(A) The rate constant $(K)$ for a reaction is independent of time at a constant temperature. The unit of the rate constant given is $\text{L mol}^{-1}

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(A) The rate constant $(K)$ for a reaction is independent of time at a constant temperature. The unit of the rate constant given is $\text{L mol}^{-1} \text{ s}^{-1}$ (or $\text{M}^{-1} \text{ s}^{-1}$). For a reaction of order $n$,the unit of the rate constant is $(\text{mol L}^{-1})^{1-n} \text{ s}^{-1}$. Comparing the units: For $n = 2$,the unit is $(\text{mol L}^{-1})^{1-2} \text{ s}^{-1} = \text{mol}^{-1} \text{ L s}^{-1} = \text{L mol}^{-1} \text{ s}^{-1}$. Since the given unit matches the unit for a second-order reaction,the order of the reaction is $2$.

Class 12 Chemistry Chemical Kinetics Rate law , Rate constant , Order of Reaction and Molecularity

Medium

For the reaction $2A + B \rightarrow \text{Product}$,the rate constant $(K)$ is $2.5 \times 10^{-5} \text{ L mol}^{-1} \text{ s}^{-1}$ after $15 \text{ s}$,$2.60 \times 10^{-5} \text{ L mol}^{-1} \text{ s}^{-1}$ after $30 \text{ s}$,and $2.55 \times 10^{-5} \text{ L mol}^{-1} \text{ s}^{-1}$ after $50 \text{ s}$. What is the order of the reaction?

A
$2$
B
$3$
C
$0$
D
$1$

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Chemical Kinetics

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Rate law , Rate constant , Order of Reaction and Molecularity

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From the rate expression for the following reaction,determine its order of reaction and the dimensions of the rate constant.
$H_2 O_2+3 I^{-}+2 H^{+} \rightarrow 2 H_2 O+I_3^{-} \text { Rate }=k\left[H_2 O_2\right]\left[I^{-}\right]$

The rate of the reaction: $2N_2O_5 \rightarrow 4NO_2 + O_2$ can be written in three ways.
$-\frac{d[N_2O_5]}{dt} = k[N_2O_5]$
$\frac{d[NO_2]}{dt} = k'[N_2O_5]$ ; $\frac{d[O_2]}{dt} = k''[N_2O_5]$
The relationship between $k$ and $k'$ and between $k$ and $k''$ are: