The first law of thermodynamics is concerned with the conservation of

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By the end of this section, you will be able to do the following: • Describe how pressure, volume, and temperature relate to one another and to work, based on the ideal gas law • Describe pressure–volume work • Describe the first law of thermodynamics verbally and mathematically • Solve problems involving the first law of thermodynamics Teacher Support The learning objectives in this section will help your students master the following standards: • (6) Science concepts. The student knows that changes occur within a physical system and applies the laws of conservation of energy and momentum. The student is expected to: • (G) analyze and explain everyday examples that illustrate the laws of thermodynamics, including the law of conservation of energy and the law of entropy. Section Key Terms Teacher Support [BL] [OL] [AL] Review the concept of force. [OL] Ask students how much force it would take to hammer a nail into a wall. Would they achieve the same result if the nail were blunt instead of pointed? Why or why not? Before covering the first law of thermodynamics, it is first important to understand the relationship between pressure, volume, and temperature. Pressure, P, is defined as Figure 12.3 (a) Although the person being poked with the finger might be irritated, the force has little lasting effect. (b) In contrast, the same force applied to an area the size of the sharp end of a needle is great enough to break the skin. The SI unit for pressure is the pascal, where 1Pa...

First Law of Thermodynamics First Law of Thermodynamics The first law of thermodynamics is the application of the The first law makes use of the key concepts of It is typical for chemistry texts to write the first law as ΔU=Q+W. It is the same law, of course - the thermodynamic expression of the conservation of energy principle. It is just that W is defined as the work done on the system instead of work done by the system. In the context of physics, the common scenario is one of adding heat to a volume of gas and using the expansion of that gas to do work, as in the pushing down of a piston in an internal combustion engine. In the context of chemical reactions and processes, it may be more common to deal with situations where work is done on the system rather than by it. R Nave Enthalpy Four quantities called " H = U + PV where P and V are the pressure and volume, and U is internal energy. Enthalpy is then a precisely measurable Q = ΔU + PΔV since in this case Q=ΔH It is a useful quantity for tracking chemical reactions. If as a result of an exothermic reaction some energy is released to a system, it has to show up in some measurable form in terms of the state variables. An increase in the enthalpy H = U + PV might be associated with an increase in internal energy which could be measured by calorimetry, or with work done by the system, or a combination of the two. The internal energy U might be thought of as the energy required to create a system in the absence of changes ...