CHEM 11200 Lecture Notes - Lecture 21: Ideal Gas, Intermolecular Force, Isochoric Process

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lemonhedgehog555

19 Jul 2020

School

University of Chicago

Department

Chemistry

Course

CHEM 11200

Professor

Kozmin

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Document Summary

Where the pressure is constant v and t are directly proportional to one another. When t increases, collisions will increase so the volume must increase so the pressure can stay constant. Where the temperature is constant p and v are inversely proportional to one another. When v decreases, there is less space, so collisions happen more, causing an increase in p. P and t proportion law: is an isochoric environment. Where the volume is constant p and t are directly proportional to one another. When p increases, the increased collisions cause an increase in. These combined laws together makes the aptly named combined gas law. Avogadro"s law : if two equal-volume containers hold gas at the same pressure and temperature, then they contain the same number of particles. Under high pressure and low temperature, the ideal gas assumptions don"t hold up.

Related Questions

So basically, Lussacâs Law is an ideal gas law where at a constant volume, the pressure of a fixed amount of gas is directly proportional to its temperature in Kelvins.

How would Lusaac's Law change if the volume is not constant?

Please Explain, Thank-You.

The ideal gas law relates the pressure P, volume V, absolutetemperature T, and amount of gas n. The law is P = nRT/V where R isthe gas constant.

An engineer must design a large natural gas storage tank to beexpandable to maintain the pressure constant at 2.2 atm. InDecember when the temperature is 4 degrees Farenheight (-15 C), thevolume of gas in the tank is 28,500 ft^3. What will the volume ofthe same quantity of gas be in July when the temperature is 88 F(31 C)? (Hint: Use the fact that n, R, and P are constant in theproblem. Note also that K = C + 273.2

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

CHEM 11200 Lecture Notes - Lecture 21: Ideal Gas, Intermolecular Force, Isochoric Process

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