What is the half-life equation for first-order?

The half-life of a first-order reaction is a constant that is related to the rate constant for the reaction: t1/2 = 0.693/k. Radioactive decay reactions are first-order reactions. The rate of decay, or activity, of a sample of a radioactive substance is the decrease in the number of radioactive nuclei per unit time.

What is the half-life in seconds of a zero order reaction?

Answers. The half-life is 96 seconds. Since this is a zero-order reaction, the half-life is dependent on the concentration. In this instance, the half-life is decreased when the original concentration is reduced to 1.0 M.

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

The half-life of a zero-order reaction increases as the initial concentration increases.

What is the formula of zero order reaction?

Solution: For zero order reaction, the rate of the reaction is equal to the rate constant or rate of reaction = k.

How does half-life of zero order reaction related to its rate constant?

For a zero order reaction (Half life decreases with decreasing concentration.) For a 1st order reaction (Half life is constant.) For a second order reaction (Half life increases with decreasing concentration.)

What is zero and first order reaction?

A zero-order reaction proceeds at a constant rate. A first-order reaction rate depends on the concentration of one of the reactants. A second-order reaction rate is proportional to the square of the concentration of a reactant or the product of the concentration of two reactants.

How do half-lives of the first order reaction and zero order reaction change with initial concentration of reactants?

The half-life of a zero-order reaction increases as the initial concentration increases. Equations for both differential and integrated rate laws and the corresponding half-lives for zero-, first-, and second-order reactions are summarized in Table 22.