CHM 191 Lecture Notes - Lecture 9: Magnetic Quantum Number, Gas Laws, Bohr Model
Document Summary
Pressure (p)=atm (atmosphere), pa (si unit, pascal), or mmhg (torr) Pascal(pa) = j/m^3, pressure (p) = force/area , f=mg (physics pressure) Graham"s law: (diffusion)the rate at which one gas mixes with another gas is related to the molar mass of the gasses. (molar mass: related to how fast the molecules are moving) Came up with by: rate of diffusion is proportional to the square root of the molar mass. 1/2m(avg)v^2 | elements at the same temp have the same average kinetic energy. m1v1^2=m2v2^2 | v1^2/v2^2 = m2/m1 = v1/v2 = (cid:884)/(cid:883) Ideal gas law: pv=nrt | v= (nrt)/p p=(rt)/(v-b) t a^2/v^2. Effusion: movement of one gas through a smaller hole into another spacious cavity, allowing the smaller ones to move quicker. He effuses 2. 8x faster than 02 t1/t2 = (cid:883)/(cid:884) 20 ne & 22 n: s= (cid:884)(cid:884)/(cid:884)(cid:882)-> 1. 05. Pressure (p)=752 mmhg ,temperature (t)=35 , amount = 0. 728 g c6h6. R= 0. 0821 latm/molk pv=nrt, 1 mole = 78g c6h6 n= #moles.
