Zero Order Reaction

Zero Order Reaction

If the rate of reaction is independent of the concentration of the reactant then the reaction is called zero order reaction e.g.

A \to \text{product} \\[3mm] r = -\dfrac{d[A]}{dt} = k


If ‘a’ is the initial concentration and is the amount decomposed in time ‘t’ then

k = \dfrac{a- (a- x)}{t} = \dfrac{x}{t}


Characteristics of Zero Order Reactions

(i)                  \text{Rate} = k[\text{Reactant}]^0


(ii)                t_{1/2} = \dfrac{a}{k} \text{or} t_{1/2} \propto a


(iii)               Unit of k = mol L^{-1} time^{-1}


(iv)              Examples; H_2Cl_2 \to 2HCl \\[3mm] 2NH_3 \overset{MO}{\rightarrow} N_2 + 3H_2 \\[3mm] N_2O \overset{Pt}{\rightarrow} N_2 + \dfrac{1}{2}O_2

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