CHM135H1 Lecture Notes - Lecture 9: Van Der Waals Equation, Ideal Gas Law, Capillary Action

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CHM135H1 Full Course Notes

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Kinetic energy increases with temperature (ke = 3 * r * t / (2n) Results from gas particles colliding with container walls. More particles -> more collisions -> greater pressure. Higher temp -> higher ke of particles -> more collisions -> greater pressure. Less volume -> more collisions -> greater pressure. High pressure -> pv/nrt > 1 due to molecular volume. Space between molecules smaller, volume of molecules becomes significant. Corrections to ideal gas law (p+n2a/v2)*(v-nb) = nrt. A -> atm * l^2 / mol ^2. Examples: 1l of gas a at 1 atm and 1l of gas b at 1atm are mixed in 2l container. Pressure of mixture is less than 1 atm: this means that molecules of b are attracted to molecules of a more than to themselves. Particles close together, but moving past each other. Surface tension : amount of energy required to expand a liquid surface.

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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

CHM135H1 Lecture Notes - Lecture 9: Van Der Waals Equation, Ideal Gas Law, Capillary Action

CHM135H1 Full Course Notes

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