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Questions and Answers

What is the average rate of appearance of B?

  • delta [A] / delta A
  • delta [B] / delta t (correct)
  • Rate = k[A]
  • Rate = k[A]^m[B]^n

What is the Rate Law formula?

Rate = k[A]^m[B]^n

What is the first order reaction differential rate law?

Rate = k[A]

What is the integrated rate law for a first order reaction?

<p>ln[A] sub t = -kT + ln[A] sub 0</p> Signup and view all the answers

What is the formula for the half-life of a first order reaction?

<p>t sub 1/2 = 0.639/k</p> Signup and view all the answers

What is the second order reaction differential rate law?

<p>Rate = k[A]^2</p> Signup and view all the answers

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

<p>1/[A] sub t = kT + 1/[A] sub 0</p> Signup and view all the answers

What is the half-life formula for a second order reaction?

<p>t1/2 = 1 / k[A] sub 0</p> Signup and view all the answers

What is the formula for the fraction of molecules with energy greater than or equal to Ea?

<p>f = e^(-Ea/RT)</p> Signup and view all the answers

What is the Arrhenius equation?

<p>K = Ae^(-Ea/RT)</p> Signup and view all the answers

How can you determine Ea using the rate constant?

<p>lnK = -Ea/RT + lnA</p> Signup and view all the answers

What does the slope represent in the context of lnK vs. 1/T?

<p>-Ea/R</p> Signup and view all the answers

What is the formula when given two temperatures to determine the change in rate constants?

<p>ln(k2/k) = (Ea/R)(1/T1 - 1/T2)</p> Signup and view all the answers

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Study Notes

Chemical Kinetics Key Concepts

  • Average Rate of Appearance: Measures the change in concentration of a reactant or product over time, calculated as delta [B] / delta t.
  • Rate Law: Describes the relationship between the rate of a reaction and the concentration of its reactants; expressed as Rate = k[A]^m[B]^n, where k is the rate constant and m, n are the reaction orders.
  • First Order Reaction Differential Rate Law: For a reaction with first-order kinetics, the rate is proportional to the concentration of one reactant: Rate = k[A].

First Order Reaction Properties

  • Integrated Rate Law: The concentration of a reactant over time can be related using the equation ln[A] sub t = -kT + ln[A] sub 0, demonstrating the logarithmic decrease in concentration.
  • Half-Life: The time required for half of the reactant to be consumed in a first-order reaction is given by t sub 1/2 = 0.639/k, indicating that half-life is independent of the initial concentration.

Second Order Reaction Properties

  • Second Order Reaction Differential Rate Law: For a reaction with second-order kinetics, the rate is proportional to the square of the concentration of one reactant: Rate = k[A]^2.
  • Integrated Rate Law: The concentration for a second-order reaction over time can be determined by the equation 1/[A] sub t = kT + 1/[A] sub 0, revealing a linear relationship.
  • Second-Order Half-Life: The half-life for a second-order reaction is calculated as t1/2 = 1 / k[A] sub 0, showing dependency on the initial concentration.

Energy and Activation Relations

  • Fraction of Molecules with Energy ≥ Ea: Describes a fraction of molecules that possess energy greater than or equal to the activation energy: f = e^(-Ea/RT).
  • Arrhenius Equation: Connects the rate constant (k) to temperature and activation energy, defined as K = A e^(-Ea/RT), where A is the pre-exponential factor.
  • Calculating Activation Energy (Ea): By rearranging the Arrhenius equation, activation energy can be found from lnK = -Ea/RT + lnA, showcasing its relationship with the rate constant and temperature.

Slope and Temperature Relations

  • Slope in Arrhenius Plot: The slope of the linear plot of ln(k) versus 1/T is represented as -Ea/R, where R is the universal gas constant.
  • Change in Rate Constant with Temperature: To analyze the effect of two temperatures on the rate constant, use the equation ln(k2/k) = (Ea/R)(1/T1 - 1/T2), indicating how the rate constant varies with temperature changes.

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