Overview
The object of reflection for this journal is your experience in learning the material during the week. You are advised to make entries regularly rather than completing it right before a submission date, and the quality of reflection should be the emphasis of your entries rather than over-emphasis on the word count.
Write an academic reflection in four paragraphs: describe, interpret, evaluate, and plan.
What did you learn this week?
What activities helped you to learn?
What activities did you find engaging?
How will you do to better understand your muddy points for the weekChapter 11 Overview and Learning Objectives OVERVIEW Gases are the state of matter easiest to theorize about. The Kinetic Molecular Theory explains gases in terms of molecules or atoms moving rapidly in mostly empty space and bouncing off of other molecules and the walls of the container. Pressure is related to the force of these collisions acting on the walls of the contain. Temperature is related to the kinetic energy of the moving molecules or atoms. Chemists use many different units to describe pressure--interconverting from one unit to another is common in problems involving gases. The Ideal Gas Law (PV=nRT) describes the relationship between the various properties used to describe gases. Dalton's Law of Partial pressure describes how mixtures of gases behave. Since the Ideal Gas Law has the number of moles (n) as one of its terms, we can make connections to stoichiometry calculations as discussed in previous chaptersChapter 12 Overview and Learning Objectives OVERVIEW LEARNING OBJECTIVES Enthalpy changes of phase transitions (12.5)
Label and explain the heating curve for a given substance
Identify phase transitions as endothermic or exothermic processes
Interconvert between enthalpies of phase transitions, heat exchanged, and the amount of sample
Explain why a substance’s enthalpy of vaporization is generally larger than a substance’s enthalpy of fusion