Difficult
For the reaction $2NOBr(g) \rightarrow 2NO(g) + Br_2(g)$, the rate law is $r = k[NOBr]^2$. If the rate constant $k = 1.62 \times 10^{-2} \text{ L mol}^{-1} \text{ s}^{-1}$ and the concentration of $[NOBr] = 2 \times 10^{-3} \text{ mol L}^{-1}$, what is the rate of reaction?
- A$6.48 \times 10^{-8} \text{ mol L}^{-1} \text{ s}^{-1}$
- B$3.24 \times 10^{-8} \text{ mol L}^{-1} \text{ s}^{-1}$
- C$1.62 \times 10^{-8} \text{ mol L}^{-1} \text{ s}^{-1}$
- D$8.10 \times 10^{-8} \text{ mol L}^{-1} \text{ s}^{-1}$
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Similar Questions
The rate constant for the reaction $2N_2O_5 \to 4NO_2 + O_2$ is $3.0 \times 10^{-5} \, sec^{-1}$. If the rate is $2.40 \times 10^{-5} \, M \, sec^{-1}$,then the concentration of $N_2O_5$ (in $M$) is?
Medium
View SolutionThe reaction $3ClO^{-} \rightarrow ClO_{3}^{-} + 2Cl^{-}$ occurs in the following two steps:
$(i)$ $ClO^{-} + ClO^{-} \xrightarrow{K_{1}} ClO_{2}^{-} + Cl^{-}$ (Slow step)
$(ii)$ $ClO_{2}^{-} + ClO^{-} \xrightarrow{K_{2}} ClO_{3}^{-} + Cl^{-}$ (Fast step)
Then the rate of the given reaction is equal to . . . . . . .
$(i)$ $ClO^{-} + ClO^{-} \xrightarrow{K_{1}} ClO_{2}^{-} + Cl^{-}$ (Slow step)
$(ii)$ $ClO_{2}^{-} + ClO^{-} \xrightarrow{K_{2}} ClO_{3}^{-} + Cl^{-}$ (Fast step)
Then the rate of the given reaction is equal to . . . . . . .
For the non-stoichiometric reaction $2A + B \to C + D$,the following kinetic data were obtained in three separate experiments,all at $298 \ K$.
Initial Conc. $(A)$ Initial Conc. $(B)$ Initial rate of formation of $C \ (mol \ L^{-1} \ s^{-1})$ $0.1 \ M$ $0.1 \ M$ $1.2 \times 10^{-3}$ $0.1 \ M$ $0.2 \ M$ $1.2 \times 10^{-3}$ $0.2 \ M$ $0.1 \ M$ $2.4 \times 10^{-3}$
For the reaction,the rate of formation of $C$ will be:
| Initial Conc. $(A)$ | Initial Conc. $(B)$ | Initial rate of formation of $C \ (mol \ L^{-1} \ s^{-1})$ |
| $0.1 \ M$ | $0.1 \ M$ | $1.2 \times 10^{-3}$ |
| $0.1 \ M$ | $0.2 \ M$ | $1.2 \times 10^{-3}$ |
| $0.2 \ M$ | $0.1 \ M$ | $2.4 \times 10^{-3}$ |
For the reaction,the rate of formation of $C$ will be:
Medium
View SolutionIn a reaction,$A + B \rightarrow$ product,the rate is doubled when the concentration of $B$ is doubled,and the rate increases by a factor of $8$ when the concentrations of both the reactants $(A$ and $B)$ are doubled. The rate law for the reaction can be written as:
For a reaction,$A + B \longrightarrow \text{product}$,it is found that the rate law is $r = k[A]^{1.5}[B]^{2.5}$. What is the order of reaction?
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