Medium
For a reaction,$I^{-} + OCl^{-} \to IO^{-} + Cl^{-}$ in an aqueous medium,the rate of reaction is given by $\frac{d[IO^{-}]}{dt} = K \frac{[I^{-}][OCl^{-}]}{[OH^{-}]}$. The overall order of reaction is
- A$-1$
- B$0$
- C$1$
- D$2$
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Similar Questions
Calculate the order of the reaction with respect to $A$ and $B$ based on the following data:
$[A] \ (mol/L)$ $[B] \ (mol/L)$ Rate $(mol/L \cdot s)$ $0.05$ $0.05$ $1.2 \times 10^{-3}$ $0.10$ $0.05$ $2.4 \times 10^{-3}$ $0.05$ $0.10$ $1.2 \times 10^{-3}$
| $[A] \ (mol/L)$ | $[B] \ (mol/L)$ | Rate $(mol/L \cdot s)$ |
| $0.05$ | $0.05$ | $1.2 \times 10^{-3}$ |
| $0.10$ | $0.05$ | $2.4 \times 10^{-3}$ |
| $0.05$ | $0.10$ | $1.2 \times 10^{-3}$ |
Easy
View SolutionFor the reaction $2NO + Cl_2 \rightarrow 2NOCl$,the following mechanism is proposed. What will be the rate law for the reaction? $NO + Cl_2 \rightleftharpoons NOCl_2$ (fast); $NOCl_2 + NO \rightarrow 2NOCl$ (slow)
Difficult
View SolutionWhich among the following is a false statement?
Easy
View SolutionThe unit of rate constant $K$ for a third-order reaction is . . . . . . .
Half-life of a reaction is found to be inversely proportional to the fifth power of its initial concentration,the order of reaction is
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