Chem 1061 1st Edition Lecture 10 Outline of Last Lecture I Elements in Reduction Oxidation Reactions a Combination b Decomposition c Displacement i Double Displacement ii Single Displacement iii Activity Series d Combustion II Reversibility of Reactions Outline of CurrentLecture III Gases and Kinetic Molecular Energy a Identity of Gas IV Gas Pressure and measurement a Measuring Gas Pressure b Units of Pressure V Gas Laws and Their Experimental Foundations a Boyle s Law b Charles Law Current Lecture These notes represent a detailed interpretation of the professor s lecture GradeBuddy is best used as a supplement to your own notes not as a substitute Gases and Kinetic Molecular Energy Energy Kinetic motion E subscript k Potential position E subscript p Kinetic Molecular Theory 1 Particles are small compared to overall volume 2 Particles are in constant random motion 3 Particles collide with each other and container by elastic collisions Total E k Constant Particles will have MOLECULAR SPEED u Molecular speed is related to the average kinetic energy and is proportional to temperature T Identity of a Gas All gases have the same average kinetic energy at a given T E k mass x Speed 2 Most probable speed increases as the molar mass decreases formula logic Gas Pressure and Measurement Gas exerts pressure on the walls of its container Pressure P force area Atmospheric Pressure is the force of atmospheric gases attracted by gravity exerted on all forces P atm atmospheric pressure 14 7 pounds per square inch psi P inside P atm implodes P inside P atm explodes Measuring Gas Pressure Barometer measures atmospheric pressure and is measured in mmHg millimeters of Mercury At sea level 0degrees Celsius P atm 760mmHg Manometer used to measure gas pressure in an experiment Figure 5 4 is useful for homework Units of Pressure Si Unit Pascal Pa 1 Pa 1 n m 2 Standard Atmosphere atm 1 atm 1 01325 x 10 5 Pa 760 mmHg Torr 1 torr 1 mmHg 760 torr 760 mmHg Gas Laws and Their Experimental Foundations Gas is described by Pressure P Volume V Temperature T Amount n number of moles Law Relation Boyle s Law Volume and Pressure Charles Law Volume and Temperature Avogadro s Law Volume and Amount mol Ideal Gas assume no interactions between particles and gas volume is small negligible compared to overall volume Boyle s Law Volume is inversely proportional to Pressure T and n are constant PV Constant Increase pressure decrease volume Decrease pressure increase volume Charles Law Volume and Temperature is proportional T and n are constant Increase T Increase V Decrease T Decrease V
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