 # Half-Life of a Chemical Reaction

## What is Reaction Half-Life?

The half-life of a chemical reaction can be defined as the time taken for the concentration of a given reactant to reach 50% of its initial concentration (i.e. the time taken for the reactant concentration to reach half of its initial value). It is denoted by the symbol ‘t1/2’ and is usually expressed in seconds.

## Half-Life Formula

It is important to note that the formula for the half-life of a reaction varies with the order of the reaction.

• For a zero-order reaction, the mathematical expression that can be employed to determine the half-life is: t1/2 = [R]0/2k
• For a first-order reaction, the half-life is given by: t1/2 = 0.693/k
• For a second-order reaction, the formula for the half-life of the reaction is: 1/k[R]0

Where,

• t1/2 is the half-life of the reaction (unit: seconds)
• [R0] is the initial reactant concentration (unit: mol.L-1 or M)
• k is the rate constant of the reaction (unit: M(1-n)s-1 where ‘n’ is the reaction order)

## Derivation of Half-Life Formula for Zero-Order Reactions

For a zero-order reaction, the units of the rate constant are mol.L-1.s-1. The expression for a zero-order rate constant is:

$$\begin{array}{l}k = \frac{[R]_{0}-[R]}{t}\end{array}$$

Substituting t = t1/2, at which point [R] = [R]0/2 (at the half-life of a reaction, reactant concentration is half of the initial concentration).

$$\begin{array}{l}k = \frac{[R]_{0}-[R]_{0}/2}{t_{1/2}}\end{array}$$

Rearranging the equation, the expression for the half-life of a zero-order reaction is found to be:

$$\begin{array}{l}t_{1/2} = \frac{[R]_{0}}{2k}\end{array}$$

## Derivation of Half-Life Formula for First-Order Reactions

For a first-order reaction, the rate constant can be mathematically expressed as follows:

$$\begin{array}{l}k = \frac{2.303}{t}log\frac{[R]_0}{[R]}\end{array}$$

From the definition of reaction half-life, at t = t1/2, [R] = [R]0/2. Substituting these values in the expression for the first-order rate constant, the following equation is obtained:

$$\begin{array}{l}k = \frac{2.303}{t_{1/2}}log\frac{[R_0]}{[R]_0/2}\end{array}$$

Rearranging the expression to find the value of t1/2:

$$\begin{array}{l}t_{1/2} = \frac{2.303}{k}log(2) = \frac{0.693}{k}\end{array}$$

Thus, the half-life of a first-order reaction is given by 0.693/k.

## Zero Order Reactions 