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Chapter 14 Notes Part I. Boyle’s, Charles’ and Gay-Lussac’s Laws Combined Gas Laws. Gas Review. In chapter 13 gases were said to be mostly empty space . This gives rise to a property called compressibility . The particles in a gas can be forced closer together. Kinetic Theory.
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Chapter 14 Notes Part I Boyle’s, Charles’ and Gay-Lussac’s Laws Combined Gas Laws
In chapter 13 gases were said to be mostly empty space. • This gives rise to a property called compressibility. • The particles in a gas can be forced closer together.
Kinetic Theory • Kinetic Energy—Energy that an object has due to motion. • The Kinetic Theory states that tiny particles form all matter, and they are constantly in motion.
Gases A gas is composed of particles that are small, hard spheres with almost no volume or particle interaction.
Gases Particles in a gas are in constant motion—they travel straight paths unless they collide with another particle or their container.
Gases All collisions are considered elastic—no energy is lost
Temperature When a substance is heated, the particles speed up, causing faster movement and more collisions. This is a rise in temperature.
Obj. 1…Ideal vs. real gases • behavior of ‘ideal gases’ (from kinetic theory)… inverse ~ ______ relationship b/n P and V. direct ~ ______ relationship b/n T and V. direct ~ ______ relationship b/n T and P. • however, there are no ‘ideal’ gases in existence. • two properties keep ‘real’ gases from being ‘ideal’… ~ real gas particles have distinct volumes …there comes a point where V can not get smaller, no matter how much P is applied ~ real gas particles are slightly attracted to each other… intermolecular attraction of gas molecules causes gases to occupy less space than assumed by the KT.
Obj. 2-3…STP • STP = standard temperature and pressure • standard temp = ~ 0°C ~ 273 K ** • standard pressure = ~ 1 atm ~ 101.3 kPa ~ 760 mmHg
There are three relationships between the conditions a gas is in that will be affected by this property. • Pressure and volume • Volume and temperature • Pressure and temperature
Boyles Law states that as the volume of a gas is decreased, the amount of pressure is increased at constant temperature. • (P#V$ or P$V#) • Mathematically, P1V1=P2V2
Obj. 4-6…Boyle’s Law • relationship b/n P and V is expressed in the Boyle’s Law equation. ~ inverse relationship ~ only works if T remains constant! p1v1 = p2v2 • Ex… V1 P1 • The pressure on 2.5 L of a gas decreases from 105 kPa to 40.5 kPa. What is the new volume of the gas? V2 P2 105(2.5) = 40.5(x) 262.5 = 40.5(x) 6.5 liters 40.5 40.5
Why? • With less volume, there is greater frequency of the same amount of particles hitting the surface of the container.
Charles Law states that as the temperature of a gas is increased, the volume is also increased at constant pressure. • (V#T# or V$T$) • Mathematically: V1 = V2 T1 T2
Obj. 7-9…Charles’s Law • relationship b/n T and V is expressed in the Charles’ Law equation. ~ direct relationship ~ only works if P remains constant! ~ temp. MUST be in Kelvin!!! (°C + 273) v1 = v2 T1 T2 • Ex… V1 T1 = 398 K • If a sample of gas occupies 6.8 L at 125°C, what will its volume be at 38°C if pressure remains constant? V2 T2 = 311 K x 6.8 6.8 (311) = x 5.3 liters = 398 398 311
Why? • As the temperature increases, the average kinetic energy of the particles increases. • This increases the amount of volume needed to maintain the same frequency of collision with the surface of the container.
Meanwhile... • Jaques Charles also noticed that no matter what gas he experimented with, when he extrapolated the volume down on a graph, the temperature was the same: -273oC!
Kelvin • William Thomson (a.k.a. Lord Kelvin) recognized this as the theoretical point at which the average kinetic energy of all substances would be zero. • Thus, the concept of absolute zero and the Kelvin scale were born!
When comparing temperatures during this chapter, they must be in Kelvin, because Celsius is a degreed scale and Kelvin is an absolute scale!
Gay-Lussac’s Law states that as you increase temperature of an amount of gas, its pressure will increase if at a constant volume. • (P#T# or P$T$) • Mathematically: P1 = P2 T1 T2
Obj. 10-12…Gay-Lussac’s Law • relationship b/n T and P is expressed in the Gay-Lussac’s Law equation. ~ direct relationship ~ only works if V remains constant! ~ temp. MUST be in Kelvin!!! (°C + 273) P1 = P2 T1 T2 • Ex… P1 T1 • A sample of gas has a pressure of 6.58 kPa at 339 K. What will the temperature be at 4.21 kPa? P2 T2 6.58 339 (4.21) 4.21 = x 217 K = x 339 6.58
Why? • As the temperature increases, the average kinetic energy of the particles increases, thus they move faster. • This increases the frequency of collisions, as well as the amount of force in each collision.
But wait a minute... NO! There’s a handy, dandy equation that will show you ALL these equations in one! Are you saying that I have to keep ALL these equations straight in my head?
Combined Gas Laws P1V1P2V2 T1 T2 =
When one variable is constant, you can just cross it out, and the equation works for all three laws, as well as for combined problems!
Practice Problem #1 • The pressure on 2.5L of anesthetic gas changes from 105 kPa to 40.5 kPa. What will the new volume be if the temperature is constant?
Practice Problem #2 • A balloon has a volume of 6.7L at 20oC. What will its volume be at 350oC if it is at constant pressure?
Practice Problem #3 • The pressure in an automobile tire that has a constant volume is 198 kPa at 27oC. On a hot sunny day the pressure has risen to 225 kPa. What is the temperature?
Practice Problem #4 • A gas at 155 kPa and 25oC occupies a container with an initial volume of 1.00L. By changing the volume the pressure of the gas increases to 605 kPa as the temperature is raised to 125oC. What is the new volume?
