Medium
The rate equation for the reaction $2A + B \to C$ is found to be: $\text{rate} = k[A][B]$. The correct statement in relation to this reaction is that the
- ARate of formation of $C$ is twice the rate of disappearance of $A$
- B$t_{1/2}$ is a constant
- CUnit of $k$ must be $s^{-1}$
- DValue of $k$ is independent of the initial concentrations of $A$ and $B$
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Similar Questions
The initial rates of decrease of $I_2$ in acetone-iodine reaction catalysed by $H^{+}$ are given in the table.
Experiment Initial $[I_2]$ $(mol \ L^{-1})$ Initial $[H^{+}]$ $(mol \ L^{-1})$ Initial $[CH_3COCH_3]$ $(mol \ L^{-1})$ Initial rate $(mol \ L^{-1} \ s^{-1})$ $1$ $0.01$ $0.1$ $0.1$ $0.096$ $2$ $0.01$ $0.2$ $0.1$ $0.192$ $3$ $0.02$ $0.2$ $0.1$ $0.192$ $4$ $0.01$ $0.2$ $0.2$ $0.384$
The order with respect to $I_2, H^{+}$,acetone and total order of the reaction respectively are:
| Experiment | Initial $[I_2]$ $(mol \ L^{-1})$ | Initial $[H^{+}]$ $(mol \ L^{-1})$ | Initial $[CH_3COCH_3]$ $(mol \ L^{-1})$ | Initial rate $(mol \ L^{-1} \ s^{-1})$ |
| $1$ | $0.01$ | $0.1$ | $0.1$ | $0.096$ |
| $2$ | $0.01$ | $0.2$ | $0.1$ | $0.192$ |
| $3$ | $0.02$ | $0.2$ | $0.1$ | $0.192$ |
| $4$ | $0.01$ | $0.2$ | $0.2$ | $0.384$ |
The order with respect to $I_2, H^{+}$,acetone and total order of the reaction respectively are:
For a given reaction $t_{1/2} = \frac{1}{Ka}$. The order of the reaction is
Medium
View SolutionFor the reaction $aA \to xP$,the rate is $2.4 \ mMs^{-1}$ when $[A] = 2.2 \ M$. When the concentration of $A$ is halved,the rate becomes $0.6 \ mMs^{-1}$. Determine the order of the reaction with respect to $A$.
Medium
View SolutionFill in the blanks:
$1.$ The rate of a zero order reaction depends on the ........... concentration of the reactant.
$2.$ The molecularity of the slow step is equal to the ........... of the overall reaction.
$3.$ Rate $=$ ........ $[A]^x [B]^y$
$1.$ The rate of a zero order reaction depends on the ........... concentration of the reactant.
$2.$ The molecularity of the slow step is equal to the ........... of the overall reaction.
$3.$ Rate $=$ ........ $[A]^x [B]^y$
Difficult
View SolutionFor the reaction,$PCl_5 \longrightarrow PCl_3 + Cl_2$,the rate and rate constant are $1.02 \times 10^{-4} \ mol \ L^{-1} \ s^{-1}$ and $3.4 \times 10^{-5} \ s^{-1}$ respectively at a given instant. The molar concentration of $PCl_5$ at that instant is
MediumKCET 2024
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