Question

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

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

Answer 1

Answer: (A)

$2A+B \rightarrow C$
Rate = k[A][B]
It represents second-order reaction. So B, C and D options are incorrect.
As value of k is independent of the initial concentrations of A and B so option A is correct.