CHEM101 Lecture Notes - Lecture 25: Ideal Gas Law, Partial Pressure, Horse Length

• School: University of Alberta
• Department: Chemistry
• Course: CHEM101
• Professor: Rylan Lundgren

Document Summary

Pv = nrt: r: 8. 314 j/mol k or 0. 08206 l atm/ mol k, make sure to use the right constant depending on what units you have in the quesion. The two gases do not react so n and t are constant: p1v1 = nrt = p2v2. For o2: p2 = (p1v1)/( v2) (1. 00atm x 46. 0 l)/(5. 00l) For he: p2 = (p1v1)/( v2) (2. 00atm x 12. 0 l)/(5. 00l) = 4. 80 atm: ptotal = 9. 20atm + 4. 80 atm. Not the case with non-ideal gases (gases which compress so much they. Paricles are in constant random moion are almost liquid: collisions between gas paricles with the walls of the container is the cause of pressure. There are no atracive or repulsive forces between paricles: all the interacions, bouncing, scatering etc are elasic. The average kineic energy of the collecion of gas paricles: directly related/proporional to the temperature of the gas. More heat = more energy = more movement = more ek = higher pressure.