For a reactions $A + B \to $product, it was found that rate of reaction increases four times if concentration of $ ‘A’$ is doubled, but the rate of reaction remains unaffected. If concentration of $‘B’ $ is doubled. Hence, the rate law for the reaction is
For a reactions $A + B \to $product, it was found that rate of reaction increases four times if concentration of $ ‘A’$ is doubled, but the rate of reaction remains unaffected. If concentration of $‘B’ $ is doubled. Hence, the rate law for the reaction is
- A
${\rm{rate}} = k[A][B]$
- B
${\rm{rate}} = k{[A]^2}$
- C
${\rm{rate}} = k{[A]^2}{[B]^1}$
- D
${\rm{rate}} = k{[A]^2}{[B]^2}$
Similar Questions
The following results have been obtained during the kinetic studies of the reaction:
$2 A+B \rightarrow C+D$
Experiment
$[ A ] / mol L ^{-1}$
$[ B ] / mol L ^{-1}$
Initial rate of formation of $D / mol \,L ^{-1} \,min ^{-1}$
$I$
$0.1$
$0.1$
$6.0 \times 10^{-3}$
$II$
$0.3$
$0.2$
$7.2 \times 10^{-2}$
$III$
$0.3$
$0.4$
$2.88 \times 10^{-1}$
$IV$
$0.4$
$0.1$
$2.40 \times 10^{-2}$
Determine the rate law and the rate constant for the reaction.
The following results have been obtained during the kinetic studies of the reaction:
$2 A+B \rightarrow C+D$
| Experiment | $[ A ] / mol L ^{-1}$ | $[ B ] / mol L ^{-1}$ | Initial rate of formation of $D / mol \,L ^{-1} \,min ^{-1}$ |
| $I$ | $0.1$ | $0.1$ | $6.0 \times 10^{-3}$ |
| $II$ | $0.3$ | $0.2$ | $7.2 \times 10^{-2}$ |
| $III$ | $0.3$ | $0.4$ | $2.88 \times 10^{-1}$ |
| $IV$ | $0.4$ | $0.1$ | $2.40 \times 10^{-2}$ |
Determine the rate law and the rate constant for the reaction.
For a reaction $A+ B\to $ Products, the rate law is - Rate $=$ $k\,[A]\, [B]^{\frac {3}{2}}$ . Can the reaction be an elementary reaction ? Explain.
For a reaction $A+ B\to $ Products, the rate law is - Rate $=$ $k\,[A]\, [B]^{\frac {3}{2}}$ . Can the reaction be an elementary reaction ? Explain.
The rate of disappearance of $S{O_2}$ in the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ is $1.28 \times {10^{ - 3}}g/sec$ then the rate of formation of $S{O_3}$ is
The rate of disappearance of $S{O_2}$ in the reaction $2S{O_2} + {O_2} \to 2S{O_3}$ is $1.28 \times {10^{ - 3}}g/sec$ then the rate of formation of $S{O_3}$ is
Assertion : In rate law, unlike in the expression for equilibrium constants, the exponents for concentrations do not necessarily match the stoichiometric coefficients.
Reason : It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.
Assertion : In rate law, unlike in the expression for equilibrium constants, the exponents for concentrations do not necessarily match the stoichiometric coefficients.
Reason : It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.
- [AIIMS 2009]
For conversion of compound $A \rightarrow B$, the rate constant of the reaction was found to be $4.6 \times 10^{-5}\,L\, mol ^{-1}\, s ^{-1}$. The order of the reaction is $..........$
For conversion of compound $A \rightarrow B$, the rate constant of the reaction was found to be $4.6 \times 10^{-5}\,L\, mol ^{-1}\, s ^{-1}$. The order of the reaction is $..........$
- [JEE MAIN 2023]