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\xrightarrow[{}]{{}}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