Medium
Identify the order of reaction for which the unit of the rate constant is $\text{mol dm}^{-3} \text{s}^{-1}$.
- A$0$
- B$1$
- C$2$
- D$3$
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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
MediumAIEEE 2004
View SolutionFor the reaction $A + B \to \text{products}$,what will be the order of reaction with respect to $A$ and $B$?
$Exp.$ $[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Initial rate $(mol \ L^{-1} \ s^{-1})$ $1$ $2.5 \times 10^{-4}$ $3 \times 10^{-5}$ $5 \times 10^{-4}$ $2$ $5 \times 10^{-4}$ $6 \times 10^{-5}$ $4 \times 10^{-3}$ $3$ $1 \times 10^{-3}$ $6 \times 10^{-5}$ $1.6 \times 10^{-2}$
| $Exp.$ | $[A] \ (mol \ L^{-1})$ | $[B] \ (mol \ L^{-1})$ | Initial rate $(mol \ L^{-1} \ s^{-1})$ |
| $1$ | $2.5 \times 10^{-4}$ | $3 \times 10^{-5}$ | $5 \times 10^{-4}$ |
| $2$ | $5 \times 10^{-4}$ | $6 \times 10^{-5}$ | $4 \times 10^{-3}$ |
| $3$ | $1 \times 10^{-3}$ | $6 \times 10^{-5}$ | $1.6 \times 10^{-2}$ |
In the reaction $A + B \to \text{Products}$,if $B$ is taken in excess,then it is an example of
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View SolutionHow can you determine the rate law of the following reaction?
$2 \, NO \, (g) + O_2 \, (g) \to 2 \, NO_2 \, (g)$
$2 \, NO \, (g) + O_2 \, (g) \to 2 \, NO_2 \, (g)$
Easy
View SolutionThe rate constant of which of the following reactions is independent of the concentration of the reactants?
Medium
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