Medium
For the reaction $H_{2(g)} + Br_{2(g)} \rightarrow 2HBr_{(g)}$,the experimental data suggests the rate law is $\text{Rate} = K[H_2][Br_2]^{1/2}$. Find the order of the reaction and its molecularity.
- AOrder $2$ and molecularity $2$ respectively
- BOrder $1\frac{1}{2}$ and molecularity $2$ respectively
- COrder $2$ and molecularity $1\frac{1}{2}$ respectively
- DOrder $1\frac{1}{2}$ and molecularity $1\frac{1}{2}$ respectively
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Similar Questions
$A_2 + B_2 \to 2AB$; $R.O.R = k[A_2]^a[B_2]^b$
Initial $[A_2]$ Initial $[B_2]$ $R.O.R. (r) \ M s^{-1}$ $0.2$ $0.2$ $0.04$ $0.1$ $0.4$ $0.04$ $0.2$ $0.4$ $0.08$
Order of reaction with respect to $A_2$ and $B_2$ are respectively:
| Initial $[A_2]$ | Initial $[B_2]$ | $R.O.R. (r) \ M s^{-1}$ |
|---|---|---|
| $0.2$ | $0.2$ | $0.04$ |
| $0.1$ | $0.4$ | $0.04$ |
| $0.2$ | $0.4$ | $0.08$ |
Order of reaction with respect to $A_2$ and $B_2$ are respectively:
Medium
View Solution$A$ reaction is first order in terms of $A$ and second order in terms of $B$. What will be the rate of reaction,if the concentration of $B$ is increased two times?
The rate constant value for a reaction is $1.75 \times 10^2 \ L^2 \ mol^{-2} \ sec^{-1}$. The half-life period $t_{1/2} \propto$ . . . . . . .
For which type of reactions,order and molecularity have the same value?
Easy
View SolutionAt what concentration of the reactant (in $M$) are the rate constants for first-order,second-order,and third-order reactions equal?
Easy
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