Chapter 1: Intermolecular Forces: Liquids‚ Solids‚ and Phase Changes Chem 11: General Chemistry 2 Topics 1.1 An Overview of Physical States and Phase Changes 1.2 Quantitative Aspects of Phase Changes 1.3 Types of Intermolecular Forces 1.4 Properties of the Liquid State 1.5 Uniqueness of Water 1.6 The Solid State: Structure‚ Properties and Bonding A hot spring on a snowy day The Kinetic Molecular View of the Three States The characteristic properties of gases‚ liquids
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AOSC 200 Fall 2011 Key Topics to Study for the Final Exam What is the carbon dioxide and hydrologic cycles? What are the sources and sinks of each? Carbon Dioxide Cycle: How carbon is recycled through the atmosphere - Maximum CO2 in the Spring and minimum in the Fall because Spring comes right after winter. Therefore‚ all the plants that died during the Winter are not taking in CO2 for photosynthesis. Because these plants are not taking in CO2 there is more of it in the atmosphere. However
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reason why water has a high/strong surface tension. Heat of Vaporization-the quantity of heat a liquid must absorb for 1 g of it to be converted from the liquid to the gaseous state. Evaporative Cooling- The faster molecules escape and become a gas and the slower/cooler molecules left behind‚ causing a cooling effect. Specific Heat- A measurement of how well a substance resists changing its temp when absorbs or releases heat. Heat-the measure of the total quantity of kinetic energy due
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enthalpy of combustion of solid naphthalene was calculated to be -6862.68 kJ/mol using bond energies for the gaseous molecules‚ the heat of vaporization of liquid water and the literature value of the heat of sublimation of naphthalene‚ which was 72 ± 4 kJ/mol.2 The absolute value of the difference between the theoretical heat of combustion and the literature value heat of combustion of naphthalene was 1702.68 ± 20 kJ/mol.2 This difference indicates that the resonance energy of naphthalene is very
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fractional distillation for separation of a mixture of toluene and cyclohexane. The mixture was first separated using simple distillation. A simple distillation apparatus was set up and a Thermowell heater containing sand will also be used as the heat source. The mixture will be slowly heated and condensed. The temperature as a function of the number of drops will again be recorded. Afterwards‚ fractional distillation apparatus was set up‚ and the mixture was brought to a boil and slowly condensed
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PROPERTY DIAGRAMS OF PURE SUBSTANCES SUBJECT : ENGINEERING THERMODYNAMICS CONTENTS: * Phase and pure substance * Properties of a substance * P-V diagram for a pure substance * P-T diagram for a pure substance * P-V-T surface * T-S diagram for a pure substance * h-s diagram for a pure substance Thermodynamic Properties * Characteristics by which physical properties of system may be described. e.g. pressure‚ volume‚ temperature‚ entropy‚ enthalpy etc
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Chemistry 101 Chapter 6 THERMOCHEMISTRY · Thermochemistry is the study of the quantity of heat energy released or absorbed in a chemical reaction. Example: the burning of fuel: is a heatevolving reaction · Heat : · Energy: is a form of energy the potential to do work (to move matter) exists in many different forms: Electrical energy Kinetic Energy (energy of motion) Light energy Heat energy Chemical energy (energy of substances) · Different forms of energy can be interconverted
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significant figures! ] SHOW YOUR WORK to get full credit. 1) Number of moles: 2) Pressure of each gas: 2. [ out of 16 pts ] When 11.1 g of lead reacts with 3.81 L of oxygen gas‚ measured at 1.00 atm and 25.0°C‚ 11.8 kJ of heat is released at constant pressure. What is ∆H° for this reaction? (R = 0.0821 L • atm/(K • mol)) 2Pb(s) + O2(g) → 2PbO(s) [ do not neglect significant figures! ] SHOW YOUR WORK to get full credit. 1) Determine
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Thermodynamics: thermo = heat (energy) dynamics = movement‚ motion Some thermodynamic terms chemists use: System: the portion of the universe that we are considering open system: energy & matter can transfer closed system: energy transfers only isolated system: no transfers Surroundings: everything else besides the system Isothermal: a system that is kept at a constant temperature by adding or subtracting heat from the surroundings. Heat Capacity: the amount of heat energy required to
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Chapter 1: Biology- The study of life A Hierarchy of Organization 1. Molecules 2. Organelle 3. Cell 4. Tissue 5. Organ 6. Organism Emergent Properties- Novel properties that emerge as each step up the hierarchy of biological order is taken. Reductionism- Reducing complex systems to simpler components that are more manageable to study. Cells- The lowest level of structure capable of performing all the activities of life‚ all organisms are composed of cells which are the basic units of structure
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