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Summary Energy, enthalpy and thermochemistry

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Summary of 9th chapter from Chemical Principles: Zumdahl and Decoste. Notes containing key concepts from the chapter and thorough explanations of the terminology. Also includes formulas and relevant course-related information.

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  • Chapter 9
  • July 19, 2019
  • 3
  • 2018/2019
  • Summary

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Energy, Enthalpy and
Thermochemistry
9.1 The nature of energy

 Energy is the capacity to do work or produce heat.
 Conservation of energy: Energy cannot be created nor destroyed but only
transferred and transformed.
 Energy can be classified as Kinetic energy or Potential energy
 Temperature is a property that reflects the random motions of the particles in a
particular substance. Heat involves transfer energy between two objects due to
temperature difference.
 Work is defined as a force acting over a distance.
 State function states that the change in its property in going from one state into
another is independent of the particular pathway taken between the two states.
 The system is the part of the universe which we study, and the surrounding is
everything else independent from the system.
 When a reaction results in the evolution of heat, it is said to be exothermic.
 Reactions that absorb energy from the surroundings are called endothermic.
 The energy gained by the surroundings equals the energy lost from the system.
 In exothermic process, the bonds of the products are stronger than the bonds of the
reactants.
 The study of energy and its conversions is known as thermodynamics
 The law of conservation or the first law of thermodynamics:
- ∆E = q + w
- Q represents heat and W represents the work.
- ∆E is the change in the systems internal energy.
 Thermodynamics quantitates include a magnitude (number) and a direction (sign).
Positive sign indicate that the system gains energy and Negative sign indicates that it
loses energy to the surroundings.
 W = - P ∆V
- P is pressure
- ∆V is change in volume

9.2 Enthalpy

 Enthalpy
- H = E + PV
- E is the internal energy of the system; P is the pressure and V is the volume.
 qp = ∆E + P∆V
- qp is heat at constant pressure.
 For a process carried out at constant pressure, where the only work allowed is that
from a volume change, ∆H = qp

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