# 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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