CH 1401 Lecture Notes - Lecture 5: Gas Constant, Jmol, Barometer

• School: St. Mary's University
• Department: Chemistry
• Course: CH 1401
• Professor: Asamoah

Document Summary

Pv/nt= r - 0. 08206 atm*l/mol*k (atm = atmosphere) Molar gas constant when working with energy the value of r = 8. 314 jmol^-1k^-1. P= pressure v= volume n= number of moles t= temperature k= kelvin. Kelvin t = celsius t + 273. Increasing the # of gas molecules causes more of them to hit the wall at the same time. In order to keep the pressure constant, the volume must then increase. The pressure of a gas is proportional to temperature. P= 1 atm & t= 273 k (0 degrees c) Diffusion- mixing into one another higher concentration to lower concentration. Effusion- where it is moving from higher to lower (small hole and it"s escaping out of it) For two different gases at the same temperature, the ratio of their rates of effusion is given by: Density = p*mm=m/v *rt p*mm/rt = density. If it does not say it is stp, use the pv=nrt equation pv= mass/ molar mass *rt.