Chapter 6 – Properties of gases lecture notes 1. Gas phase Gases have neither definite shape or volume 1) volume changes with pressure 2) volume changes with temperature 3) gases are miscible 4) gases are generally MUCH less dense than liquids 2. Atmospheric pressure 1 atm = 760 torr (mm of Hg) F= ma F = force m = mass a = acceleration P = F/A - ma/A P = pressure
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First Law-Exercise: Problem 1: A volume 10 m3 contains 8 kg of oxygen at a temperature of 300 K. Find the work necessary to decrease the volume to 5 m3‚ (a) at a constant pressure and (b) at constant temperature. (c) What is the temperature at the end of the process in (a)? (d) What is the pressure at the end of process in (b)? (e) Show both processes in the p-V plane. Problem 2: The temperature of an ideal gas at an initial pressure p1 and volume V1 is increased at constant volume until the pressure
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LESSON 05.01 Wood blocks- solid Hammer- solid Lightning- plasma Fluorescent light bulb- plasma Steam and helium filled balloon is gas Water from a faucet and swimming pool is liquid - Can be distinguished at the molecular level by how the particles are held together - The phase of matter is considered a physical property because a change in a substance’s phase does not change the chemical properties or identity of the substance. - The phases of matter are determined by the kinetic energy
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important principles of physics: the ideal gas law and Archimedes’ principle are the reasons hot air balloons fly. The mathematical relationship between the volume pressure and the temperature of a gas is called the ideal gas law. When a gas is heated‚ as in a hot air balloon‚ then its volume will increase. However‚ there is a heater located in the balloon’s basket that heats the air inside the balloon and blows hot air into the balloon. As the volume of gas increases‚ it fills the balloon. As soon
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energy -only particles in liquid and gas have this type of energy Gases and Pressures Changes Pressure -recall: pressure id the force that is exerted on an object perunit of surface area -formula: pressure = force/area OR P = F/A -the SI unit for force is newtons (N) and unit for area is square meters (m2) -therefore pressure has a unit of N/m2 -other units of pressure -Pascal (Pa) -millitetres mercury (mmHg) -atmosphere Atmospheric Pressure -the gas molecules in our atmoshpere are pulled
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Chapter 3 The second law Physical Chemistry. Atkins 9th ed. 1 Outcomes • Concepts 1. The second law of thermodynamics: Spontaneous changes‚ Entropy (ΔS)‚ Heat engine (Carnot cycle)‚ Clausius inequality. 2. Entropy changes: ΔS of expansion‚ ΔS of phase transitions‚ ΔS during heating‚ measuring entropy‚ the 3rd law of thermodynamics‚ 3rd law entropies. 3. Criteria for spontaneity: Helmholtz energy (A)‚ Gibbs energy (G)‚ Maximum work (ΔA)‚ maximum non-expansion work (ΔG). 4. Combining
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Contents ------------------------------------------------------------------------ I. Introduction………………………………………......3 II. Thermodynamics Properties………...….……………5 III. Thermodynamic Laws……………………………….6 IV. Compression Cycles…………………………………7 V. Ideal Positive Displacement Compressor Cycle……………8 VI. Ideal Dynamic Compressor Cycle.......………………9 VII. Compressor Types……………………………...……9 VIII. Centrifugal Compressor……………………...….…..9 IX. Centrifugal Compressor Types……………………...10 X. Compressors
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Kinetic Theory of ideal gases - It is employed to express quantitatively the ideal gas model. Postulates: 1- A gas consists of molecules of mass (m) and diameter (d). 2- Molecules move continuously and randomly. 3- Molecules are treated as points‚ having no volume 4- Molecules collide with each other‚ changing direction and velocity. 5- Collisions are elastic (no loss of translational energy) no potential energy of interaction between them. Derivation of the ideal gas equation from the
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atom (F‚ O or N) of another molecule. THERMAL ENERGY Thermal energy is the energy of a body arising from motion of its atoms or molecules. It is directly proportional to the temperature of the substance. THE GAS LAWS Boyle’s Law At constant temperature‚ the pressure of a fixed amount of gas is inversely proportional to its volume. P1V1 = P2V2 Each curve corresponds to a different constant temperature and is known
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Chemistry June Exam Notes Quantities in Chemical Reactions Molecular and formula mass o The mass of one unit of a compound (a molecule or a formula unit) o The sum of the mass of all the atoms in a compound o With knowledge of the mass of each individual atom‚ the percentage composition by mass can be determined The Mole (mol) o A counting unit‚ one mole refers to 6.02 x 1023 particles of any given substance o Known as Avogadro’s Constant and given the symbol NA Molar Mass o The
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