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CHEM 121 Lecture Notes - Lecture 3: Gas Laws, Root Mean Square

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ivorycrocodile554

11 May 2016

School

Simon Fraser University

Department

Course

Professor

Steven Holdcroft

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3:44 pm (cid:1) (cid:1) (cid:1) (cid:1) (cid:1) (cid:1) (cid:1) (cid:1) (cid:1) (cid:1) (cid:1) (cid:1) (cid:1) (cid:1) (cid:1) Kinetic energy of gas particle is proportional with temperature. Collisions of gas particles against container = pressure. Ideal gas law assumes that gas particles have no intermolecular attraction and no volume. Elastic collision: particle bounces off with the same amount of energy. Physics: force = mass x acceleration (f = ma) Applied to gases: force = change in momentum/change in time (mv/t) Units: change in momentum per unit time (2mv2/t) Keavg = na(1/2mv2) (cid:1) average kinetic energy for one mole of particle. Pv/n = 2/3keavg (cid:1) in relation to gas laws. Keavg = 3/2rt (cid:1) kinetic energy relation to temperature (kelvin) Temperature is the physical measure of kinetic energy. Collisions against the wall cause exchange of energy to equilibrate ke in two separate gas containers. To find ratio of root mean square velocities: O2 at stp, 1023 collisions/s per cm2 of wall.

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Related Questions

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