CHEM 1A Lecture Notes - Lecture 14: Gas Constant, Collision Frequency, Molar Mass

• School: UCSB
• Department: Chemistry and Biochemistry
• Course: CHEM 1A
• Professor: BERNT C M

Document Summary

Calculate the collision frequency for an o 2 molecule at 27 degree c and 1 atm (assume d. N = number of molecules (not moles, the actual number), d = collision diameter, M = the molar mass of the molecule in kg, and. R is the ideal gas constant = 8. 314j/mol k. To obtain n/v, we can solve it using pv = nrt. N (0. 082057 l atm mol k ) (27+273. 15k) *note that little n is the number of a substance in moles, while the big n is number of a substance in real terms. M = molar mass of o 2 in kg. O 2 : m = 2 x (16. 00g/mol) x (1kg/1000g) = 0. 032 kg/mol. And 1 picometer = 10 -12 m molecules/m ) *note: this collision rate is the intermolecular collision rate, meaning the collision rate between o 2 molecules, not between o 2 molecule and the container"s wall.