A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is
$(i)$ doubled
$(ii)$ reduced to half $?$
A reaction is second order with respect to a reactant. How is the rate of reaction affected if the concentration of the reactant is
$(i)$ doubled
$(ii)$ reduced to half $?$
Let the concentration of the reactant be $[ A ]=a$
Rate of reaction, $R=k[A]^{2}$
$=k a^{2}$
$(i)$ If the concentration of the reactant is doubled, i.e. $[ A ]=2 a$, then the rate of the reaction would be
$R ^{\prime}=k(2 a)^{2}$
$=4 ka ^{2}$
$=4 R$
Therefore, the rate of the reaction would increase by $4$ times.
$(ii)$ If the concentration of the reactant is reduced to half, i.e. $[ A ]=\frac{1}{2} a$
the reaction would be
$R ^{\prime \prime}=k\left(\frac{1}{2} a\right)^{2}$
$=\frac{1}{4} k a$
$=\frac{1}{4} R$
Therefore, the rate of the reaction would be reduced to ${\frac{1}{4}^{th}}$
Similar Questions
If the concentration is expressed in moles per litre, the unit of the rate constant for a first order reaction is
If the concentration is expressed in moles per litre, the unit of the rate constant for a first order reaction is
${A_2} + {B_2} \to 2AB;R.O.R = k{[{A_2}]^a}{[{B_2}]^b}$
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
For a general reaction $A \to B$, plot of concentration of $A$ vs time is given in figure. Answer the following question on the basis of this graph.
$(i)$ What is the order of the reaction ?
$(ii)$ What is the slope of the curve ?
$(iii)$ What are the units of rate constant ?
For a general reaction $A \to B$, plot of concentration of $A$ vs time is given in figure. Answer the following question on the basis of this graph.
$(i)$ What is the order of the reaction ?
$(ii)$ What is the slope of the curve ?
$(iii)$ What are the units of rate constant ?
If $R = K{[NO]^2}[{O_2}],$ rate constant may be increased by
If $R = K{[NO]^2}[{O_2}],$ rate constant may be increased by
For the following reaction: $NO_2(g) + CO(g) \to NO(g) + CO_2(g)$, the rate law is: Rate $= k \,[NO_2]^2$. If $0.1\,mole$ of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true?
For the following reaction: $NO_2(g) + CO(g) \to NO(g) + CO_2(g)$, the rate law is: Rate $= k \,[NO_2]^2$. If $0.1\,mole$ of gaseous carbon monoxide is added at constant temperature to the reaction mixture which of the following statements is true?
- [AIIMS 2016]