Chemistry Reaction Rates and Laws
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Questions and Answers

What is the integrated rate law expression for a second-order reaction?

  • [A] = [A]_0 - kt
  • ln[A] = ln[A]_0 - kt
  • t_{1/2} = k[A]_0
  • 1/[A] = 1/[A]_0 + kt (correct)
  • What does the half-life of a zero-order reaction depend on?

  • The temperature alone.
  • The activation energy.
  • Only the rate constant.
  • The initial concentration and the rate constant. (correct)
  • In the context of the Arrhenius equation, what does the symbol $E_a$ represent?

  • The equilibrium constant.
  • The universal gas constant.
  • The activation energy. (correct)
  • The rate constant.
  • Which of the following equations represents the half-life for a first-order reaction?

    <p>t_{1/2} = rac{0.693}{k}</p> Signup and view all the answers

    What is the form of the rate equation for a zero-order reaction?

    <p>Rate = k</p> Signup and view all the answers

    For a first-order reaction, how does the natural logarithm of the concentration change over time?

    <p>$ln[A] = ln[A]_0 - kt$</p> Signup and view all the answers

    What occurs to the rate constant $k$ as the temperature increases, based on the Arrhenius equation?

    <p>It increases exponentially.</p> Signup and view all the answers

    Which of the following expressions correctly represents the half-life of a zero-order reaction?

    <p>$t_{1/2} = rac{[A]_0}{2k}$</p> Signup and view all the answers

    In a second-order reaction, how does the concentration relate to time according to the integrated rate law?

    <p>$ rac{1}{[A]} = kt + rac{1}{[A]_0}$</p> Signup and view all the answers

    How does the activation energy $E_a$ affect the rate constant $k$ according to the linear Arrhenius form?

    <p>Higher $E_a$ decreases $k$ at any temperature.</p> Signup and view all the answers

    Study Notes

    Reaction Rates and Integrated Rate Laws

    • Reaction Rate: The rate of a reaction is expressed as the change in concentration of a reactant or product per unit time. The equation is: d[A]/dt = k[A]^m[B]^n, where k is the rate constant, [A] and [B] are reactant concentrations, and m and n are the reaction orders (typically integers).

    Zero-Order Reaction

    • Integrated Rate Law: [A] = [A]0 - kt (where [A]0 is the initial concentration of A)
    • Half-life: t1/2 = [A]0 / 2k

    First-Order Reaction

    • Integrated Rate Law: ln[A] = ln[A]0 - kt
    • Half-life: t1/2 = 0.693 / k

    Second-Order Reaction

    • Integrated Rate Law: 1/[A] = 1/[A]0 + kt
    • Half-life: t1/2 = 1 / k[A]0

    Arrhenius Equation

    • Equation: k = Ae-Ea/RT
    • describes the temperature dependence of the rate constant, k, where:
    • A = pre-exponential factor
    • Ea = activation energy
    • R = ideal gas constant
    • T = absolute temperature

    Linear Arrhenius Form

    • Equation: ln k = -Ea/RT + ln A
    • This form of the Arrhenius equation allows for determination of activation energy by plotting ln k vs 1/T.

    Integrated Rate Laws (Summary)

    • Zero-Order: [A] = [A]0 - kt
    • First-Order: ln[A] = ln[A]0 - kt
    • Second-Order: 1/[A] = 1/[A]0 + kt

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    Description

    This quiz covers the concepts of reaction rates and integrated rate laws, focusing on zero, first, and second-order reactions. It includes the Arrhenius equation and discusses the mathematical relationships governing these reactions, helping students understand how to calculate reaction rates and half-lives effectively.

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