Question

Explain the zero order of reaction by giving examples.

Hint:

Zero-order reactions are rare, typically occurring on a surface or where a catalyst is involved.

Answer 1

Step 1: Define Zero Order Reaction
A zero-order reaction is one in which the rate of reaction is independent of the concentration of the reactants. Mathematically, it is expressed as: \[ \text{Rate} = k \] where \(k\) is the rate constant. The concentration of reactants does not affect the rate, and the reaction rate remains constant over time.
Step 2: Example of Zero Order Reaction
An example of a zero-order reaction is the decomposition of hydrogen peroxide on the surface of platinum: \[ 2H_2O_2 \xrightarrow{Pt} 2H_2O + O_2 \] In this reaction, the rate of decomposition is independent of the concentration of hydrogen peroxide. Final Answer: In zero-order reactions, the rate is constant and does not depend on the concentration of reactants. Correct Answer: Zero-order reactions have a constant rate, unaffected by reactant concentration.