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
Identify the correct statement regarding the order of reaction from the following.
The rate constant of a first order reaction at $27^{\circ} C$ is $10^{-3} \ min^{-1}$. The temperature coefficient of this reaction is $2$. What is the rate constant (in $min^{-1}$) at $17^{\circ} C$ for this reaction?
Write the formula for the rate of reaction $R \to P$ for zero-order and first-order reactions.
Easy
View SolutionThe reaction between $A$ and $B$ is first order with respect to $A$ and zero order with respect to $B$. Fill in the blanks in the following table:
Experiment $[A] / mol \, L^{-1}$ $[B] / mol \, L^{-1}$ Initial rate / $mol \, L^{-1} \, min^{-1}$ $I$ $0.1$ $0.1$ $2.0 \times 10^{-2}$ $II$ $-$ $0.2$ $4.0 \times 10^{-2}$ $III$ $0.4$ $0.4$ $-$ $IV$ $-$ $0.2$ $2.0 \times 10^{-2}$
| Experiment | $[A] / mol \, L^{-1}$ | $[B] / mol \, L^{-1}$ | Initial rate / $mol \, L^{-1} \, min^{-1}$ |
|---|---|---|---|
| $I$ | $0.1$ | $0.1$ | $2.0 \times 10^{-2}$ |
| $II$ | $-$ | $0.2$ | $4.0 \times 10^{-2}$ |
| $III$ | $0.4$ | $0.4$ | $-$ |
| $IV$ | $-$ | $0.2$ | $2.0 \times 10^{-2}$ |
Difficult
View SolutionIf the surface area of the reactants increases,then the order of the reaction:
Easy
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