Chem Exam 3 Ch. 11
About this set
Created by:
BelletristicBeast Plus on April 21, 2012
Description:
Gases and Their Properties
Log in to favorite or report as inappropriate.
Order by
43 terms
Terms | Definitions |
|---|---|
 Pressure | force exerted on an object divided by the area over which it is exerted; measured by a barometer in atm |
| Millimeters of Mercury (mm Hg) | 760 mm Hg = 1 atm; at sea level |
| Boyle's Law | volume of a fixed amount of gas at a given temperature is inversely proportional to the pressure exerted by the gas |
| Boyle's equation | P1V1=P2V2 at constant n and T |
| Charles's Law | the volume of a fixed quantity of gas at constant pressure decreases with decreasing temperature |
| Charles's equation | V1/T1=V2T2 at constant n and P |
| Temperature (T) | must always be expressed in Kelvins (°C+ 273.15=K) |
| General Gas Law | also known as Combined Gas law; combination of Boyle's and Charles's Law |
| General Gas Law Equation | P1V1/T1=P2V2/T2 when when T2 is greater than T1, P2 will be greater than P1 |
| Avogadro's Hypothesis | equal volumes of gases under the same conditions of temperature and pressure have equal numbers of particles |
| Avogadro's equation | Volume (V) = Constant (K) x Moles (n) |
| Ideal Gas Law | PV=nRT |
| R; Gas Constant (Ideal Gas Law) | 0.08206PV/nT; universal constant |
| n | PV/RT |
| V | nRT/P |
| P | nRt/V |
| T | PV/nR |
| Density (d) | PM/RT M=molar mass |
| M | dRT/P |
| Partial Pressure | pressure of each gas in a mixture |
| Dalton's Law of Partial Pressures | the pressure of a mixture of ideal gases is the sum of the partial pressures of the different gases in the mixture |
| Dalton's equation | Ptotal=P1+P2+P3... |
| Ptotal | (nA+nB+nC)(RT)/V = (ntotal)(RT)/V |
| Mole Fraction (X) | the number of moles of a particular substance in a mixture divided by the total number of moles of all substances present |
| (Pa) Pressure of a Gas | (Xa)(Ptotal) the ________________ in a mixture of gases is the product of its mole fraction and the total pressure of the mixture |
| Kinetic Molecular Theory of Gases | all gases, regardless of their molecular mass, have the same average kinetic energy at the same temperature (does not mean they have the same rms speed); average kinetic energy of gas particles is proportional to gas temperature |
| Kinetic Molecular Theory Equation | √U^2^ = √3RT/M |
| R (Kinetic Molecular Theory Rquation) | 8.314J/molK |
| M | molar mass= kg/mol |
| √U^2^ | root mean square (rms) |
| Temperature | kinetic energy of molecule increases; collision with the wall increases; therefore __________ of gas increases |
| Pressure | increasing the number of molecules of a gas at a fixed temperature and volume does not change average collision force but does increase number of collisions occurring per second; therefore _________ increases |
| Volume | ________ increases when pressure remains constant and number of molecules of gas or temperature increases |
| n | __________ is constant when volume decreases; number of collisions with the container walls per second must increase and pressure increases |
| Gas Pressure | force of collision/area |
| Diffusion | mixing of molecules of two or more gases due to their random molecular motions |
| Effusion | the movement of gas through a tiny opening in a container into another container where the pressure is very low; lighter molecules with average speeds strike the barrier more often and pass more often through it than heavier, slower molecules at the same temperature |
| Rate of Effusion (of a Gas) | the amount of gas moving from one place to another in a given amount of time; inversely proportional to the square root of its molar mass |
| Graham's Law | rate of effusion depends on the speed of the molecules |
| Graham's equation | rate of effusion of gas 1/rate of effusion of gas 2 = √molar mass of gas 2/molar mass of gas 1 |
| Real Gases | As attractive forces between molecules increase, deviations from ideal behavior become more apparent at relatively low temperatures; The volume occupied by the molecules can cause an increase in pressure compared to the ideal gas. |
| Ideal Gases | There are no attractive forces between molecules; Replacing one gas by another under the same conditions, has no effect on pressure |
| Van der Waals equation | (P+a[n/V]^2^)(V-bn)=nRT; developed to correct for the errors arising from nonideality |
First Time Here?
Welcome to Quizlet, a fun, free place to study. Try these flashcards, find others to study, or make your own.