chapter 10 Gases

chapter 10 Gases - General Chemistry I General Chapter 10...

Info iconThis preview shows pages 1–15. Sign up to view the full content.

View Full Document Right Arrow Icon
General Chemistry I General Chemistry I Chapter 10 Chapter 10 Gases Gases
Background image of page 1

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

View Full DocumentRight Arrow Icon
Gases You Have Encountered Gases You Have Encountered
Background image of page 2
Characteristics of Gases Characteristics of Gases Gases always form homogeneous mixtures with other gases Gases are highly compressible and occupy the full volume of their containers. (Chapter 1) When a gas is subjected to pressure, its volume decreases. .
Background image of page 3

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

View Full DocumentRight Arrow Icon
Pressure is the force acting on an object per unit area: Gravity exerts a force on the earth’s atmosphere A column of air 1 m 2 in cross section exerts a force of 10 5 N. The pressure of a 1 m 2 column of air is 100 kPa. SI Units: 1 N = 1 kg.m/s 2 ; 1 Pa = 1 N/m 2 . Pressure Pressure A F P =
Background image of page 4
Background image of page 5

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

View Full DocumentRight Arrow Icon
Background image of page 6
Atmosphere Pressure and The Barometer If a tube is inserted into a container of mercury open to the atmosphere, the mercury will rise 760 mm up the tube. Atmospheric pressure is measured with a barometer . Standard atmospheric pressure is the pressure required to support 760 mm of Hg in a column . Units: 1 atm = 760 mmHg = 760 torr = 1.01325 × 105 Pa = 101.325 kPa.
Background image of page 7

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

View Full DocumentRight Arrow Icon
Class Guided Practice Problem (a) Convert 0.527 atm to torr (b) Convert 760 torr to kPa Class Practice Problem (c) Convert 147.2 kPa to (1) atm and (2) torr
Background image of page 8
Atmosphere Pressure and The Manometer The pressures of gases not open to the atmosphere are measured in manometers. A manometer consists of a bulb of gas attached to a U-tube containing Hg: – If P gas < P atm then P gas + P h 2 = P atm . – If P gas > P atm then P gas = P atm + P h 2 . (See example problem 10.2)
Background image of page 9

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

View Full DocumentRight Arrow Icon
Defining States of Gases Defining States of Gases Gas experiments revealed that four variables will affect the state of a gas: Temperature, T Volume, V Pressure, P Quantity of gas present, n (moles) These variables are related through equations know as the gas laws.
Background image of page 10
Consider the three gas laws. We can combine these into a general gas law: Boyle’s Law: Charles’s Law : Avogadro’s Law: The Ideal Gas Equation The Ideal Gas Equation ) , (constant 1 T n P V ) , (constant P n T V ) , (constant T P n V P nT V
Background image of page 11

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

View Full DocumentRight Arrow Icon
The Gas Laws: The Gas Laws: Boyle’s Law The Pressure-Volume Relationship : Weather balloons are used as a practical consequence to the relationship between pressure and volume of a gas. As the weather balloon ascends, the volume increases. As the weather balloon gets further from the earth’s surface, the atmospheric pressure decreases. Boyle’s Law: the volume of a fixed quantity of gas is inversely proportional to its pressure. Boyle used a manometer to carry out the experiment.
Background image of page 12
Boyle’s Law
Background image of page 13

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

View Full DocumentRight Arrow Icon
Mathematically: A plot of V versus P is a hyperbola. Similarly, a plot of V versus 1/P must be a straight line
Background image of page 14
Image of page 15
This is the end of the preview. Sign up to access the rest of the document.

This note was uploaded on 02/20/2011 for the course CHEM 101 taught by Professor John during the Spring '11 term at Caldwell College.

Page1 / 48

chapter 10 Gases - General Chemistry I General Chapter 10...

This preview shows document pages 1 - 15. Sign up to view the full document.

View Full Document Right Arrow Icon
Ask a homework question - tutors are online