PPT-Molar Volume of Gases ,

Percent Composition Empirical Molecular Formula Finishing Up Ch 10 In 1811 Avogadro proposed a hypothesis Volumes of gases at the same temp and pressure have the same number of particles. Chapter 5. E-mail: . benzene4president@gmail.com. Web-site: http://clas.sa.ucsb.edu/staff/terri/. Gases – Ch. 5. 1. Draw the following:. a. A closed monometer attached to a flask filled with CO at 250 . Chapter 16.3. Behavior of Gases. What behaviors do gases display?. Do they behave the same all the time?. What variables are involved with gas behavior?. Variables . Pressure – the amount of collisions between gas particles and walls of the container (balloon). Measured in kilopascals (. What is the density in g/L of hydrogen gas at 20.0 . o. C. and a pressure of 1655 psi?. A sample of gas has a mass of 0.555 g. Its volume is 117 mL at a temperature of 85 . o. C. and a pressure of 753 mmHg. Find the molar mass of the gas. . Stoichiometry. of Gases. Objectives. Apply the principles of . stoichiometry. to determine the volume of any gas that is produced or consumed in a chemical reaction.. Volume-Volume Calculations. At STP, what volume of hydrogen gas is needed to react completely with 4.55 L of oxygen gas to produce water vapor?. Chapter . 3.2. Behavior of Gases. What behaviors do gases display?. Do they behave the same all the time?. What variables are involved with gas behavior?. Variables . Pressure – the amount of collisions between gas particles and walls of the container (balloon). Measured in kilopascals (. The Kinetic-Molecular Theory of Matter. Gases. Behavior of Atoms. Kinetic-molecular theory. .  . based on the idea that particles of matter are always in motion. Can be used to explain the properties of solids, liquids, and gases in terms of the energy of the atoms and the forces that act between them. 2. Gas Laws. We will examine the quantitative relationships, or . empirical laws. , governing gases. . Basically, we will learn about equations that are available to calculate P, V, T, & n for gases. . Behavior of Gases Chapter 3.2 Behavior of Gases What behaviors do gases display? Do they behave the same all the time? What variables are involved with gas behavior? Variables Pressure – the amount of collisions between gas particles and walls of the container (balloon). Measured in kilopascals ( Particle Theory. All . matter consists of many, very small particles . The particles . are constantly moving or in a continual state of motion. . The . degree to which the particles move is determined by the amount of energy they have and their relationship to other particles. . Molar Volume. 1 . mol. of gas = 22.4 L .  molar volume. What volume would be occupied by 0.77 moles of helium gas at STP?. Density of Gases. Density = molar mass/molar volume. What is the density of (in grams per liter) of carbon dioxide gas at STP?. Kinetic Molecular Theory of Gases. This is the six point model that is used to explain the behavior of gases. Points of the Kinetic Molecular Theory. 1. Gases are composed of atoms or molecules that have mass. 2. CHAPTER OUTLINE. Properties of Gases. Pressure & Its Measurement. The Gas Laws. Vapor Pressure & Boiling Point. Combined Gas Law. Avogadro’s Law. STP & Molar Volume. Ideal Gas Law. Partial Pressures. Equal volumes of gases contain equal numbers of molecules. Volume of a gas varies directly with the number of molecules if pressure and temperature stay constant. Standard Molar Volume. Volume occupied by 1 mole of a gas at STP. A strong attraction to each other and a large volume . A strong attraction to each other and no volume . A weak attraction to each other and a large volume . A weak attraction to each other and no volume .