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



Related posts:

  1. Order of Reaction The order of reaction may be defined as the sum...
  2. Rate constant or Specific Reaction rate According to collision theory, the rate of the reaction is...
  3. Rate of reactions The rate (speed or velocity) of the reaction may be...
  4. Redox Reaction Worksheet All the chemical reaction in which atoms change their oxidation...
  5. Factors Influencing Rate of Reaction Some important factors which influence the rate of reaction are...