Experiment 11 The Gas Laws Introduction: In this experiment you will (1) determine whether Boyle’s Law applies to a mixture of gases (air) and (2) calculate the gas constant‚ R‚ by determining the volume of a known amount of gas (H2) at a measured temperature and pressure. Determination of Whether Boyle’s Law Applies to Air Boyle’s Law states that for a fixed amount of gas at constant temperature‚ the pressure of the gas will vary inversely with the volume so that P ∝ 1/V or PV = a constant (if
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atoms/ions in a chemical formula. They are the small numbers within the chemical formula. They tell how many individual atoms/ions are present. 2. State the Law of Conservation of Mass and explain its relationship to stoichiometry. The Law of Conservation of Mass states that “Matter can neither be created nor destroyed during a chemical reaction.” This law is dictates the necessity for balancing a chemical equation with coefficients; if we didn’t balance equations‚ we would be created and/or destroying
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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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molecular considerations‚ identify which intermolecular interactions are significant (including estimating relative strengths of dipole moments‚ polarizability‚ etc.) • Apply simple rules for calculating P‚ v‚ or T ◦ Calculate P‚ v‚ or T from non-ideal equations of state (cubic equations‚ the virial equation‚ compressibility charts‚ and ThermoSolver) ◦ Apply the Rackett equation‚ the thermal expansion coefficient‚ and the isothermal compressibility to find v for liquids and solids • State the molecular
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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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Practical 6 -Determining the Gas Constant Aim: To verify the gas constant as 8.31 J/mol/K ( ) and to calculate the molar mass of butane. Theory: The ideal gas law‚ PV=nRT‚ is used to model an ideal gas‚ which is a gas with no intermolecular forces other than those of collisions‚ perfectly spherical and elastic particles. Although an ideal gas is a theoretical model and so cannot exist in practice‚ most gases behave fairly similarly to an ideal gas. Gases behave more like an ideal gas when they are at a higher
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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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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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