From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(iii)$ $CH _{3} CHO ( g ) \rightarrow CH _{4}( g )+ CO ( g ) \quad$ Rate $=k\left[ CH _{3} CHO \right]^{3 / 2}$
From the rate expression for the following reactions, determine their order of reaction and the dimensions of the rate constants.
$(iii)$ $CH _{3} CHO ( g ) \rightarrow CH _{4}( g )+ CO ( g ) \quad$ Rate $=k\left[ CH _{3} CHO \right]^{3 / 2}$
$(iii)$ Given rate $=k\left[ CH _{3} CHO \right]^{3 / 2}$
Therefore, order of $=\frac{3}{2}$
Dimension of $k=\frac{\text { Rate }}{\left[ CH _{3} CHO \right]^{\frac{3}{2}}}$
$=\frac{m o l\, L^{-1} \,s^{-1}}{\left(m o l \,L^{-1}\right)^{\frac{3}{2}}}$
$=\frac{m o l\, L^{-1} \,s^{-1}}{m o l^{\frac{3}{2}} \,L^{\frac{3}{2}}}$
$=L^{\frac{1}{2}} m o l^{\frac{1}{2}} s^{-1}$
Similar Questions
The following data is given for reaction between $A$ and $B$
$S.NO.$
$[A]$ $mol.L^{-1}$
$[B]$ $mol.L^{-1}$
$Rate$ $mol.L^{-1}\,sec^{-1}$
$I$
$1 \times 10^{-2}$
$2 \times 10^{-2}$
$2 \times 10^{-4}$
$II$
$2 \times 10^{-2}$
$2 \times 10^{-2}$
$4 \times 10^{-4}$
$III$
$2 \times 10^{-2}$
$4 \times 10^{-2}$
$8 \times 10^{-4}$
Which of the following are correct statements -
$(a)$ Rate constant of the reaction $10^{-4}$
$(b)$ Rate law of the reaction is $k[A][B]$
$(c)$ Rate of reaction increases four times on doubling the concentration of both the reactant
The following data is given for reaction between $A$ and $B$
| $S.NO.$ | $[A]$ $mol.L^{-1}$ | $[B]$ $mol.L^{-1}$ | $Rate$ $mol.L^{-1}\,sec^{-1}$ |
| $I$ | $1 \times 10^{-2}$ | $2 \times 10^{-2}$ | $2 \times 10^{-4}$ |
| $II$ | $2 \times 10^{-2}$ | $2 \times 10^{-2}$ | $4 \times 10^{-4}$ |
| $III$ | $2 \times 10^{-2}$ | $4 \times 10^{-2}$ | $8 \times 10^{-4}$ |
Which of the following are correct statements -
$(a)$ Rate constant of the reaction $10^{-4}$
$(b)$ Rate law of the reaction is $k[A][B]$
$(c)$ Rate of reaction increases four times on doubling the concentration of both the reactant
For the non-stoichiometric reaction $2A + B \to C + D,$ the following kinetic data were obtained in three separate experiments, all at $298\,K$.
Initial Conc.
$(A)$
Initial Conc.
$(B)$
Initial rate of
formation of $C\,(mol\, L^-S^-)$
$0.1\,M$
$0.1\,M$
$1.2 \times 10^{-3}$
$0.1\,M$
$0.2\,M$
$1.2 \times 10^{-3}$
$0.2\,M$
$0.1\,M$
$2.4 \times 10^{-3}$
For the reaction the rate of formation of $C$ will be
For the non-stoichiometric reaction $2A + B \to C + D,$ the following kinetic data were obtained in three separate experiments, all at $298\,K$.
| Initial Conc. $(A)$ |
Initial Conc. $(B)$ |
Initial rate of |
| $0.1\,M$ | $0.1\,M$ | $1.2 \times 10^{-3}$ |
| $0.1\,M$ | $0.2\,M$ | $1.2 \times 10^{-3}$ |
| $0.2\,M$ | $0.1\,M$ | $2.4 \times 10^{-3}$ |
For the reaction the rate of formation of $C$ will be
Select the correct statement
Select the correct statement
The rate law for the reaction below is given by the expression $k\left[ A \right]\left[ B \right]$
$A + B \to$ Product
If the concentration of $B$ is increased from $0.1$ to $0.3\, mole$, keeping the value of $A$ at $0.1\, mole$, the rate constant will be
The rate law for the reaction below is given by the expression $k\left[ A \right]\left[ B \right]$
$A + B \to$ Product
If the concentration of $B$ is increased from $0.1$ to $0.3\, mole$, keeping the value of $A$ at $0.1\, mole$, the rate constant will be
- [JEE MAIN 2016]
Which of these does not influence the rate of reaction
Which of these does not influence the rate of reaction