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Questions and Answers
What is the integrated rate law expression for a second-order reaction?
What is the integrated rate law expression for a second-order reaction?
What does the half-life of a zero-order reaction depend on?
What does the half-life of a zero-order reaction depend on?
In the context of the Arrhenius equation, what does the symbol $E_a$ represent?
In the context of the Arrhenius equation, what does the symbol $E_a$ represent?
Which of the following equations represents the half-life for a first-order reaction?
Which of the following equations represents the half-life for a first-order reaction?
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What is the form of the rate equation for a zero-order reaction?
What is the form of the rate equation for a zero-order reaction?
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For a first-order reaction, how does the natural logarithm of the concentration change over time?
For a first-order reaction, how does the natural logarithm of the concentration change over time?
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What occurs to the rate constant $k$ as the temperature increases, based on the Arrhenius equation?
What occurs to the rate constant $k$ as the temperature increases, based on the Arrhenius equation?
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Which of the following expressions correctly represents the half-life of a zero-order reaction?
Which of the following expressions correctly represents the half-life of a zero-order reaction?
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In a second-order reaction, how does the concentration relate to time according to the integrated rate law?
In a second-order reaction, how does the concentration relate to time according to the integrated rate law?
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How does the activation energy $E_a$ affect the rate constant $k$ according to the linear Arrhenius form?
How does the activation energy $E_a$ affect the rate constant $k$ according to the linear Arrhenius form?
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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.