Difficult
The rate constant for a second order reaction,$A \rightarrow \text{Product}$ is $1.62 \ M^{-1} \ s^{-1}$. What will be the rate of reaction when concentration of reactant is $2 \times 10^{-3} \ M$ (in $M \ s^{-1}$)?
- A$3.24 \times 10^{-3}$
- B$3.24 \times 10^{-6}$
- C$6.48 \times 10^{-6}$
- D$2 \times 10^{-3}$
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The rate of reaction between two reactants $A$ and $B$ decreases by a factor of $4$ if the concentration of reactant $B$ is doubled. The order of this reaction with respect to reactant $B$ is
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View SolutionCalculate the order of the reaction with respect to $A$ and $B$ based on the following data:
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| $[A] \ (mol/L)$ | $[B] \ (mol/L)$ | Rate $(mol/L \cdot s)$ |
| $0.05$ | $0.05$ | $1.2 \times 10^{-3}$ |
| $0.10$ | $0.05$ | $2.4 \times 10^{-3}$ |
| $0.05$ | $0.10$ | $1.2 \times 10^{-3}$ |
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