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 $1$.
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 $1$.
Similar Questions
What is the order of reaction' for $A + B \to C$
Observation
$[A]$
$[B]$
Rate of reaction
$1$
$0.1$
$0.1$
$2\times10^{-3}\, mol\, L^{-1}\,sec^{-1}$
$2$
$0.2$
$0.1$
$0.4\times10^{-2}\, mol\, L^{-1}\,sec^{-1}$
$3$
$0.1$
$0.2$
$1.4\times10^{-2}\, mol\, L^{-1}\,sec^{-1}$
What is the order of reaction' for $A + B \to C$
| Observation | $[A]$ | $[B]$ | Rate of reaction |
| $1$ | $0.1$ | $0.1$ | $2\times10^{-3}\, mol\, L^{-1}\,sec^{-1}$ |
| $2$ | $0.2$ | $0.1$ | $0.4\times10^{-2}\, mol\, L^{-1}\,sec^{-1}$ |
| $3$ | $0.1$ | $0.2$ | $1.4\times10^{-2}\, mol\, L^{-1}\,sec^{-1}$ |
${A_2} + {B_2} \to 2AB;R.O.R = k{[{A_2}]^a}{[{B_2}]^b}$
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
The rate constant for the reaction, $2N_2O_5 \to 4NO_2 + O_2$ is $3.0\times 10^{- 4}\,s^{-1}$ . If start made with $1.0\,mol\,L^{-1}$ of $N_2O_5$, calculate the rate of formation of $NO_2$ at the moment of the reaction when concentration of $O_2$ is $0.1\, mol\, L^{-1}$.
The rate constant for the reaction, $2N_2O_5 \to 4NO_2 + O_2$ is $3.0\times 10^{- 4}\,s^{-1}$ . If start made with $1.0\,mol\,L^{-1}$ of $N_2O_5$, calculate the rate of formation of $NO_2$ at the moment of the reaction when concentration of $O_2$ is $0.1\, mol\, L^{-1}$.
- [AIIMS 2011]
The reaction $2{N_2}{O_5}$ $\rightleftharpoons$ $2N{O_2} + {O_2}$ follows first order kinetics. Hence, the molecularity of the reaction is
The reaction $2{N_2}{O_5}$ $\rightleftharpoons$ $2N{O_2} + {O_2}$ follows first order kinetics. Hence, the molecularity of the reaction is
The rate of the simple reaction, $2NO + O_2 \to 2NO_2$, when the volume of the reaction vessel is doubled
The rate of the simple reaction, $2NO + O_2 \to 2NO_2$, when the volume of the reaction vessel is doubled