State a condition under which a bimolecular reaction is kinetically first order reaction.
State a condition under which a bimolecular reaction is kinetically first order reaction.
A bimolecular reaction becomes first order reaction when one of the reactant is in excess.
$\underset{\text { Ethyl acetate }}{\mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}+}+\mathrm{H}_{2} \mathrm{O} \rightarrow \underset{\text { Ethenoic acid }}{\mathrm{CH}_{3} \mathrm{COOH}}+\underset{\begin{array}{l}\mathrm{CO}_{2} \mathrm{H}_{5} \mathrm{OH} \\ \text { Ethenol }\end{array}}{\mathrm{C}}$
This reaction is bimolecular but its order depends only on conc. of $\mathrm{CH}_{3} \mathrm{COOC}_{2} \mathrm{H}_{5}$ and $\left[\mathrm{H}_{2} \mathrm{O}\right]$ almost remain constant.
Similar Questions
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
Order of radioactive disintegration reaction is
Order of radioactive disintegration reaction is
For any reaction, if we plot a graph between time '$t$' and $\log (a - x)$, a simple line is obtained. The order of reaction is
For any reaction, if we plot a graph between time '$t$' and $\log (a - x)$, a simple line is obtained. The order of reaction is
The reaction of formation of phosgene from $CO$ and $Cl_2$ is $CO + Cl_2 \to COCl_2.$ The proposed mechanism is
$(i)$ $C{l_2}\,\underset{{{k_2}}}{\overset{{{k_1}}}{\longleftrightarrow}}\,2Cl$
$(ii)$ $Cl + CO\,\underset{{{k_4}}}{\overset{{{k_3}}}{\longleftrightarrow}}\,COCl$
$(iii)$ $COCl\, + \,C{l_2}\,\,\xrightarrow{{{k_5}}}\,COC{l_2}\, + \,Cl$ (slow)
Find the correct expression of rate law
The reaction of formation of phosgene from $CO$ and $Cl_2$ is $CO + Cl_2 \to COCl_2.$ The proposed mechanism is
$(i)$ $C{l_2}\,\underset{{{k_2}}}{\overset{{{k_1}}}{\longleftrightarrow}}\,2Cl$
$(ii)$ $Cl + CO\,\underset{{{k_4}}}{\overset{{{k_3}}}{\longleftrightarrow}}\,COCl$
$(iii)$ $COCl\, + \,C{l_2}\,\,\xrightarrow{{{k_5}}}\,COC{l_2}\, + \,Cl$ (slow)
Find the correct expression of rate law
The data for the reaction $A + B \to C$ isThe rate law corresponds to the above data is
Exp.
$[A]_0$
$[B]_0$
Initial rate
$(1)$
$0.012$
$0.035$
$0.10$
$(2)$
$0.024$
$0.070$
$0.80$
$(3)$
$0.024$
$0.035$
$0.10$
$(4)$
$0.012$
$0.070$
$0.80$
The data for the reaction $A + B \to C$ isThe rate law corresponds to the above data is
|
Exp. |
$[A]_0$ |
$[B]_0$ |
Initial rate |
|
$(1)$ |
$0.012$ |
$0.035$ |
$0.10$ |
|
$(2)$ |
$0.024$ |
$0.070$ |
$0.80$ |
|
$(3)$ |
$0.024$ |
$0.035$ |
$0.10$ |
|
$(4)$ |
$0.012$ |
$0.070$ |
$0.80$ |
- [AIPMT 1994]