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CHEM 6B Lecture Notes - Lecture 3: Ideal Gas Law, Ideal Gas, Torr

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burgundyporpoise729

6 Apr 2018

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Department

Chemistry and Biochemistry

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Professor

Sandrine Bernoilles

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P t : as temperature increases, volume increases in an elastic container, temperature is a measure of relative kinetic energy of a substance, adding more gas to a system increases pressure and volume. If the same balloon is put in a freezer at 255k, what will be the new volume: pv = nrt, v/t = v/t. 255k: 1. 2*255/305, v = 1. 0l, nitrogen is often injected into cans and bottles to keep the contents from oxidizing. If the n2 is injected into a bottle w/ a volume of 10. 0ml @ a pressure of 1. 2 bar, what volume will it occupy @ a pressure of 0. 95 bar: pv = nrt pv = pv. Ideal gas calculations: pv = nrt, calculate the number of grams of propane, c3h8 in a 50. 0l container at a pressure of 7. 50atm and 25deg c. 7. 50atm == n: n = 15. 335 mol c3h8, 15. 335 mol * 44. 095g/mol = 676g, gas mixtures.

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Related Questions

Which of the following is NOT true in the kinetic molecular theory of ideal gases?

The size of the molecules are negligible compared to the volume of the container

The kinetic energy of a sample is proportional to the temperature of the gas.

Collisions are elastic (no friction occurs between the molecules when they collide)

The pressure of a sample is affected by which gases are present.

AND WHY?

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