For the hypothetical reaction $2X + G \to Q + 2M$ , the rate expression is $\frac{{d\left[ Q \right]}}{{dt}} = k{\left[ X \right]^2}$ . Which of the following is the most likely mechanism ?
For the hypothetical reaction $2X + G \to Q + 2M$ , the rate expression is $\frac{{d\left[ Q \right]}}{{dt}} = k{\left[ X \right]^2}$ . Which of the following is the most likely mechanism ?
- A
$2X + G \rightleftharpoons 2Q + R$ (fast)
$Q + R + G \to 2M$ (slow)
- B
$X + G \rightleftharpoons Q + R$ (fast)
$R + X \to 2M$ (slow)
- C
$X + X \rightleftharpoons {X_2}$ (fast)
${X_2} \to Q + T$ (slow)
$T + G \to 2M$ (fast)
- D
$G + G \rightleftharpoons {G_2}$ (fast)
${G_2} + X \to Q + T$ (slow)
$T + X \to 2M$ (fast)
Similar Questions
For a reaction $X + Y \to Z$, rate $ \propto \, [X]$. What is $(i)$ molecularity and $(ii)$ order of reaction ?
For a reaction $X + Y \to Z$, rate $ \propto \, [X]$. What is $(i)$ molecularity and $(ii)$ order of reaction ?
The rate of disappearance of $S{O_2}$ in the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ is $1.28 \times {10^{ - 3}}g/sec$ then the rate of formation of $S{O_3}$ is
The rate of disappearance of $S{O_2}$ in the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ is $1.28 \times {10^{ - 3}}g/sec$ then the rate of formation of $S{O_3}$ is
For the reaction
$2 \mathrm{H}_{2}(\mathrm{g})+2 \mathrm{NO}(\mathrm{g}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$
the observed rate expression is, rate $=\mathrm{k}_{\mathrm{f}}[\mathrm{NO}]^{2}\left[\mathrm{H}_{2}\right] .$ The rate expression of the reverse reaction is
For the reaction
$2 \mathrm{H}_{2}(\mathrm{g})+2 \mathrm{NO}(\mathrm{g}) \rightarrow \mathrm{N}_{2}(\mathrm{g})+2 \mathrm{H}_{2} \mathrm{O}(\mathrm{g})$
the observed rate expression is, rate $=\mathrm{k}_{\mathrm{f}}[\mathrm{NO}]^{2}\left[\mathrm{H}_{2}\right] .$ The rate expression of the reverse reaction is
- [JEE MAIN 2020]
For a certain reaction : $(A)(g) \to B(g)$ Half life for different initial pressures of $A$ is given below
$\begin{array}{|l|l|l|} \hline {P_{{A_0}}}(atm) & 0.1 & 0.025 \\ \hline {t_{1/2}}(\sec\,\,) & 100 & 50 \\ \hline \end{array}$
The correct statement about order of reaction is
For a certain reaction : $(A)(g) \to B(g)$ Half life for different initial pressures of $A$ is given below
$\begin{array}{|l|l|l|} \hline {P_{{A_0}}}(atm) & 0.1 & 0.025 \\ \hline {t_{1/2}}(\sec\,\,) & 100 & 50 \\ \hline \end{array}$
The correct statement about order of reaction is
Write about elementary and complex reactions.
Write about elementary and complex reactions.