Medium
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.
Reason : It is the mechanism and not the balanced chemical equation for the overall change that governs the reaction rate.
- A$A$. If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.
- B$B$. If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.
- C$C$. If the Assertion is correct but Reason is incorrect.
- D$D$. If both the Assertion and Reason are incorrect.
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Similar Questions
For the reaction $A + B \rightarrow C$, we have the following data:
Initial concentration of $A$ $(M)$ Initial concentration of $B$ $(M)$ Initial Rate $(M \cdot s^{-1})$ $1$ $10$ $100$ $1$ $1$ $1$ $10$ $1$ $10$
The order of the reaction with respect to $A$ and $B$ are:
| Initial concentration of $A$ $(M)$ | Initial concentration of $B$ $(M)$ | Initial Rate $(M \cdot s^{-1})$ |
| $1$ | $10$ | $100$ |
| $1$ | $1$ | $1$ |
| $10$ | $1$ | $10$ |
The order of the reaction with respect to $A$ and $B$ are:
In a reaction $A \rightarrow B$,if the concentration of reactant is increased by $9$ times,then the rate of reaction increases $3$ times. What is the order of reaction?
For the reaction $N_2O_5 \rightarrow 2NO_2 + \frac{1}{2} O_2$,given that:
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?
$-\frac{d[N_2O_5]}{dt} = K_1[N_2O_5]$,
$\frac{d[NO_2]}{dt} = K_2[N_2O_5]$,
$\frac{d[O_2]}{dt} = K_3[N_2O_5]$
What is the relationship between $K_1$,$K_2$,and $K_3$?
Difficult
View SolutionFor a chemical reaction $A + B \rightarrow \text{Product}$,the order is $1$ with respect to $A$ and $B$.
Rate $(mol \ L^{-1} \ s^{-1})$ $[A]$ $(mol \ L^{-1})$ $[B]$ $(mol \ L^{-1})$ $0.10$ $20$ $0.5$ $0.40$ $x$ $0.5$ $0.80$ $40$ $y$
What is the value of $x$ and $y$?
| Rate $(mol \ L^{-1} \ s^{-1})$ | $[A]$ $(mol \ L^{-1})$ | $[B]$ $(mol \ L^{-1})$ |
|---|---|---|
| $0.10$ | $20$ | $0.5$ |
| $0.40$ | $x$ | $0.5$ |
| $0.80$ | $40$ | $y$ |
What is the value of $x$ and $y$?
Which of the following is an example of a second-order reaction?
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