Zero, First and Second-Order Reactions
The comparison of zero order, with the first-order and second-order reactions is as follows:
Features | Zero-Order | First-Order | Second-Order |
---|---|---|---|
Rate law | Rate = K | Rate = k[A] | Rate = k[A]2 or k[A][B] |
Integrated rate law | [A] = -kt + [A]_0 | ln[A] = -kt + ln[A]_0 | 1/[A] = kt + 1/[A]_0 |
Graphical behavior | Concentration vs. time yields a straight line with a negative slope | ln[Concentration] vs. time yields a straight line | 1/[Concentration] vs. time yields a straight line |
Half life time | Half-life is directly proportional to the initial concentration | Constant half-life | Half-life increases with decreasing concentration |
Reaction order | Zero order with respect to reactant | First order with respect to reactant | Second order with respect to reactant |
Reaction constant unit | Molarity per time (M/s) | Inverse time (s-1) | M-1 s-1 |
Example | Enzyme-catalyzed reactions | Radioactive decay | Dimerization of molecules |
Experimental data | Concentration changes linearly over time | Concentration changes exponentially over time | Concentration changes quadratically over time |
Reaction | Rate is constant | Unimolecular Process | Bimolecular Process |
Zero Order Reaction
Zero Order Reaction is a type of chemical reaction where the reaction rate does not change with variations in the concentration of the reactants. In such reactions, the concentration rates remain constant over time. This type of reaction is characterized by the fact that the concentration of the reactants does not influence the reaction rate.
In this article, we look into What the order of the reaction is, what the zero-order reaction is, definition characteristics, rate law expression, etc.
Table of Content
- What is Order of Reaction?
- What is a Zero Order Reaction?
- Characteristics of Zero Order Reactions
- Rate Law for Zero Order Reactions
- Half-Life Time (t1/2) for Zero Order Reaction
- Zero, First and Second-Order Reactions
- Significance of Zero Order Reactions
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