From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(i)$ $3 NO ( g ) \rightarrow N _{2} O$ $(g)$ Rate $=k[ NO ]^{2}$
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(i)$ $3 NO ( g ) \rightarrow N _{2} O$ $(g)$ Rate $=k[ NO ]^{2}$
$(i)$ Given rate $=k[ NO ]^{2}$
Therefore, order of the reaction $=2$
Dimension of $k=\frac{\text { Rate }}{[ NO ]^{2}}$
$=\frac{\operatorname{mol}\, L^{-1} \,s^{-1}}{\left(\operatorname{mol}\, L^{-1}\right)^{2}}$
$=\frac{\operatorname{mol}\, L^{-1} \,s^{-1}}{\operatorname{mol}^{2} \,L^{-2}}$
$=L \,m o l^{-1}\, s^{-1}$
Similar Questions
${A_2} + {B_2} \to 2AB;R.O.R = k{[{A_2}]^a}{[{B_2}]^b}$
Initial $[A_2]$
Initial $[B_2]$
$R.O.R.\,(r)\,Ms^{-1}$
$0.2$
$0.2$
$0.04$
$0.1$
$0.4$
$0.04$
$0.2$
$0.4$
$0.08$
Order of reaction with respect to $A_2$ and $B_2$ are respectively
${A_2} + {B_2} \to 2AB;R.O.R = k{[{A_2}]^a}{[{B_2}]^b}$
| Initial $[A_2]$ | Initial $[B_2]$ | $R.O.R.\,(r)\,Ms^{-1}$ |
| $0.2$ | $0.2$ | $0.04$ |
| $0.1$ | $0.4$ | $0.04$ |
| $0.2$ | $0.4$ | $0.08$ |
Order of reaction with respect to $A_2$ and $B_2$ are respectively
In the reaction : $P + Q \longrightarrow R + S$ the time taken for $75\%$ reaction of $P$ is twice the time taken for $50\%$ reaction of $P$. The concentration of $Q$ varies with reaction time as shown in the figure. The overall order of the reaction is
In the reaction : $P + Q \longrightarrow R + S$ the time taken for $75\%$ reaction of $P$ is twice the time taken for $50\%$ reaction of $P$. The concentration of $Q$ varies with reaction time as shown in the figure. The overall order of the reaction is
For a certain reaction, the rate $=k[A]^2[B]$, when the initial concentration of $A$ is tripled keeping concentration of $B$ constant, the initial rate would
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- [NEET 2023]
For a certain reaction, $10\%$ of the reactant dissociates in $1\, hour$, $20\%$ of the reactant dissociate in $2\, hour$, $30\%$ of the reactant dissociates in $3\, hour$. Then the units of rate constant is
For a certain reaction, $10\%$ of the reactant dissociates in $1\, hour$, $20\%$ of the reactant dissociate in $2\, hour$, $30\%$ of the reactant dissociates in $3\, hour$. Then the units of rate constant is
Reaction : $KCl{O_3} + 6FeS{O_4} + 3{H_2}S{O_4} \to $ $KCl + 3F{e_2}{\left( {S{O_4}} \right)_3} + 3{H_2}O$
Which is True $(T)$ and False $(F)$ in the following sentence ?
The order of this reaction is $10$.
Reaction : $KCl{O_3} + 6FeS{O_4} + 3{H_2}S{O_4} \to $ $KCl + 3F{e_2}{\left( {S{O_4}} \right)_3} + 3{H_2}O$
Which is True $(T)$ and False $(F)$ in the following sentence ?
The order of this reaction is $10$.