ENVIRSC 1A03 Lecture Notes - Lecture 3: Density Of Air, Ideal Gas Law, Atmospheric Pressure

• School: McMaster University
• Department: Environmental Science
• Course: ENVIRSC 1A03
• Professor: Luc Bernier

Document Summary

Iclicker question: why does a mountain climber at the top of mt. Everest need to use an oxygen tank: b) there is less air. Atmospheric pressure > weight = mass x gravity. Weight = mass x g: 10,339. 3 kg x 9. 8 m s(-2, = 101325 kg m s(-2, = 101325 n. Pressure = force/area: = 101,325 n m(-2, = 101,325 pa, = 101,325 kpa. Relations between air pressure and altitude: air pressure: decreases with altitude, with rising altitude, the greatest drop occurs: near the surface. A mountain climber at the top of mt. Air density: density = mass/volume, near sea level = 1. 2 kg m(-3) Standard sea-level pressure: = 1013. 2 hpa, = 29. 92 in hg, = 76 cm hg, = 1cm hg = 13. 32 hpa. The ideal gas law: the law states that: P = air density (kg/m(3)) (2nd p)