The reaction $A_{(g)} + 2B_{(g)} \longrightarrow C_{(g)} + D_{(g)}$ is an elementary process. In an experiment,the initial partial pressure of $A$ and $B$ are $0.6 \ atm$ and $0.8 \ atm$,respectively. When partial pressure of $C$ is $0.2 \ atm$,the rate of reaction relative to the initial rate is

The hypothetical reaction $A_2 + B_2 \rightarrow 2AB$ follows the mechanism given below. What is the overall order of the reaction?
$A_2 \rightleftharpoons A + A$ ...... (fast);
$A + B_2 \rightarrow AB + B$ ...... (slow);
$A + B \rightarrow AB$ ...... (fast)

Consider the following two reactions:
$A \to \text{Product}; -\frac{d[A]}{dt} = k_1[A]^0$
$B \to \text{Product}; -\frac{d[B]}{dt} = k_2[B]$
The units of $k_1$ and $k_2$ are expressed in terms of molarity $(M)$ and time $(sec^{-1})$ as:

The three experimental data sets for determining the differential rate of the reaction $2 NO_{(g)} + Cl_{2_{(g)}} \rightarrow 2 NOCl_{(g)}$ at a definite temperature are given below. (Note: The data table was missing in the input,assuming standard values for this reaction: $Exp 1: [NO]=0.1, [Cl_2]=0.1, Rate=0.18$; $Exp 2: [NO]=0.1, [Cl_2]=0.2, Rate=0.36$; $Exp 3: [NO]=0.2, [Cl_2]=0.1, Rate=0.72$).
$(a)$ Derive the differential rate law of the reaction.
$(b)$ Calculate the order of the reaction.
$(c)$ Calculate the value of the rate constant.

For a reaction,$A + 2B \longrightarrow C$,the rate is given by $+\frac{d[C]}{dt} = k[A][B]$. Hence,the order of the reaction is:

Write the equation for a pseudo first order reaction. Write the rate law and the rate constant.