The rate law for the reaction $2 \mathrm{X}+\mathrm{Y} ightarrow \mathrm{Z}$ is Rate…

The rate law for the reaction $2 \mathrm{X}+\mathrm{Y} ightarrow \mathrm{Z}$ is Rate $=k[\mathrm{X}][\mathrm{Y}] .$ The correct statement with regard to this relation is
  1. the unit of $k$ is $\mathrm{s}^{-1}$
  2. the rate of the reaction is independent of $[\mathrm{X}]$ and $[\mathrm{Y}]$
  3. for this reaction $t_{1 / 2}$ is independent of initial concentrations of reactant
  4. the rate of formation of $Z$ is half of the rate of disappearance of $X$

Solution

The given reaction is $: 2 \mathrm{X}+\mathrm{Y} \longrightarrow \mathrm{Z}$
$-\frac{\mathrm{d}[\mathrm{X}]}{2 \mathrm{dt}}=\frac{\mathrm{d}[\mathrm{Z}]}{\mathrm{dt}}$
$\therefore$ Rate of formation of $Z$ is half of the rate of disappearance of $X$.

Asked in: JEE-TOPICTESTS-CHEMISTRY

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