Kinetic Theory of Gases 2023 with verified questions and answers

Kinetic Theory of Gases Gases are made up of tiny particles. - Usually atoms or molecules The particles of a gas are far apart from each other. -The volume of gas particles is insignificant relative to the space between the particles The particles of a gas are in constant motion and collide with each other and the walls of their container. -The collisions are elastic; no K.E. is lost. -Collisions exert a force pressure The particles of a gas do not exert any force on each other except when they collide Temperature is a measure of the average kinetic energy of the particles of a gas Explain why gases do not have a definite shape and why they expand to fill their container They don't have intermolecular forces to keep them together. Explain how a sailboat works. Describe the process which allows it to be propelled forward through the water. Particles are always in motion when they collide with the sail they exert a force on it, and the boat moves. The force of the gas on the sail is greater than the drag force. Explain why a balloon feels squishy. The particles are far apart from each other so you can easily push them together Explain why gas particles can mix easily with each other. For example, why do odors travel quickly throughout a room? There are no forces holding them together so the can spread Particles are moving fast Explain why twisting an empty water bottle can cause the cap to fly off. Gas particles are constantly moving and colliding with things, so the particles would be hitting the cap. When the bottle is twisted there is an increased pressure so more gas particles will hit the cap of the bottle more frequently. When someone opens the bottle the cap could fly off due to the pressure from the gas particles Explain how a bicycle tire filled with air maintains its shape. Particles are always in motion, they collide with the inside of the tire and when enough oxygen gas is added to the tire they will be hitting the inside of the tire enough times that the tire will maintain its shape. Expansion of gases -No definite shape or volume -Expand to fill their container -No molecular forces holding them together Fluidity of Gases -Gases have the ability to flow Low Density 1 mole of H2O @ 20oC: 18 mL 1 mole of H2O @ 120oC and 1 atm: 22.4 L Compressibility -Gases can be easily compressed Diffusion mixing of particles due to random motion of particles Effusion process in which gases past through a tiny opening Real gas -one that does not behave according to the KMT Pressure= force/surface area Atmospheric Pressure` The gases that make up the atmosphere exert pressure on their surroundings. It is a result of: -Collisions between gas particles. -The weight of the atmospheric gases above the earth's surface. Measuring Pressure Atmosphere: -using a barometer -Atmospheric pressure depends on elevation and weather. -The normal atmospheric pressure at sea level: 760 mm Hg Normal: -A manometer can be used to measure the pressure of an enclosed gas. -The pressure is measured relative to atmospheric pressure Standard Temperature and Pressure 1 atm 0C Units of Pressure Unit - Symbol - Std. Atmospheric pressure Atmospheres - atm - 1 Millimeters of Hg - mm Hg - 760 Centimeters of Hg - cm Hg - 76 Avogadro's Law -Equal volumes of a gas at constant temperature and pressure contain equal number of particles. -At constant temperature and pressure the number of moles of gas is directly proportional to the volume k=V/n Combined Gas Law Boyle's Law, Charles' Law, and Gay-Lussac's Law can be combined k=PV/T Dalton's Law of Partial Pressures -The pressure of a mixture of gases is equal to the sum of the pressures of each individual gas. -Partial pressure- the pressure of an individual gas in a gas mixture. PT= P1 + P2 + P3 +....