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AP Chemistry “The Behavior of Gases” Effusion and Diffusion Root Mean Speed Average Kinetic Energy.

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Presentation on theme: "AP Chemistry “The Behavior of Gases” Effusion and Diffusion Root Mean Speed Average Kinetic Energy."— Presentation transcript:

1 AP Chemistry “The Behavior of Gases” Effusion and Diffusion Root Mean Speed Average Kinetic Energy

2 Diffusion is: Effusion: Gas escaping through a tiny hole in a container. Both of these depend on the molar mass of the particle, which determines the speed. u Molecules moving from areas of high concentration to low concentration. u Example: perfume molecules spreading across the room.

3 Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing. Molecules move from areas of high concentration to low concentration.

4 Effusion: a gas escapes through a tiny hole in its container -Think of a nail in your car tire… Diffusion and effusion are explained by the next gas law: Graham’s

5 Graham’s Law The rate of effusion and diffusion is inversely proportional to the square root of the molar mass of the molecules. Derived from: Kinetic energy = 1/2 mv 2 m = the molar mass, and v = the velocity. Rate A  Mass B Rate B  Mass A =

6 Comparing distance traveled You can compare the distanced traveled by 2 gases in the same amount of time using this equation also. Distance traveled by A =  MassB Distance traveled by B  MassA

7 Sample: compare rates of effusion of Helium with Nitrogen – With effusion and diffusion, the type of particle is important: Gases of lower molar mass diffuse and effuse faster than gases of higher molar mass. Helium effuses and diffuses faster than nitrogen – thus, helium escapes from a balloon quicker than many other gases! Graham’s Law

8 How much faster does methane (CH 4 ) effuse than propane (C 3 H 8 )? Determine molar masses of each gas Determine molar masses of each gas CH 4 = g/mol CH 4 = g/mol C 3 H 8 = g/mol Plug into formula Plug into formula Rate CH4 M C3H8 Rate CH4  M C3H8 Rate C3H8 M CH4 Rate C3H8  M CH4 = = 1.65 =  =  This means that methane diffuses 1.65 times faster than propane gas This means that methane diffuses 1.65 times faster than propane gas

9 Graham’s Law of Effusion Examples 1) A compound effuses through a porous cylinder 1.41 times faster than helium. What is it’s molar mass? Rate Gas x = √He Rate He √X 1.41 = √4 √x 1.41 (√x ) = 2 √x = 2/1.41 X = (1.41) 2 = 2.01 g/mole = Hydrogen (H 2 )

10 If mol of NH 3 effuse through a hole in 2.47 min, how much HCl would effuse in the same time? If mol of NH 3 effuse through a hole in 2.47 min, how much HCl would effuse in the same time? Assuming the time is the same, we can use the following relationship with Graham’s Law Moles NH 3 = √M HCl Moles HCL √M NH = √36.45 Moles HCl √ = Moles HCl Moles HCl = Moles

11 A sample of N 2 effuses through a hole in 38 seconds. what must be the molecular weight of gas that effuses in 55 seconds under identical conditions? A sample of N 2 effuses through a hole in 38 seconds. what must be the molecular weight of gas that effuses in 55 seconds under identical conditions? Moles / 55sec = √ M N2 Moles / 38sec √Mgas 38 = √28 55 √Mgas Mgas = 58.5 g/mol

12 Molecular Speeds and Average Kinetic Energy The Kelvin temperature scale is a measurement of the average kinetic energy of gas particles. The Kelvin temperature scale is a measurement of the average kinetic energy of gas particles. KE = ½ mv 2 KE = ½ mv 2 As kinetic energy increases, then the temperature increases, and molecules move faster. As kinetic energy increases, then the temperature increases, and molecules move faster. KE avg = 3 RT KE avg = 3 RT 2 Where = J/Kelvin Mole This formula represents the average energy of the particles at a given temperature. This formula represents the average energy of the particles at a given temperature.

13 Maxwell Speed Distribution Curve Peaks represent the average speeds Remember, some are moving faster and some slower at the same temperature! Peak moves to greater speed with higher temps. Curve flattens due to more molecules moving at greater speeds.

14 Root Mean Square Speed (or Velocity) rms or μ rms (Units are meters/sec) rms or μ rms (Units are meters/sec) Estimates the average molecular speed based on molecular mass and temperature. Μ rms = √3RT Μ rms = √3RT √M √M M = Molar Mass in kg/mole M = Molar Mass in kg/mole R = J/K Mol T = Temperature in Kelvin

15 This Formula relates the difference in speed (not kinetic energy!) to the molar mass of the gas. This Formula relates the difference in speed (not kinetic energy!) to the molar mass of the gas. Maxwell Speed Distribution Curve Maxwell Speed Distribution Curve Oxygen (O 2 ) Helium Hydrogen (H 2 ) These are speed distribution curves for 3 different gases a the same temperature Shows that lighter molecules (like hydrogen) move faster on average than heavier ones (like oxygen)

16 Big Points to Remember: All gases at the same temperature have the same average kinetic energy. All gases at the same temperature have the same average kinetic energy. But, they do not have the same average velocity (or speed!) But, they do not have the same average velocity (or speed!) Speed depends on Molar Mass (root mean square speed!) Speed depends on Molar Mass (root mean square speed!) The heavier the gas, the slower it moves! The heavier the gas, the slower it moves! The lighter the gas, the faster it moves! The lighter the gas, the faster it moves!


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