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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HVAC 101 Definitions Atom – Is the smallest particle of an element. BTU – The amount of heat required to raise the temperature of 1lb of water 1 degree F Molecule – The smallest particle that a substance can be broken into and still retain its chemical identity. Conduction – Is energy that travels from one molecule to another molecule. Convection – To move heat from one location to another be means of current set up in a fluid medium. Density – The weight per unit of volume of a substance.
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Part III PHYSICS HSE II Time:2Hours Max:60 Scores 1. Three identical charges each +q are placed at the corners of an equilateral triangle of side d cm. Calculate the force on a +ive charge +2q at the centroid of the triangle. 2 2.If the earth is supposed to be a metallic sphere‚its capacity will be nearly (a) 700pf (b) 700 microfarad (c) 700f (d) 6.4 X10^6 f 1score 3. write the relation between dielectric constant and electric susceptibility. 1score 4. A box encloses an electric dipole consisting
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Mofu Lin Ms. Conte 15/3/12 IB Chemistry Soda can calorimeter(Energy content of food) Lab report Introduction We‚ human needs energy to live and for movements. Thus‚ we eat and combust food to release its heat energy in our bodies. In this experiment‚ we will determine how much heat energy released when we eat snack foods such as popcorn or potato chips. This lab includes three burning tests of different foods with different energy contents. Calorimetry is the science associated with determining the
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Homer Gere Science - Perry 7-3 Kober Balloon Lab Report Problem: The goal of the balloon lab was to get a balloon attached to a line all the way across the room. One limitation was that we could only use one balloon‚ two straws‚ and tape. The circumference of the circle at its largest point couldn’t be larger than 100 cm. Procedure/Results: Trial Number | Distance Traveled (CM) | Time (sec) | Velocity (CM/sec) | 1 | 346 | 1.02 | 339.2 | 2 | 471 | .79 | 596.2 | 3 | 356 | .8 |
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Change in Pressure and Different Depths in a Static Fluid Lab Marcus Uchaker MET: 2050 January 26‚ 2012 Purpose: The purpose of this lab is to devise a correlation between that of the data we have collected from our experiment and compare it to that of theory. In this experiment 3 different tests were done in order to test this theory. The first test was to tie a balloon on the end of a manometer and measure the pressure at different depths in a large beaker filled with water. The next
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2. First stage of Martens’ model of competition is Objective Competitive Situation: This means that without a witness or another person present then you cannot have proper competition. An example of this would be you running a mile at the track and you want to run this mile under 5 min. You have a friend there recording your time and you tell him you want to run under 5 min. This would be considered competition based on Martens’ thought on Objective Competitive Situation. Second in Martens’
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Experiment B2‚ Heats of Combustion – The Bomb Calorimeter. Objectives: To calibrate a bomb calorimeter by the combustion of benzoic acid. Then to use the calibrated calorimeter to measure the heat of combustion of naphthalene and calculate the heat of formation of naphthalene. Theory: q = C.ΔTBA C = q / ΔTBA Moles = mass / Mr ΔŪ = ΔU / moles ΔHoc‚298 = ΔŪoc‚298 + PDV = ΔŪoc‚298 + RTΔn C10H8 (s) + 12O2 (g) 10CO2 (g) + 4H2O (l) ΔHoc‚298 = - 1
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Assignment 3 ES230 Key solutions Problem 3.1 | | | | |A 90-N force is applied to the control rod AB as shown. Knowing that the length of the rod is | | |225 mm‚ determine the moment of the force about point B by resolving the force into components
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<i>1. State the five assumptions of the Kinetic-Molecular Theory of gases.</i><br><br>a) Gases consist of large numbers of tiny particles. These particles‚ usually molecules or atoms‚ typically occupy a volume about 1000 times larger than occupied by the same number of particles in the liquid or solid state. Thus molecules of gases are much further apart than those of liquids or solids.<br><br>Most of the volume occupied by a gas is empty space. This accounts for the lower density of gases compared
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