Assertion :The order of a reaction can have fractional value.
Reason : The order of a reaction cannot be written from balanced equation of a reaction.
Assertion :The order of a reaction can have fractional value.
Reason : The order of a reaction cannot be written from balanced equation of a reaction.
- [AIIMS 2008]
- 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
For an elementary reaction, $2A + B \to C + D$ the molecularity is
For an elementary reaction, $2A + B \to C + D$ the molecularity is
Calculate the order of the reaction in $A$ and $B$
$A$
$(mol/l)$
$B$
$(mol/l)$
Rate
$0.05$
$0.05$
$1.2\times 10^{-3}$
$0.10$
$0.05$
$2.4\times 10^{-3}$
$0.05$
$0.10$
$1.2\times 10^{-3}$
Calculate the order of the reaction in $A$ and $B$
|
$A$ $(mol/l)$ |
$B$ $(mol/l)$ |
Rate |
| $0.05$ | $0.05$ | $1.2\times 10^{-3}$ |
| $0.10$ | $0.05$ | $2.4\times 10^{-3}$ |
| $0.05$ | $0.10$ | $1.2\times 10^{-3}$ |
The experimental data for the reaction $2A + {B_2} \to 2AB$ isThe rate equation for the above data is
Exp.
$[A]_0$
$[B]_0$
Rate (mole $s^{-1}$)
$(1)$
$0.50$
$0.50$
$1.6 \times {10^{ - 4}}$
$(2)$
$0.50$
$1.00$
$3.2 \times {10^{ - 4}}$
$(3)$
$1.00$
$1.00$
$3.2 \times {10^4}$
The experimental data for the reaction $2A + {B_2} \to 2AB$ isThe rate equation for the above data is
|
Exp. |
$[A]_0$ |
$[B]_0$ |
Rate (mole $s^{-1}$) |
|
$(1)$ |
$0.50$ |
$0.50$ |
$1.6 \times {10^{ - 4}}$ |
|
$(2)$ |
$0.50$ |
$1.00$ |
$3.2 \times {10^{ - 4}}$ |
|
$(3)$ |
$1.00$ |
$1.00$ |
$3.2 \times {10^4}$ |
- [AIPMT 1997]
The alkaline hydrolysis of ethyl acetate is represented by the equation$C{H_3}COO{C_2}{H_5} + NaOH \to C{H_3}COONa + {C_2}{H_5}OH$ Experimentally it is found that for this reaction$\frac{{dx}}{{dt}} = k[C{H_3}COO{C_2}{H_5}]\,[NaOH]$ Then the reaction is
The alkaline hydrolysis of ethyl acetate is represented by the equation$C{H_3}COO{C_2}{H_5} + NaOH \to C{H_3}COONa + {C_2}{H_5}OH$ Experimentally it is found that for this reaction$\frac{{dx}}{{dt}} = k[C{H_3}COO{C_2}{H_5}]\,[NaOH]$ Then the reaction is
In the following reaction $A \longrightarrow B + C$, rate constant is $0.001\, Ms^{-1}$. If we start with $1\, M$ of $A$ then concentration of $A$ and $B$ after $10\, minutes$ are respectively
In the following reaction $A \longrightarrow B + C$, rate constant is $0.001\, Ms^{-1}$. If we start with $1\, M$ of $A$ then concentration of $A$ and $B$ after $10\, minutes$ are respectively