Solutions for Chapter 15: Chemical Kinetics

Chemical Principles | 8th Edition | ISBN: 9781305581982 | Authors: Steven S. Zumdahl

Full solutions for Chemical Principles | 8th Edition

ISBN: 9781305581982

Chemical Principles | 8th Edition | ISBN: 9781305581982 | Authors: Steven S. Zumdahl

Solutions for Chapter 15: Chemical Kinetics

Solutions for Chapter 15
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Textbook: Chemical Principles
Edition: 8
Author: Steven S. Zumdahl
ISBN: 9781305581982

This textbook survival guide was created for the textbook: Chemical Principles, edition: 8. Since 135 problems in chapter 15: Chemical Kinetics have been answered, more than 22869 students have viewed full step-by-step solutions from this chapter. Chapter 15: Chemical Kinetics includes 135 full step-by-step solutions. This expansive textbook survival guide covers the following chapters and their solutions. Chemical Principles was written by Sieva Kozinsky and is associated to the ISBN: 9781305581982.

Key Chemistry Terms and definitions covered in this textbook
  • activation energy (Ea).

    The minimum amount of energy required to initiate a chemical reaction. (13.4)

  • anode.

    The electrode at which oxidation occurs. (18.2)

  • antiaromatic

    Instability that arises when a planar ring of continuously overlapping p orbitals contains 4n p electrons.

  • bonding molecular orbital.

    A molecular orbital that is of lower energy and greater stability than the atomic orbitals from which it was formed. (10.6)

  • Chromatography

    A separation method involving passing a vapor or solution mixture through a column packed with a material with different affi nities for different components of the mixture.

  • critical mass.

    The minimum mass of fissionable material required to generate a self-sustaining nuclear chain reaction. (19.5)

  • Excited state

    A state of a system at higher energy than the ground state.

  • fats

    Triglycerides that are solids atroom temperature.

  • Hemiacetal

    A molecule containing an !OH and an !OR or !OAr group bonded to the same carbon

  • Hund’s rule

    When considering electrons in atomic orbitals, a rule that states that one electron is placed in each degenerate orbital first, before electrons are paired up.

  • hydroboration-oxidation

    A twostep process that achieves an anti-Markovnikov addition of a proton and a hydroxyl group (OH) across an alkene.

  • Kinetic control

    Experimental conditions under which the composition of the product mixture is determined by the relative rates of formation of each product.

  • Living polymer

    A polymer chain that continues to grow without chain-termination steps until either all of the monomer is consumed or some external agent is added to terminate the chain. The polymer chains will continue to grow if more monomer is added.

  • molecular equation

    A chemical equation in which the formula for each substance is written without regard for whether it is an electrolyte or a nonelectrolyte. (Section 4.2)

  • molecular-orbital theory

    A theory that accounts for the allowed states for electrons in molecules.(Section 9.7)

  • Nucleic acid

    A biopolymer containing three types of monomer units: heterocyclic aromatic amine bases derived from purine and pyrimidine, the monosaccharides d-ribose or 2-deoxy-d-ribose, and phosphoric acid

  • photodissociation

    The breaking of a molecule into two or more neutral fragments as a result of absorption of light. (Section 18.2)

  • S (Section 3.3

    From the Latin, sinister, left; used in the R,S convention to show that the order of priority of groups on a chiral center is counterclockwise

  • tertiary

    A term used to indicate that exactly three alkyl groups are attached directly to a particular position. For example, a tertiary carbocation has three alkyl groups attached directly to the electrophilic carbon atom (C+).

  • Upfield

    A signal of an NMR spectrum that is shifted toward the right (smaller chemical shift) on the chart paper.

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