6 Oct 09

# 6 Oct 09 - Chemistry 6 Oct 09 Ch. 5.1 Pressure, P =...

This preview shows pages 1–3. Sign up to view the full content.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

Unformatted text preview: Chemistry 6 Oct 09 Ch. 5.1 Pressure, P = Force/area-force per unit area Barometer: P = pgh-Torriceli Barometer|-Manometer Units of pressure-standard atmosphere-mmHg/torr-psi (lb/in^2)-Pascal (Pa= N/m^2)-Bar (ba, b) Conversions of Pressure Standard atmosphere- atm-1 atm = 760 mmHg-1 atm = 760 torr (1 torr= 1mmHg?)-1 atm = 14.7 psi-1 atm = 101325 Pa-1 bar = 100,000 Pa (1mb = 100 Pa) Sample Exercise 5.1: Pressure Conversion, p. 181-The pressure of a gas is measured as 49 torr. Represent this pressure in both atm and Pa. 49 torr = 49 x 1 torr = 49 x (1/760)atm = 6.4 x 10^-2 atm 6.4 x 10^-2 atm = 6.4 x 10^-2 101325 Pa = 6.5 x 10^3 Pa Law of Gases-Boyle's Law P 1- V 1 = P 2 V 2-Charles' Law V 1 /T 1 = V 2 /T 1-Gay-Lussac's Law P 1 /T 1 = P 2 /T 2-Avogadro's Law V 1 /n 1 = V 2 /n 2 5.1 Boyle's Law product of pressure times volume is a constant, provided the temperature remains the same 1. PV= k (k is a constant) 2. P is inversely related to V, P= k/V 3. The P-V graph is hyperbolic.-Another format of Boyle's Law P 1 V 1 = k = P 2 V 2 P 1 V 1 =P 2 V 2 5.2 Gay-Lussac's Law:-pressure of a fixed mass and fixed volume of a gas is directly proportional to the gas' temperature...
View Full Document

## This note was uploaded on 08/29/2011 for the course CHEM 101 taught by Professor Luikang during the Fall '10 term at SPSU.

### Page1 / 6

6 Oct 09 - Chemistry 6 Oct 09 Ch. 5.1 Pressure, P =...

This preview shows document pages 1 - 3. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online