Difficult
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 $(mol \ L^{-1} \ s^{-1})$ |
| $0.05$ | $0.05$ | $0.045$ |
| $0.10$ | $0.05$ | $0.090$ |
| $0.20$ | $0.10$ | $0.72$ |
- ARate $= k[A]^2[B]^2$
- BRate $= k[A][B]^2$
- CRate $= k[A][B]$
- DRate $= k[A]^2[B]$
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Similar Questions
$A \rightarrow$ products ($1^{st}$ order reaction). Three sets of experiment were performed for a reaction under similar experimental conditions. Run $1 \Rightarrow 100 \ mL$ of $10 \ M$ solution of reactant $A$. Run $2 \Rightarrow 200 \ mL$ of $10 \ M$ solution of reactant $A$. Run $3 \Rightarrow 100 \ mL$ of $10 \ M$ solution of reactant $A + 100 \ mL$ of $H_2O$ added. The correct variation of rate of reaction is:
DifficultJEE MAIN 2026
View SolutionBy “the overall order of a reaction”,we mean
Easy
View Solution$A_2 + B_2 \to 2AB$; $R.O.R = k[A_2]^a[B_2]^b$
Initial $[A_2]$ Initial $[B_2]$ $R.O.R. (r) \ M s^{-1}$ $0.2$ $0.2$ $0.04$ $0.1$ $0.4$ $0.04$ $0.2$ $0.4$ $0.08$
Order of reaction with respect to $A_2$ and $B_2$ are respectively:
| Initial $[A_2]$ | Initial $[B_2]$ | $R.O.R. (r) \ M s^{-1}$ |
|---|---|---|
| $0.2$ | $0.2$ | $0.04$ |
| $0.1$ | $0.4$ | $0.04$ |
| $0.2$ | $0.4$ | $0.08$ |
Order of reaction with respect to $A_2$ and $B_2$ are respectively:
Medium
View Solution........ of a reaction cannot be determined experimentally.
An elementary reaction between $A$ and $B$ is a second order reaction. Which of the following rate equations must be correct?
Medium
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