Review the formula for determination of entropy change, write the formula and discuss. Present a problem which involves determination of the change in entropy when nitrous oxide reacts with oxygen to form nitrogen dioxide. List and discuss each step in the process and then analyze the answer.

Discuss the increase in entropy as it relates to the number of microstates and particles. Review Boltzmann law. Summarize the spontaneous reactions which occur. Discuss movement of gas particles between connected flasks and why the entropy of the system increases. Introduce the 3rd law of thermodynamics and " a perfect crystal". Discuss measurement or entropy.

View and discuss Bozmann entropy equation. View from YouTube how to determine the number of microstates present, Bozmann's constant and the use of the natural log. Determine the entropy for a gas, as liquid and a solid at the same temperature. Note that the entropy for the gas is greater than for the liquid, and that the solid is zero. Summarize the entropy process.

Discuss the dispersion of entropy. Elicit how and way thermal energy is distributed from matter . Discuss why the distribution/dispersion of the energy occurs depending on th number of atoms present in th system. Statistically , large numbers of particles increases the accuracy of the dispersion. Discuss micro-states. Introduce Boltzman's formula which will quantify entropy based on a constant, the number of micro states in the system, and the natural log of the number of microstates.

Discuss the second law of thermodynamics, which is a process that results in an increase of entropy. Discuss heat as the random motion of particles and that potential energy is dispersed when converted to thermal. Use q to represent heat, T to represent temperature in Kelvin and delta S to represent the change in entropy. Define the formula S + q/T in joules/kelvinb.

Review some common exothemic reactions and note have a negative heat of reaction and are spontaneous reactions . Present a few endothermic reactions, specifically the melting of ice which has a positive heat of reaction. Demonstrate and discuss the direction of heat flow in that system. Elicit that the flow transfers heat energy from hot to cold. Determine the energy is transferred from the surroundings to the system. State that the evolution of heat energy is not sufficient to determine spontaneity. Discuss the first law of thermodynamics and how energy transferred as heat proceeds from higher concentration to a more dispersed system. Quantify this function of dispersed heat energy as entropy by being able to give it a number.

Define and discuss spontaneous reactions, which occur without outside interference. Determine that they occur only in the direction that leads to equilibrium . Show examples of spontaneous reactions and elicits that they are all exothermic . Change in heat energy is negative. List and discuss. Few reactions occur spontaneously, but possess a positive heat of reaction. Use melting of ice when left in a beaker sitting on a table top. Elicit what occurs when a beaker of cold water is left sitting out. Define which way the heat energy moves. Discuss the energy transfer as heat is from hot to cold, from surrounding to system.

Describe how enthalpy changes accompany chemical reactions. Discuss the standard enthalpy change delta H. Define and explain delta rH and the subscript r. Define standard state as the most stable form in the system. Explain "per mole-rxn" Show examples of heat of formation reaction and note the change due to coefficients in the written equation. State general features for the heat of reaction, both exothermic and endothermic. Work on two examples designed to show how to calculate the energy of the reaction using an endothermic and an exothermic reaction

To determine the expansion of a gas under constant atmospheric pressure when a specific amount of energy is transferred as. heat from the surroundings. The calculation of work done is found by utilizing w=-P ( delta V). Once the work is calculated, the change in internal energy is calculated from delta U = q + w.

Review the formula changes in energy content equals energy transferred as heat plus energy transferred as work. U = q+ w. Discuss how the energy of the universe is constant, conserved and must be accounted for. Elicit that U = internal energy, which is the sum of potential and kinetic energy. Work is determined by the formula W= -P + delta V, were V is the volume of a gas and P is the pressure. Work is in Joules, pressure in Pascals, and volume change om M^3. Start solving problem on page 269, check your understanding.