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]
- A
If both Assertion and Reason are correct and the Reason is a correct explanation of the Assertion.
- B
If both Assertion and Reason are correct but Reason is not a correct explanation of the Assertion.
- C
If the Assertion is correct but Reason is incorrect.
- D
If both the Assertion and Reason are incorrect.
Similar Questions
In a reaction, $2X \to Y$ , the concentration of $X$ decreases from $0.50\, M$ to $0.38\, M$ in $10\, min$ . what is the rate of reaction in $Ms^{-1}$ during the interval ?
In a reaction, $2X \to Y$ , the concentration of $X$ decreases from $0.50\, M$ to $0.38\, M$ in $10\, min$ . what is the rate of reaction in $Ms^{-1}$ during the interval ?
The following data was obtained for chemical reaction given below at $975\, \mathrm{~K}$.
$2 \mathrm{NO}_{(\mathrm{g})}+2 \mathrm{H}_{2(\mathrm{~g})} \rightarrow \mathrm{N}_{2(\mathrm{~g})}+2 \mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})}$
$[NO]$
$\mathrm{mol} \mathrm{L}^{-1}$
${H}_{2}$
$\mathrm{mol} \mathrm{L}^{-1}$
Rate
$\mathrm{mol}L^{-1}$ $s^{-1}$
$(A)$
$8 \times 10^{-5}$
$8 \times 10^{-5}$
$7 \times 10^{-9}$
$(B)$
$24 \times 10^{-5}$
$8 \times 10^{-5}$
$2.1 \times 10^{-8}$
$(C)$
$24 \times 10^{-5}$
$32 \times 10^{-5}$
$8.4 \times 10^{-8}$
The order of the reaction with respect to $\mathrm{NO}$ is ..... .
The following data was obtained for chemical reaction given below at $975\, \mathrm{~K}$.
$2 \mathrm{NO}_{(\mathrm{g})}+2 \mathrm{H}_{2(\mathrm{~g})} \rightarrow \mathrm{N}_{2(\mathrm{~g})}+2 \mathrm{H}_{2} \mathrm{O}_{(\mathrm{g})}$
|
$[NO]$ $\mathrm{mol} \mathrm{L}^{-1}$ |
${H}_{2}$ $\mathrm{mol} \mathrm{L}^{-1}$ |
Rate $\mathrm{mol}L^{-1}$ $s^{-1}$ |
|
| $(A)$ | $8 \times 10^{-5}$ | $8 \times 10^{-5}$ | $7 \times 10^{-9}$ |
| $(B)$ | $24 \times 10^{-5}$ | $8 \times 10^{-5}$ | $2.1 \times 10^{-8}$ |
| $(C)$ | $24 \times 10^{-5}$ | $32 \times 10^{-5}$ | $8.4 \times 10^{-8}$ |
The order of the reaction with respect to $\mathrm{NO}$ is ..... .
- [JEE MAIN 2021]
If $‘a’ $ is the initial concentration and $ ‘n’ $ is the order of the reaction and the half life period is $ ‘T’,$ then
If $‘a’ $ is the initial concentration and $ ‘n’ $ is the order of the reaction and the half life period is $ ‘T’,$ then
The rate of a gaseous reaction is given by the expression $K\,[A]\,[B]$. If the volume of the reaction vessel is suddenly reduced to $1/4^{th} $ of the initial volume, the reaction rate relating to original rate will be
The rate of a gaseous reaction is given by the expression $K\,[A]\,[B]$. If the volume of the reaction vessel is suddenly reduced to $1/4^{th} $ of the initial volume, the reaction rate relating to original rate will be
What is the order of a reaction which has a rate expression rate $ = K{[A]^{3/2}}{[B]^{ - 1}}$
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