For the reaction $A + B \to$ products,doubling the concentration of $A$ the rate of the reaction is doubled,but on doubling the concentration of $B$ the rate remains unaltered. The overall order of the reaction is:
- A$1$
- B$0$
- C$2$
- D$3$
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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 $2FeCl_3 + SnCl_2 \to 2FeCl_2 + SnCl_4$ is an example of
MediumAIPMT 1996
View SolutionSelect the rate law that corresponds to the data shown for the following reaction $A + B \to C$
$Expt. \ No.$ $[A]$ $[B]$ $Initial \ Rate$ $1$ $0.012$ $0.035$ $0.10$ $2$ $0.024$ $0.070$ $0.80$ $3$ $0.024$ $0.035$ $0.10$ $4$ $0.012$ $0.070$ $0.80$
| $Expt. \ No.$ | $[A]$ | $[B]$ | $Initial \ Rate$ |
|---|---|---|---|
| $1$ | $0.012$ | $0.035$ | $0.10$ |
| $2$ | $0.024$ | $0.070$ | $0.80$ |
| $3$ | $0.024$ | $0.035$ | $0.10$ |
| $4$ | $0.012$ | $0.070$ | $0.80$ |
DifficultAIIMS 2012
View SolutionFor a chemical reaction,the rate law is $\text{rate} = k[A]^2[B]$. If $[A]$ is doubled at constant $[B]$,the rate of reaction:
Why is molecularity applicable only for elementary reactions,while order is applicable for both elementary and complex reactions?
Easy
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