Integrated Rate Equations

Chemistry ⇒ Chemical Kinetics and Equilibrium

Integrated Rate Equations starts at 11 and continues till grade 12. QuestionsToday has an evolving set of questions to continuously challenge students so that their knowledge grows in Integrated Rate Equations. How you perform is determined by your score and the time you take. When you play a quiz, your answers are evaluated in concept instead of actual words and definitions used.

See sample questions for grade 11

A first-order reaction has a half-life of 10 minutes. How long will it take for the reactant to be reduced to 12.5% of its original concentration?

A reaction follows the rate law: rate = k[A]². If the initial concentration of A is doubled, how does the half-life change?

A reaction has a rate constant of 0.1 L mol^-1 s^-1. What is the order of the reaction?

A reaction has the integrated rate law: [A] = [A]₀ - kt. If [A] becomes zero after 40 minutes and [A]₀ = 0.8 mol/L, what is the value of k?

A reaction is first order in A. If the concentration of A decreases from 0.8 mol/L to 0.2 mol/L in 40 minutes, what is the rate constant?

A reaction is found to have a constant half-life regardless of the initial concentration. What is the order of the reaction?

Describe how you would determine the order of a reaction using integrated rate equations and experimental data.

Explain the significance of the slope in a plot of ln[A] versus time for a first-order reaction.

Explain why the half-life of a first-order reaction does not depend on the initial concentration.

For a first-order reaction, the rate constant is 2.0 × 10^-3 s^-1. What is the half-life?

For a reaction: 2A → Products, the rate law is rate = k[A]². If [A]₀ = 0.2 mol/L and k = 0.5 L mol^-1 min^-1, calculate the half-life.

For a reaction: A → Products, the concentration of A decreases from 0.4 mol/L to 0.1 mol/L in 30 minutes. If the reaction is first order, calculate the rate constant.

If a plot of 1/[A] versus time is a straight line, what is the order of the reaction?

If the initial concentration of a reactant is 0.5 mol/L and after 20 minutes it becomes 0.25 mol/L in a first-order reaction, calculate the rate constant.

State the integrated rate law for a zero-order reaction.

The integrated rate law for a first-order reaction is ln([A]₀/[A]) = kt. If [A]₀ = 1.0 mol/L, [A] = 0.5 mol/L, and t = 10 min, what is the value of k?

The integrated rate law for a reaction is ln([A]₀/[A]) = kt. What is the order of the reaction?

The integrated rate law for a zero-order reaction is [A] = [A]₀ - kt. If [A]₀ = 0.8 mol/L and k = 0.02 mol L^-1 min^-1, how long will it take for [A] to reach 0.2 mol/L?

The integrated rate law for a zero-order reaction is [A] = [A]₀ - kt. If [A]₀ = 1.0 mol/L and k = 0.1 mol L^-1 min^-1, what will be the concentration after 5 minutes?

The rate constant for a first-order reaction is 0.693 min^-1. What is the half-life of the reaction?