5 Ideal gasRelationship between Avogadro’s number, Universal Gas constant, and Boltzmann constant.
6 Kinetic –molecular theory Many molecules are in a container and they behave like point particles.(No volume)The molecules move around randomly, and obey Newton’s laws.The only interactions that the molecules undergo are elastic collisions with each other and the walls of the container.
7 Kinetic –molecular theory Pressure is a result of the molecules colliding with the walls of the container. As the number of molecules or thir average speed increases, the pressure increases.
8 Kinetic –molecular theory Results of kinetic-molecular theory.
9 Kinetic –molecular theory Results of kinetic-molecular theory.
10 Kinetic –molecular theory Internal energy of an ideal monatomic gas..
11 Kinetic –molecular theory Other gas laws – the amount of gas does not change
12 Laws of Thermodynamics The first Law of Termodynamics – If U is the internal energy of a system, than DU=Q-W. If Q>0 System gains heat If Q<0 System loses heat If W>0 Work is done by the system If W<0 Work is done on the system
13 Laws of Thermodynamics The first Law of Thermodynamics – If U is the internal energy of a system, than DU=Q-W
14 Table 18-1 Signs of Q and WQ positiveSystem gains heatQ negativeSystem loses heatW positiveWork done by systemW negativeWork done on system
17 Laws of Thermodynamics At constant pressure, the work done by or on a system is W=PΔV The area under a PV curve represents work. If a process occurs at a constant volume, the work done during the process is 0.
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