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`t_(1/2) = ([A]_0)/(2k)`

Enter a value for all fields

The **Half-Life of Zero Order Reaction** calculator computes the half-life in nuclear decay for a zero order reaction.

**INSTRUCTIONS**: Enter the following:

- (
**k**) This is the temperature-dependent reaction rate constant. - (
**A**) This is the initial concentration_{0}

**Half-Life**: The calculator returns the half-life.

- Zero Order
**Rate Law (Integral form)** - Zero Order
**Half Life** - Zero Order
**Rate Law** - First Order
**Rate Law (Integral form)** - First Order
**Half Life** - First Order
**Rate Law** - Second Order
**Rate Law (Integral form)** - Second Order
**Half Life** - Second Order
**Rate Law**

The half-life of a chemical reaction is defined as the time required for half the amount of a reactant to be converted into product. To find the half-lives of different order reactions, we use integrated rate laws and rate constants to relate concentration to time. There are three different rate laws that can be used to find the half-life of a chemical reaction: zero, first, and second order.

For zero order kinetics, the half-life is not dependent on the concentration of the substance. In other words, **rate = k**. This means that no matter how much substrate is added, and no matter how high of a concentration is present in solution, the rate of the reaction will not increase. A graphical representation of this would show linear data with a negative slope, as shown in the image below. The** rate law** for a zero order reaction is **[A] = [A] _{0} - kt**. To find the

Where

- k is the temperature-dependent reaction rate constant
- t
_{1/2}is the half-life - [A]
_{0}is the initial concentration

Whitten, et al. "Chemistry" 10th Edition. Pp. 631