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The rate equation for the reaction $2 \mathrm{~A}+\mathrm{B} \longrightarrow \mathrm{C}$ is found to be: rate $\mathrm{k}[\mathrm{A}][\mathrm{B}]$. The correct statement in relation to this reaction is that the

ChemistryChemical KineticsJEE MainJEE Main 2004

Options:

A
unit of $\mathrm{K}$ must $\mathrm{be} \mathrm{s}^{-1}$
B
values of $\mathrm{k}$ is independent of the initial concentration of $A$ and $B$
C
rate of formation of $C$ is twice the rate of disappearance of $A$
D
$t_{1 / 2}$ is a constant

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