CHM110H5 Study Guide - Midterm Guide: Chemical Polarity, Molar Mass, Phenolphthalein

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26 Nov 2012

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Study notes for chemistry midterm 2 - friday, nov 9th. Molecules are far apart; most of the volume is empty space. Molecules are in constant motion; they travel in straight line paths. Diffusion process by which a gas mixed with another; random movement of gas particles in a medium. Effusion process by which a gas escapes a container through a small opening; gas movement through a hole. Molecular velocities: at constant t, the average kinetic energy and velocity are constant, there is a wide range of values for the kinetic energy and velocity of individual molecules, relative average velocities depend on relative masses. So, the heavier the molecule, the slower it moves. Diffusion and effusion rates are known as r, so: r1 = m2 r2 m1. Mean free path: the average distance a particle travels before it collides with other particles effusion < diffusion < molecular velocities (due to collisions) Van der waal"s equation: (p + n2a/v2)(v-nb) = nrt where,

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M 121 1 201 Ideal Gas Law (PV n Experiment to T ) Determine the Ideal Gas Constant R 1. Conduct basic measurements, measurement , mathematical calculations and conversions for of volume, pressure, and temperature: calculate percent error and account for sources of error in an e xperimental result name and by following safety proced ty experiments for a redox reaction by using equipment identifiable by form chemical calculations using mass, mole and volumes and idenify limitatios of measuring devices in order to state the uncertainty/significant figures in measurements and calculation results. 5. Demonstrate a proficiency in relating the chemistry of gases to everyday phenomenon. Introduction Molecules in gases have very little attraction for one another, because relative to their size, they are so far apart from each other. For this reason we can often assume that a gas behaves "idcally." meaning that the physical behavior of the gas is independent of the composition of the gas. If a gas behaves ideally, then its physical properties can be described by the Ideal Gas Equation: Let's consider why the variables in the ideal gas equation have the relationships expressed in Equation 1aã The ideal gas equation assumes that there are no attractive forces between gas molecules. One can picture two billiard balls bouncing off one another in a totally clastic collision. If these molecules are placed in a balloon the collisions will occur not only with each other but also with the wall of the balloon, causing the balloon to expand. This expansion can be measured as a volume (V). More molecules will cause more collisions and thus more expansion. Therefore the quantity of molecules or number of moles (n) is directly proportional to the volume, and thus volume and number of moles appear on opposite sides of the equation. Another factor to consider is the kinetic energy of these molecules. Kinetic energy is related to the temperature (T) of the molecules, in that the kinetic energy. If the collisions with the wall of the balloon are happening at a very high speed due to high kinetic energy, the collisions will be harder and more frequent and thus the wall of the balloon will be pushed out further (a larger volume) than if the kinetic energy were less. The result is that volume is also directly proportional to the temperature. This relationship is seen in Equation la with (T) on the right side of the equation and (V) on the left. higher the temperature the greater the considered. While the molecules inside the balloon are pushing the balloon out, there are also molecules in thea Finally the pressure of the outside environment (atmospheric pressure) needs to be 59

CHM110H5 Study Guide - Midterm Guide: Chemical Polarity, Molar Mass, Phenolphthalein

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