CH 101 Study Guide - Final Guide: Mean Free Path, Partial Pressure, Ideal Gas

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plumtermite154

8 Dec 2016

School

University of Alabama

Department

Chemistry

Course

CH 101

Professor

Jared M.Allred

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Document Summary

Gases are: one of the phases of matter, composed of particles that are moving randomly and very fast in their container(s) Gas particles move in straight lines until they collide with either the container wall or another particle; then they bounce off. A gaseous atom or molecule exerts a force when it collides with: a surface, other gaseous particles. Pressure is the force exerted per unit area by gas molecules as they strike the surfaces around them: pressure = (cid:3033)(cid:3032) (cid:4666)(cid:4667) (cid:3032) (cid:4666)(cid:4667) the surfaces around them. Gas pressure is a result of the constant movement of the gas molecules and their collisions with: the pressure of a gas depends on several factors: Average speed of the gas particles: the total pressure exerted by a gas depends on several factors: Concentration of gas molecules in the sample. The higher the concentration, the greater the pressure. Number of gas particles in a given volume.

Related Questions

1.) A gas is found to have a density of 3.165 g/L at STP. What is its molar mass? Which of the following gases is it most likely to be?

Molar Mass: _________

a. NH3
b. O2
c. Cl2

d. SF6

2.) Calculate the pressure exerted by 5.05 moles of NCl3 gas in a 20.00-L container at -205Â°C for a real gas. (for xenon: a= 42.63 atmÂ·L2/mol2 and b= 0.2450 L/mol)

3.) 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.

1. Consider the following equation: 4C3H5(NO3)3(s) â 12CO2(g) + 10H2O(g) + 6 N2(g) + O2(g) MW C3H5(NO3)3(s) = 227.1 g/mol 205 g of C3H5(NO3)3 is reacted. Assume reaction goes to completion and all the product gases are collected at 195.0 Co. The pressure is 0.95 atm. What is the total volume of the gases?

2.Which of the following is a TRUE statement about gas?

Gas particles exert a pressure when they hit the sides of the container.

In general, doubling the pressure of a gas doubles its volume.

Because the molecules have small distances between them compared

to their size, they can't be compressed

Hold the volume constant and decrease temperature

3.One mole of oxygen gas is at one atmosphere of pressure and 10 ^oC. How can a scientist increase the pressure of the gas?

Decrease the temperature and hold volume constant

Increase the volume constant and decrease the temperature

Decrease the volume and increase the temperature

hold temperature constant and increase the volume

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

CH 101 Study Guide - Final Guide: Mean Free Path, Partial Pressure, Ideal Gas

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