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CHEM 1A (149)
Lecture

gases:introandreview.pdf

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Department
Chemistry
Course
CHEM 1A
Professor
Amanda Brindley
Semester
Winter

Description
Gases - Intro & Review gas - particles move - compressible - exert pressure on surroundings - no defined shape - expand to fill surroundings - gases mix evenly - lower density than solids and liquids pressure = force / area or N / m^2 - called pascal, Pa - other units: torr, atm, mmHg - 1 atm = 760 mmHg = 101,325 Pa 825 mmHg to atm, Pa, and kPa 825 mmHg ( 1 atm / 760 mmHg) = 1.08 atm 5 2 825 mmHg ( 101325 Pa / 760 mmHg) = 1.10 x 10 Pa / 1000 = 1.10 x 10 kPa ideal gas - molecules move randomly - donʼt interact with each other - no volume - collisions are elastic, no energy is lost - work well at low pressure and high temperatures Gas Laws - boyleʼs law - assumes temperature and moles are constant - relates pressure to volume - increase in volume => decrease in pressure - P and V graph - curve // P and 1/V graph - straight po
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