Which of the following reaction will have fractional order for $A_2$ or $B_2$ ?
Which of the following reaction will have fractional order for $A_2$ or $B_2$ ?
- A
$A_2 \rightleftharpoons A + A$ (fast)
$A + B_2 \rightleftharpoons AB + B$ (slow)
$A + B \rightleftharpoons AB$ (fast)
- B
$A_2 \rightleftharpoons C$ (slow)
$C + B_2 \rightleftharpoons D $ (fast)
$D + A_2 \rightleftharpoons $ Products
- C
$B_2 \rightleftharpoons B + B$ (fast)
$A_2 + B \rightleftharpoons AB + A $ (slow)
$AB \to $ Products
- D
Both $(A)$ and $(C)$
Similar Questions
The half life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $'p_0'$ as follows :
$\begin{array}{|l|l|l|} \hline P_0\,\,(mmHg) & 250 & 300 \\ \hline t_{1/2}\,\,(minutes) & 135 & 112.5 \\ \hline \end{array}$
The order of reaction is -
The half life period of a gaseous reactant undergoing thermal decomposition was measured for various initial pressures $'p_0'$ as follows :
$\begin{array}{|l|l|l|} \hline P_0\,\,(mmHg) & 250 & 300 \\ \hline t_{1/2}\,\,(minutes) & 135 & 112.5 \\ \hline \end{array}$
The order of 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
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]
Select the rate law for reaction $A + B \longrightarrow C$
Exp
$[A]$
$[B]$
Rate
$1$
$0.012$
$0.035$
$0.10$
$2$
$0.024$
$0.070$
$0.80$
$3$
$0.024$
$0.035$
$0.10$
$4$
$0.012$
$0.070$
$0.80$
Select the rate law for reaction $A + B \longrightarrow C$
| Exp | $[A]$ | $[B]$ | Rate |
| $1$ | $0.012$ | $0.035$ | $0.10$ |
| $2$ | $0.024$ | $0.070$ | $0.80$ |
| $3$ | $0.024$ | $0.035$ | $0.10$ |
| $4$ | $0.012$ | $0.070$ | $0.80$ |
For the following rate law determine the unit of rate constant. Rate $=-\frac{d[ R ]}{d t}=k[ A ]^{\frac{1}{2}}[ B ]^{2}$
For the following rate law determine the unit of rate constant. Rate $=-\frac{d[ R ]}{d t}=k[ A ]^{\frac{1}{2}}[ B ]^{2}$
$A + B \to $ products, it is found that the rate of the reaction is proportional to the concentration of $A,$ but it is independent of the concentration of $B$, then
$A + B \to $ products, it is found that the rate of the reaction is proportional to the concentration of $A,$ but it is independent of the concentration of $B$, then