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
In a reaction $A_2B_3(g) \to A_2(g) + \frac{3}{2}B_2(g)$, the pressure increases from $60$ torr to $75$ torr in $2.5\, minutes$. The rate of disappearance of $A_2B_3$ is ........ $torr\, min^{-1}$
In a reaction $A_2B_3(g) \to A_2(g) + \frac{3}{2}B_2(g)$, the pressure increases from $60$ torr to $75$ torr in $2.5\, minutes$. The rate of disappearance of $A_2B_3$ is ........ $torr\, min^{-1}$
Write differential rate expression of following reaction and give its order of reaction :
$5 B r^{-}+B r O_{3}^-+6 H^{+} \rightarrow 3 B r_{2}+3 H_{2} O$
Write differential rate expression of following reaction and give its order of reaction :
$5 B r^{-}+B r O_{3}^-+6 H^{+} \rightarrow 3 B r_{2}+3 H_{2} O$
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
The conversion of $A \to B$ follows second order kinetics. Doubling the concentration of $A$ will increase the rate of formation of $B$ by a factor
The conversion of $A \to B$ follows second order kinetics. Doubling the concentration of $A$ will increase the rate of formation of $B$ by a factor
Assertion : The kinetics of the reaction -
$mA + nB + pC \to m' X + n 'Y + p 'Z$
obey the rate expression as $\frac{{dX}}{{dt}} = k{[A]^m}{[B]^n}$.
Reason : The rate of the reaction does not depend upon the concentration of $C$.
Assertion : The kinetics of the reaction -
$mA + nB + pC \to m' X + n 'Y + p 'Z$
obey the rate expression as $\frac{{dX}}{{dt}} = k{[A]^m}{[B]^n}$.
Reason : The rate of the reaction does not depend upon the concentration of $C$.
- [AIIMS 2017]