Difficult
The rate law for the reaction below is given by the expression $Rate = k[A][B]$.
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:
$A + B \to \text{Product}$
If the concentration of $B$ is increased from $0.1 \ M$ to $0.3 \ M$,keeping the concentration of $A$ constant at $0.1 \ M$,the rate constant $(k)$ will be:
- A$3k$
- B$9k$
- C$k/3$
- D$k$
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Similar Questions
Which among the following is a false statement?
Easy
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 SolutionConsider the gaseous reaction $A_2 + B_2 \rightarrow 2 AB$. The following data was obtained for the above reaction:
$[A_2]_0$ $[B_2]_0$ Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$ $0.1 \ M$ $0.1 \ M$ $2.5 \times 10^{-4}$ $0.2 \ M$ $0.1 \ M$ $5.0 \times 10^{-4}$ $0.2 \ M$ $0.2 \ M$ $1.0 \times 10^{-3}$
The value of the rate constant for the above reaction is:
| $[A_2]_0$ | $[B_2]_0$ | Initial rate of formation of $AB$ $(mol \ L^{-1} s^{-1})$ |
| $0.1 \ M$ | $0.1 \ M$ | $2.5 \times 10^{-4}$ |
| $0.2 \ M$ | $0.1 \ M$ | $5.0 \times 10^{-4}$ |
| $0.2 \ M$ | $0.2 \ M$ | $1.0 \times 10^{-3}$ |
The value of the rate constant for the above reaction is:
DifficultTS EAMCET 2024
View SolutionThe half-lives of two samples are $0.1 \ s$ and $0.4 \ s$. Their respective concentrations are $200$ and $50$. What is the order of the reaction?
Medium
View SolutionWhich of the following is a unimolecular reaction?
Easy
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