independent of the initial concentrations of A and B

$k=\frac{v}{\left[A\right]\left[B\right]}⟶$$k$ depends on instantaneous concentration of $\left[A\right]$ and $\left[B\right]$ and not on initial $\left[A_o\right]$ and $\left[B_o\right]$