How is the half-life of a first order reaction affected by the initial reactant concentration?

The half-life of a reaction is the time required for a reactant to reach one-half its initial concentration or pressure. For a first-order reaction, the half-life is independent of concentration and constant over time.

Does the half-life of a first order reaction depend on the initial concentration of the reactant?

The decomposition of hydrogen peroxide is a first-order reaction, and, as can be shown, the half-life of a first-order reaction is independent of the concentration of the reactant. However, half-lives of reactions with other orders depend on the concentrations of the reactants.

What happens to half-life period of a first order reaction if initial concentration of the reactant is doubled?

In the question, the time for half reaction is doubled when initial concentration is doubled it is zero order reaction.

How does half-life change with concentration?

Therefore, for a zero-order reaction, half-life and initial concentration are directly proportional. As initial concentration increases, the half-life for the reaction gets longer and longer.

What affects the half-life of a reaction?

The half-life of a first order reaction is independent of its initial concentration and depends solely on the reaction rate constant, k. As you can see, the half-life of the second order reactions depends on the initial concentration and rate constant.

How is the half-life of a second order reaction affected by the initial reactant concentration?

For a second-order reaction, the half-life is inversely related to the initial concentration of the reactant (A). For a second-order reaction each half-life is twice as long as the life span of the one before.

What is the half-life of first order reaction if time is required to reduce concentration?

Concentration is reduced to 25\%. It means it takes two half-lives to decrease the concentration of reactant from 0.8 M to 0.2 M in first-order reaction. Hence, half-life of the reaction is 12/2 = 6 hours.

Why is the half-life of a first order reaction independent of concentration?

The best way to determine rate constant k in half-life of first order is to determine half-life by experimental data. The reason is half-life in first order order doesn’t depend on initial concentration. In a first order reaction, A⟶B.

Why is half-life of first order reaction is independent of concentration of the reactant?

The expression for the half-life period of a first order reaction does not contain a concentration term. Thus, the half-life period for such reactions is independent of the initial concentration of the reactants.

When initial concentration of reactant is doubled in reaction the half-life period is not affected the order of reaction is?

In a zero order reaction, if the concentration of the reactant is doubled, the half-life period is also doubled.

Does the half-life of a second order reaction increase/decrease or remain the same as the reaction proceeds How does the half-life vary as the reaction proceeds?

The quantity [A]_0 decreases in concentration over the course of the reaction. As a result, since \large{t_{1/2} = \frac {1}{k[A]_0}} in a second-order reaction, the half-life of a second-order reaction gets longer as the reaction proceeds. as the reaction proceeds.