Medium
The rate law for the reaction $A + B \rightarrow C$ at $25^{\circ} C$ is given by $\text{rate} = k[A][B]^2$. Calculate the rate of reaction if the rate constant at the same temperature is $6.25 \ mol^{-2} \ dm^6 \ s^{-1}$ where $[A] = 1 \ M$ and $[B] = 0.2 \ M$.
- A$0.25 \ mol \ dm^{-3} \ s^{-1}$
- B$0.5 \ mol \ dm^{-3} \ s^{-1}$
- C$0.75 \ mol \ dm^{-3} \ s^{-1}$
- D$1.25 \ mol \ dm^{-3} \ s^{-1}$
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For a chemical reaction,$A + 2B \to C + D$,the rate of reaction increases $3$ times when the concentration of $A$ only is increased $9$ times. While when the concentration of $B$ only is increased $2$ times,the rate of reaction also increases $2$ times. The order of this reaction is:
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$(a)$ Calculate the order of reaction.
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$(b)$ Calculate the value of the rate constant.
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View SolutionWhich among the following reactions can be an example of a pseudo first order reaction?
For the reaction $2A + B \to C$,the values of initial rate at different reactant concentrations are given in the table below: The rate law for the reaction is
$[A] \ (mol \ L^{-1})$ $[B] \ (mol \ L^{-1})$ Initial Rate $(mol \ L^{-1} \ s^{-1})$ $0.05$ $0.05$ $0.045$ $0.10$ $0.05$ $0.090$ $0.20$ $0.10$ $0.72$
| $[A] \ (mol \ L^{-1})$ | $[B] \ (mol \ L^{-1})$ | Initial Rate $(mol \ L^{-1} \ s^{-1})$ |
| $0.05$ | $0.05$ | $0.045$ |
| $0.10$ | $0.05$ | $0.090$ |
| $0.20$ | $0.10$ | $0.72$ |
DifficultJEE MAIN 2019
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