Write general equation of reaction and explain - what is order of reaction ? Which is its value ?
Write general equation of reaction and explain - what is order of reaction ? Which is its value ?
General Reaction : $a \mathrm{~A}+b \mathrm{~B} \rightarrow c \mathrm{C}+d \mathrm{D}$
The differential rate expression of reaction is as under.
Rate $=-\frac{\mathrm{d}[\mathrm{R}]}{\mathrm{dt}}=k[\mathrm{~A}]^{x}[\mathrm{~B}]^{y}$
Where, the value of $x$ and $y$ are determine experimentally which are same or not to $a$ and $b$.
Where, $x$ and $y$ indicate how sensitive the rate is to the change in concentration of $\mathrm{A}$ and $\mathrm{B}$.
$(i)$ $x$ represent the order with respect to the reactant $\mathrm{A}$.
$(ii)$ $y$ represent the order with respect to the reactant $\mathrm{B}$.
$(iii)$ $(x+y)=$ Overall order of a reaction.
Order of Reaction : The sum of powers of the concentration of the reactants in the rate law expression is called the order of that chemical reaction.
Order of a reaction can be $0,1,2,3$ and even a fraction, these values are always determined by experimentally.
Similar Questions
For the elementary reaction $M \rightarrow N$, the rate of disappearance of $M$ increases by a factor of $8$ upon doubling the concentration of $M$. The order of the reaction with respect to $M$ is :
For the elementary reaction $M \rightarrow N$, the rate of disappearance of $M$ increases by a factor of $8$ upon doubling the concentration of $M$. The order of the reaction with respect to $M$ is :
- [IIT 2014]
Write the rate equation for the reaction $2A + B\to C$ if the order of the reaction is zero.
Write the rate equation for the reaction $2A + B\to C$ if the order of the reaction is zero.
$2 NO ( g )+ Cl _{2}( g ) \rightleftharpoons 2 NOCl ( s )$
This reaction was studied at $-10^{\circ} C$ and the following data was obtained
run
$[ NO ]_{0}$
$\left[ Cl _{2}\right]_{0}$
$r _{0}$
$1$
$0.10$
$0.10$
$0.18$
$2$
$0.10$
$0.20$
$0.35$
$3$
$0.20$
$0.20$
$1.40$
$[ NO ]_{0}$ and $\left[ Cl _{2}\right]_{0}$ are the initial concentrations and $r _{0}$ is the initial reaction rate.
The overall order of the reaction is ..........
(Round off to the Nearest Integer).
$2 NO ( g )+ Cl _{2}( g ) \rightleftharpoons 2 NOCl ( s )$
This reaction was studied at $-10^{\circ} C$ and the following data was obtained
| run | $[ NO ]_{0}$ | $\left[ Cl _{2}\right]_{0}$ | $r _{0}$ |
| $1$ | $0.10$ | $0.10$ | $0.18$ |
| $2$ | $0.10$ | $0.20$ | $0.35$ |
| $3$ | $0.20$ | $0.20$ | $1.40$ |
$[ NO ]_{0}$ and $\left[ Cl _{2}\right]_{0}$ are the initial concentrations and $r _{0}$ is the initial reaction rate.
The overall order of the reaction is ..........
(Round off to the Nearest Integer).
- [JEE MAIN 2021]
The mechanism of the reaction,
$2NO(g) + 2{H_2}(g) \to {N_2}(g) + 2{H_2}O(g)$ is :
Step $1$ : $2NO(g) + {H_2}(g)\xrightarrow{{slow}}{N_2} + {H_2}{O_2}$
Step : $2$ ${H_2}{O_2} + {H_2}\xrightarrow{{fast}}2{H_2}O$
Then the correct statement is
The mechanism of the reaction,
$2NO(g) + 2{H_2}(g) \to {N_2}(g) + 2{H_2}O(g)$ is :
Step $1$ : $2NO(g) + {H_2}(g)\xrightarrow{{slow}}{N_2} + {H_2}{O_2}$
Step : $2$ ${H_2}{O_2} + {H_2}\xrightarrow{{fast}}2{H_2}O$
Then the correct statement is
For a reaction $A \to B$, the rate of reaction quadrupled when the concentration of $A$ is doubled. The rate expression of the reaction is $r = K{(A)^n}$. when the value of $n$ is
For a reaction $A \to B$, the rate of reaction quadrupled when the concentration of $A$ is doubled. The rate expression of the reaction is $r = K{(A)^n}$. when the value of $n$ is