University:
Ohio State University
Course:
CHEM 1210 | General Chemistry I
Academic year:

2021
Views:

318

Pages:

2
Author:

Harriet D.

Chapter 10 Temperature and Pressure Temperature: average speed of gas molecules Pressure: result of the force they exert when they bounce off of things kinetic Molecular Theory of Gases 3 Assumptions Size of particle is negligibly small (take up no space) Speed of particles is proportional to kinetic energy average KE = temperature Thus, heavier atoms/molecules move more slowly at given temp Collisions are elastic (no energy is lost to deformation, but it can be transferred) Pressure = Force area average number of collisions creates pressure Density and Molar Mass density = molar mass / molar volume = g/mol / L = g/L Density of gas is directly proportional to the molar mass d = M / V Kinetic Molecular Theory basis for the ideal behavior of gases approximates particles have negligible size no interactions Speed: Urm² = √(5RT/M²) Kinetic energy: Ek = (3/2)kT = (3/2)RT (1/2)mv² = (3/2)kB T Boltzmann Constant kB = 1.38 * 10^-23 J/K log(m²/5k) = (1/k)k = J V = √(3kB T / m) Latm Velocity of molecule R = 0.08206 mol K NA = 6.022 * 10^23 molecules/mol 1.38 * 10^-23 J/K = 8.314 J/mol K = R OR U = √(3RT/M) • Average kinetic energy is proportional to temperature As mass increases, average velocities decrease Ump: the speed exhibited by the largest number of molecules Vav: the average (mean) speed of all the molecules Urms: the speed of a molecule whose kinetic energy is equal to the average (mean) kinetic energy of all the molecules • Diffusion: process of spreading out in response to concentration gradient faster (lighter) molecules spread faster

Chemistry Unit 3 - Chapter 7 + Chapter 9 - Stoichemistry

Related Documents

Recommended Documents

Description

Related Documents

Free up your schedule!

Take 5 seconds to unlock