The half-life is inversely proportional to the concentration in first-order kinetics.

Here's a step-by-step explanation:

1. In chemical kinetics, the order of a reaction is determined by the power dependence of the rate on the concentration of each reactant.

2. For a first-order reaction, the rate of the reaction is directly proportional to the concentration of one reactant. This can be represented as: Rate = k[A], where k is the rate constant and [A] is the concentration of the reactant.

3. The half-life of a reaction (t1/2), which is the time it takes for half of the reactant to be consumed, is a constant for first-order reactions. It is independent of the initial concentration of the reactant.

4. However, if we look at the equation for the half-life of a first-order reaction, t1/2 = 0.693/k, we can see that the half-life is inversely proportional to the rate constant k.

5. Since the rate constant k is directly proportional to the concentration of the reactant for a first-order reaction, we can therefore say that the half-life is inversely proportional to the concentration in first-order kinetics.

Question

The half-life is inversely proportional to the concentration in first-order kinetics.

Here's a step-by-step explanation:

1. In chemical kinetics, the order of a reaction is determined by the power dependence of the rate on the concentration of each reactant.

2. For a first-order reaction, the rate of the reaction is directly proportional to the concentration of one reactant. This can be represented as: Rate = k[A], where k is the rate constant and [A] is the concentration of the reactant.

3. The half-life of a reaction (t1/2), which is the time it takes for half of the reactant to be consumed, is a constant for first-order reactions. It is independent of the initial concentration of the reactant.

4. However, if we look at the equation for the half-life of a first-order reaction, t1/2 = 0.693/k, we can see that the half-life is inversely proportional to the rate constant k.

5. Since the rate constant k is directly proportional to the concentration of the reactant for a first-order reaction, we can therefore say that the half-life is inversely proportional to the concentration in first-order kinetics.

Knowee AI · Accepted Answer

The half-life is inversely proportional to the concentration in first-order kinetics.

Here's a step-by-step explanation:

1. In chemical kinetics, the order of a reaction is determined by the power dependence of the rate on the concentration of each reactant.

2. For a first-order reaction, the rate of the reaction is directly proportional to the concentration of one reactant. This can be represented as: Rate = k[A], where k is the rate constant and [A] is the concentration of the reactant.

3. The half-life of a reaction (t1/2), which is the time it takes for half of the reactant to be consumed, is a constant for first-order reactions. It is independent of the initial concentration of the reactant.

4. However, if we look at the equation for the half-life of a first-order reaction, t1/2 = 0.693/k, we can see that the half-life is inversely proportional to the rate constant k.

5. Since the rate constant k is directly proportional to the concentration of the reactant for a first-order reaction, we can therefore say that the half-life is inversely proportional to the concentration in first-order kinetics.

Half life is inversely proportional to concentration in which order kinetics

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