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Solutions for Chapter 7.4a: ENERGY BALANCES ON OPEN SYSTEMS AT STEADY STATE

Elementary Principles of Chemical Processes | 4th Edition | ISBN: 9780470616291 | Authors: Richard M. Felder Ronald W. Rousseau, Lisa G. Bullard

Full solutions for Elementary Principles of Chemical Processes | 4th Edition

ISBN: 9780470616291

Elementary Principles of Chemical Processes | 4th Edition | ISBN: 9780470616291 | Authors: Richard M. Felder Ronald W. Rousseau, Lisa G. Bullard

Solutions for Chapter 7.4a: ENERGY BALANCES ON OPEN SYSTEMS AT STEADY STATE

Solutions for Chapter 7.4a
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Since 2 problems in chapter 7.4a: ENERGY BALANCES ON OPEN SYSTEMS AT STEADY STATE have been answered, more than 8752 students have viewed full step-by-step solutions from this chapter. Elementary Principles of Chemical Processes was written by Patricia and is associated to the ISBN: 9780470616291. This textbook survival guide was created for the textbook: Elementary Principles of Chemical Processes, edition: 4. This expansive textbook survival guide covers the following chapters and their solutions. Chapter 7.4a: ENERGY BALANCES ON OPEN SYSTEMS AT STEADY STATE includes 2 full step-by-step solutions.

Key Chemistry Terms and definitions covered in this textbook
  • alcohol

    A compound that possesses a hydroxyl group (OH).

  • alkyl halide

    An organic compound containing at least one halogen.

  • beta particles.

    See beta rays.

  • delocalized molecular orbitals.

    Molecular orbitals that are not confined between two adjacent bonding atoms but actually extend over three or more atoms. (10.8)

  • diastereotopic

    Nonequivalent protons for which the replacement test produces diastereomers.

  • Energy

    The ability to do work.

  • frequency

    The number of times per second that one complete wavelength passes a given point. (Section 6.1)

  • gauche conformation

    A conformation that exhibits a gauche interaction.

  • Gibbs free energy change (DG°)

    The energy that dictates the position of chemical equilibria and rates of chemical reactions. A thermodynamic function of enthalpy, entropy, and temperature, given by the equation DG° 5 DH° 2 TDS°. If DG° , 0, the position of equilibria for the reaction favors products. If DG° . 0, the position of equilibria favors reactants.

  • Homotopic groups

    Atoms or groups on an atom that give an achiral molecule when one of the groups is replaced by another group. The hydrogens of the CH2 group of propane, for example, are homotopic. Replacing either one of them with deuterium gives 2-deuteropropane, which is achiral. Homotopic groups have identical chemical shifts under all conditions

  • IUPAC

    The International Union of Pure and Applied Chemistry

  • Mass spectrum

    A plot of the relative abundance of ions versus their mass-to-charge ratio

  • miscible liquids

    Liquids that mix in all proportions. (Section 13.3)

  • partially condensed structures

    A drawing style in which the CH bonds are not drawn explicitly, but all other bonds are drawn.

  • polar covalent bond

    A covalent bond in which the electrons are not shared equally. (Section 8.4)

  • polysaccharides

    Polymers made up of repeating monosaccharide units linked together by glycoside bonds.

  • quaternary structure

    The structure that arises when a protein consists of two or more folded polypeptide chains that aggregate to form one protein complex.

  • sodium cyanoborohydride

    A selective reducing agent (NaBH3CN) that can be used for reductive amination.

  • Solvolysis

    A nucleophilic substitution in which the solvent is also the nucleophile

  • vicinal

    A term used to describe two identical groups attached to adjacent carbon atoms.

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