userdata-paziras-Chem101-Chap_05A

Mmhg vgas100ml pgas1520mmhg vgas500ml pisdoubled

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Unformatted text preview: stry 101 Chapter 5 MEASURING THE PRESSURE OF GASES IN CLOSED CONTAINERS 1. The Closed Tube Manometer No pressure exerted Pressure of enclosed gas = difference in height = Dh 4 Chemistry 101 Chapter 5 2. The Open –Tube Manometer Pgas = Patm Pgas < Patm Pgas = Patm – Dh 5 Pgas > Patm Pgas = Patm + Dh Chemistry 101 Chapter 5 THE GAS LAWS · Assume the fo llowing measurements are obtained: Pgas = 760. mm Hg V gas = 100. mL Pgas = 1520 mm Hg V gas = 50.0 mL · P is doubled · V is halved P x V NOTE: 76,000 (mmHg)(mL) 76,000 (mmHg)(mL) Pgas = 2280.mm Hg V gas = 33.3 mL · · P is tripled V is one­third 76,000 (mmHg)(mL) 1. Volume and Pressure are inversely proportional 2. The product of the Pressure anf the Vo lume is constant. 6 Chemistry 101 Chapter 5 BOYLE’S LAW · The relat ionship between pressure and volume is called Bo yle’s Law. · At constant temperature, the volume of a fixed amount of gas is inversely proportional to its pressure. · Boyle’s Law can be interpreted and used both Mathematically and Graphically. Mathematically: PV = constant OR P1 V2 ¾¾ = ¾¾ P2 V1 OR P1V1 = P2 V2 Graphically: Assume the fo llowing data are obtained: P (atm) 0.50 V (mL) 20. P (a...
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This document was uploaded on 03/18/2014 for the course CHEM 101 at Los Angeles Mission College.

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