Question

For each of the scenarios, identify the order with respect to the reactant, A. A⟶products The half‑life of A increases as the initial concentration of A decreases. order: A three‑fold increase in the initial concentration of A leads to a nine‑fold increase in the initial rate. order: A three‑fold increase in the initial concentration of A leads to a 1.73‑fold increase in the initial rate. order: The time required for [A] to decrease from [A]0 to [A]0/2 is equal to the time required for [A] to decrease from [A]0/2 to [A]0/4. order: The rate of decrease of [A] is a constant. order:

Answer 1

Answer:

Answers are in the explanation.

Explanation:

• The half‑life of A increases as the initial concentration of A decreases. order: 2. In the half-life of second-order reactions, the half-life is inversely proportional to initial concentration.
• A three‑fold increase in the initial concentration of A leads to a nine‑fold increase in the initial rate. order: 2. The rate law of second-order is: rate = k[A]²
• A three‑fold increase in the initial concentration of A leads to a 1.73‑fold increase in the initial rate. order: 1/2. The rate law for this reaction is: rate = k √[A]
• The time required for [A] to decrease from [A]₀ to [A]₀/2 is equal to the time required for [A] to decrease from [A]₀/2 to [A]₀/4. order: 1. The concentration-time equation for first-order reaction is: ln[A] = ln[A]₀ - kt. That means the [A] decreasing logarithmically.
• The rate of decrease of [A] is a constant. order: 0. The rate law is: rate = k -where k is a constant-

Answer 2

The order of the reaction can be defined as the rate of depletion of the products and the reactants with respect to time.

The order of reaction for the following can be given by:

• The half‑life of A increases as the initial concentration of A decreases.

The order of reaction has been second order. The half-life has been inversely proportional to the initial concentration of the reactants.

• A three‑fold increase in the initial concentration of A leads to a nine‑fold increase in the initial rate.

The order of the reaction has been second order. The increase in the half-life has been directly proportional to the initial concentration with the rate being k[$\rm A^2$].

• A three‑fold increase in the initial concentration of A leads to a 1.73‑fold increase in the initial rate.

The order of the reaction has been the half-order reaction. The rate of the reaction in the half order reaction can be given by k$\rm \sqrt{A}$.

• The time required for [A] to decrease from [A]0 to [A]0/2 is equal to the time required for [A] to decrease from [A]0/2 to [A]0/4.

The order of the reaction has been the first-order reaction. The half-life of the first-order reaction has been directly proportional to the initial concentration.

• The rate of decrease of [A] is a constant.

The order of the reaction has been zero order. The rate of the reaction has been independent of the initial concentration in the zero-order reaction.

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