Segment E: Ideal Gas Law
Segment E: Ideal Gas Law
This segment dives further into the ideal gas law. It includes the students and teacher discussing the models the student made in segment D to demonstrate the relationship between pressure and volume in gases. The teacher gives the students an engineering and design challenge: create a safe model of an airbag using what they have learned about the behavior of gases.
Obtain, evaluate, and communicate information about how to refine the design of a chemical system by applying engineering principles to manipulate the factors that affect a chemical reaction.
Plan and carry out an investigation to provide evidence of the effects of changing concentration, temperature, and pressure on chemical reactions.
Obtain, evaluate, and communicate information about the Kinetic Molecular Theory to model atomic and molecular motion in chemical and physical processes.
Develop and use models to quantitatively, conceptually, and graphically represent the relationships between pressure, volume, temperature, and number of moles of a gas.
Obtain, evaluate, and communicate information to compare and contrast the phases of matter as they relate to atomic and molecular motion.
Plan and carry out investigations to identify the relationships among temperature, pressure, volume, and density of gases in closed systems.
activation energy - the minimum amount of energy that reactants must possess in order to undergo a specific reaction.
catalyst - a substance that provides a lower energy pathway for reactants to convert to products without getting used up or changing itself.
collision theory - a theory that states that particles must collide in order to react.
effective collision - collisions that result in a successful reaction.
ideal gas - gas that follows the behavior described by kinetic molecular theory.
ineffective collision - collisions that do not result in a successful reaction.
kinetic energy - the energy of motion.
kinetic molecular theory - A theory of the thermodynamic behavior of matter, especially the relationships among pressure, volume, and temperature in gases, based on the dependence of temperature on the kinetic energy of the particles of a substance.
reaction rate - the change in concentration of a reactant or product over time.
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