Gases Ideal Gases Ideal gases are imaginary gases
![Gases Gases](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-1.jpg)
![Ideal Gases Ideal gases are imaginary gases that perfectly fit all of the assumptions Ideal Gases Ideal gases are imaginary gases that perfectly fit all of the assumptions](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-2.jpg)
![Ideal Gases (continued) q Gas particles are in constant, rapid motion. They therefore possess Ideal Gases (continued) q Gas particles are in constant, rapid motion. They therefore possess](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-3.jpg)
![The Nature of Gases q Gases expand to fill their containers q Gases are The Nature of Gases q Gases expand to fill their containers q Gases are](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-4.jpg)
![Pressure q Is caused by the collisions of molecules with the walls of a Pressure q Is caused by the collisions of molecules with the walls of a](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-5.jpg)
![Measuring Pressure The first device for measuring atmospheric pressure was developed by Evangelista Torricelli Measuring Pressure The first device for measuring atmospheric pressure was developed by Evangelista Torricelli](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-6.jpg)
![An Early Barometer The normal pressure due to the atmosphere at sea level can An Early Barometer The normal pressure due to the atmosphere at sea level can](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-7.jpg)
![Standard Temperature and Pressure “STP” • • • P = 1 atmosphere, 760 torr Standard Temperature and Pressure “STP” • • • P = 1 atmosphere, 760 torr](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-8.jpg)
![Converting Celsius to Kelvin Gas law problems involving temperature require that the temperature be Converting Celsius to Kelvin Gas law problems involving temperature require that the temperature be](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-9.jpg)
![The Combined Gas Law The combined gas law expresses the relationship between pressure, volume The Combined Gas Law The combined gas law expresses the relationship between pressure, volume](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-10.jpg)
![Boyle’s Law Pressure is inversely proportional to volume when temperature is held constant. Boyle’s Law Pressure is inversely proportional to volume when temperature is held constant.](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-11.jpg)
![Charles’s Law • The volume of a gas is directly proportional to temperature, and Charles’s Law • The volume of a gas is directly proportional to temperature, and](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-12.jpg)
![Gay Lussac’s Law The pressure and temperature of a gas are directly related, provided Gay Lussac’s Law The pressure and temperature of a gas are directly related, provided](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-13.jpg)
![Avogadro’s Law v For a gas at constant temperature and pressure, the volume is Avogadro’s Law v For a gas at constant temperature and pressure, the volume is](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-14.jpg)
![Ideal Gas Law PV = n. RT v P = pressure in atm v Ideal Gas Law PV = n. RT v P = pressure in atm v](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-15.jpg)
![Standard Molar Volume Equal volumes of all gases at the same temperature and pressure Standard Molar Volume Equal volumes of all gases at the same temperature and pressure](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-16.jpg)
![Gas Density … so at STP… Gas Density … so at STP…](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-17.jpg)
![Density and the Ideal Gas Law Combining the formula for density with the Ideal Density and the Ideal Gas Law Combining the formula for density with the Ideal](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-18.jpg)
![Gas Stoichiometry #1 If reactants and products are at the same conditions of temperature Gas Stoichiometry #1 If reactants and products are at the same conditions of temperature](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-19.jpg)
![Gas Stoichiometry #2 How many liters of ammonia can be produced when 12 liters Gas Stoichiometry #2 How many liters of ammonia can be produced when 12 liters](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-20.jpg)
![Gas Stoichiometry #3 How many liters of oxygen gas, at STP, can be collected Gas Stoichiometry #3 How many liters of oxygen gas, at STP, can be collected](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-21.jpg)
![Gas Stoichiometry #4 How many liters of oxygen gas, at 37. 0 C and Gas Stoichiometry #4 How many liters of oxygen gas, at 37. 0 C and](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-22.jpg)
![Dalton’s Law of Partial Pressures For a mixture of gases in a container, PTotal Dalton’s Law of Partial Pressures For a mixture of gases in a container, PTotal](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-23.jpg)
![Kinetic Energy of Gas Particles At the same conditions of temperature, all gases have Kinetic Energy of Gas Particles At the same conditions of temperature, all gases have](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-24.jpg)
![The Meaning of Temperature q Kelvin temperature is an index of the random motions The Meaning of Temperature q Kelvin temperature is an index of the random motions](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-25.jpg)
![Kinetic Molecular Theory q Particles of matter are ALWAYS in motion q Volume of Kinetic Molecular Theory q Particles of matter are ALWAYS in motion q Volume of](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-26.jpg)
![Diffusion: describes the mixing of gases. The rate of diffusion is the rate of Diffusion: describes the mixing of gases. The rate of diffusion is the rate of](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-27.jpg)
![Effusion: describes the passage of gas into an evacuated chamber. Effusion: describes the passage of gas into an evacuated chamber.](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-28.jpg)
![Graham’s Law Rates of Effusion and Diffusion Effusion: Diffusion: Graham’s Law Rates of Effusion and Diffusion Effusion: Diffusion:](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-29.jpg)
![Real Gases Must correct ideal gas behavior when at high pressure (smaller volume) and Real Gases Must correct ideal gas behavior when at high pressure (smaller volume) and](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-30.jpg)
- Slides: 30
![Gases Gases](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-1.jpg)
Gases
![Ideal Gases Ideal gases are imaginary gases that perfectly fit all of the assumptions Ideal Gases Ideal gases are imaginary gases that perfectly fit all of the assumptions](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-2.jpg)
Ideal Gases Ideal gases are imaginary gases that perfectly fit all of the assumptions of the kinetic molecular theory. Ø Gases consist of tiny particles that are far apart relative to their size. Ø Collisions between gas particles and between particles and the walls of the container are elastic collisions Ø No kinetic energy is lost in elastic collisions
![Ideal Gases continued q Gas particles are in constant rapid motion They therefore possess Ideal Gases (continued) q Gas particles are in constant, rapid motion. They therefore possess](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-3.jpg)
Ideal Gases (continued) q Gas particles are in constant, rapid motion. They therefore possess kinetic energy, the energy of motion q There are no forces of attraction between gas particles q The average kinetic energy of gas particles depends on temperature, not on the identity of the particle.
![The Nature of Gases q Gases expand to fill their containers q Gases are The Nature of Gases q Gases expand to fill their containers q Gases are](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-4.jpg)
The Nature of Gases q Gases expand to fill their containers q Gases are fluid – they flow q Gases have low density q 1/1000 the density of the equivalent liquid or solid q Gases are compressible q Gases effuse and diffuse
![Pressure q Is caused by the collisions of molecules with the walls of a Pressure q Is caused by the collisions of molecules with the walls of a](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-5.jpg)
Pressure q Is caused by the collisions of molecules with the walls of a container q is equal to force/unit area q SI units = Newton/meter 2 = 1 Pascal (Pa) q 1 atmosphere = 101, 325 Pa q 1 atmosphere = 1 atm = 760 mm Hg = 760 torr
![Measuring Pressure The first device for measuring atmospheric pressure was developed by Evangelista Torricelli Measuring Pressure The first device for measuring atmospheric pressure was developed by Evangelista Torricelli](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-6.jpg)
Measuring Pressure The first device for measuring atmospheric pressure was developed by Evangelista Torricelli during the 17 th century. The device was called a “barometer” Baro = weight Meter = measure
![An Early Barometer The normal pressure due to the atmosphere at sea level can An Early Barometer The normal pressure due to the atmosphere at sea level can](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-7.jpg)
An Early Barometer The normal pressure due to the atmosphere at sea level can support a column of mercury that is 760 mm high.
![Standard Temperature and Pressure STP P 1 atmosphere 760 torr Standard Temperature and Pressure “STP” • • • P = 1 atmosphere, 760 torr](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-8.jpg)
Standard Temperature and Pressure “STP” • • • P = 1 atmosphere, 760 torr T = 0 C, 273 Kelvins The molar volume of an ideal gas is 22. 42 liters at STP
![Converting Celsius to Kelvin Gas law problems involving temperature require that the temperature be Converting Celsius to Kelvin Gas law problems involving temperature require that the temperature be](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-9.jpg)
Converting Celsius to Kelvin Gas law problems involving temperature require that the temperature be in KELVINS! Kelvins = C + 273 °C = Kelvins - 273
![The Combined Gas Law The combined gas law expresses the relationship between pressure volume The Combined Gas Law The combined gas law expresses the relationship between pressure, volume](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-10.jpg)
The Combined Gas Law The combined gas law expresses the relationship between pressure, volume and temperature of a fixed amount of gas. Boyle’s law, Gay-Lussac’s law, and Charles’ law are all derived from this by holding a variable constant.
![Boyles Law Pressure is inversely proportional to volume when temperature is held constant Boyle’s Law Pressure is inversely proportional to volume when temperature is held constant.](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-11.jpg)
Boyle’s Law Pressure is inversely proportional to volume when temperature is held constant.
![Charless Law The volume of a gas is directly proportional to temperature and Charles’s Law • The volume of a gas is directly proportional to temperature, and](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-12.jpg)
Charles’s Law • The volume of a gas is directly proportional to temperature, and extrapolates to zero at zero Kelvin. (P = constant)
![Gay Lussacs Law The pressure and temperature of a gas are directly related provided Gay Lussac’s Law The pressure and temperature of a gas are directly related, provided](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-13.jpg)
Gay Lussac’s Law The pressure and temperature of a gas are directly related, provided that the volume remains constant.
![Avogadros Law v For a gas at constant temperature and pressure the volume is Avogadro’s Law v For a gas at constant temperature and pressure, the volume is](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-14.jpg)
Avogadro’s Law v For a gas at constant temperature and pressure, the volume is directly proportional to the number of moles of gas (at low pressures). V = an a = proportionality constant V = volume of the gas n = number of moles of gas
![Ideal Gas Law PV n RT v P pressure in atm v Ideal Gas Law PV = n. RT v P = pressure in atm v](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-15.jpg)
Ideal Gas Law PV = n. RT v P = pressure in atm v V = volume in liters v n = moles v R = proportionality constant v= 0. 08206 L atm/ mol·K v T = temperature in Kelvins Holds closely at P < 1 atm
![Standard Molar Volume Equal volumes of all gases at the same temperature and pressure Standard Molar Volume Equal volumes of all gases at the same temperature and pressure](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-16.jpg)
Standard Molar Volume Equal volumes of all gases at the same temperature and pressure contain the same number of molecules. - Amedeo Avogadro
![Gas Density so at STP Gas Density … so at STP…](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-17.jpg)
Gas Density … so at STP…
![Density and the Ideal Gas Law Combining the formula for density with the Ideal Density and the Ideal Gas Law Combining the formula for density with the Ideal](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-18.jpg)
Density and the Ideal Gas Law Combining the formula for density with the Ideal Gas law, substituting and rearranging algebraically: M = Molar Mass P = Pressure R = Gas Constant T = Temperature in Kelvins
![Gas Stoichiometry 1 If reactants and products are at the same conditions of temperature Gas Stoichiometry #1 If reactants and products are at the same conditions of temperature](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-19.jpg)
Gas Stoichiometry #1 If reactants and products are at the same conditions of temperature and pressure, then mole ratios of gases are also volume ratios. 3 H 2(g) + N 2(g) 2 NH 3(g) 3 moles H 2 + 1 mole N 2 2 moles NH 3 3 liters H 2 + 1 liter N 2 2 liters NH 3
![Gas Stoichiometry 2 How many liters of ammonia can be produced when 12 liters Gas Stoichiometry #2 How many liters of ammonia can be produced when 12 liters](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-20.jpg)
Gas Stoichiometry #2 How many liters of ammonia can be produced when 12 liters of hydrogen react with an excess of nitrogen? 3 H 2(g) + 12 L H 2 N 2(g) 2 L NH 3 3 L H 2 2 NH 3(g) = 8. 0 L NH 3
![Gas Stoichiometry 3 How many liters of oxygen gas at STP can be collected Gas Stoichiometry #3 How many liters of oxygen gas, at STP, can be collected](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-21.jpg)
Gas Stoichiometry #3 How many liters of oxygen gas, at STP, can be collected from the complete decomposition of 50. 0 grams of potassium chlorate? 2 KCl. O 3(s) 2 KCl(s) + 3 O 2(g) 50. 0 g KCl. O 3 1 mol KCl. O 3 122. 55 g KCl. O 3 3 mol O 2 22. 4 L O 2 2 mol KCl. O 3 1 mol O 2 = 13. 7 L O 2
![Gas Stoichiometry 4 How many liters of oxygen gas at 37 0 C and Gas Stoichiometry #4 How many liters of oxygen gas, at 37. 0 C and](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-22.jpg)
Gas Stoichiometry #4 How many liters of oxygen gas, at 37. 0 C and 0. 930 atmospheres, can be collected from the complete decomposition of 50. 0 grams of potassium chlorate? 2 KCl. O 3(s) 2 KCl(s) + 3 O 2(g) 50. 0 g KCl. O 3 1 mol KCl. O 3 122. 55 g KCl. O 3 3 mol O 2 2 mol KCl. O 3 = “n” 0. 612 mol O 2 = 16. 7 L
![Daltons Law of Partial Pressures For a mixture of gases in a container PTotal Dalton’s Law of Partial Pressures For a mixture of gases in a container, PTotal](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-23.jpg)
Dalton’s Law of Partial Pressures For a mixture of gases in a container, PTotal = P 1 + P 2 + P 3 +. . . This is particularly useful in calculating the pressure of gases collected over water.
![Kinetic Energy of Gas Particles At the same conditions of temperature all gases have Kinetic Energy of Gas Particles At the same conditions of temperature, all gases have](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-24.jpg)
Kinetic Energy of Gas Particles At the same conditions of temperature, all gases have the same average kinetic energy.
![The Meaning of Temperature q Kelvin temperature is an index of the random motions The Meaning of Temperature q Kelvin temperature is an index of the random motions](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-25.jpg)
The Meaning of Temperature q Kelvin temperature is an index of the random motions of gas particles (higher T means greater motion. )
![Kinetic Molecular Theory q Particles of matter are ALWAYS in motion q Volume of Kinetic Molecular Theory q Particles of matter are ALWAYS in motion q Volume of](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-26.jpg)
Kinetic Molecular Theory q Particles of matter are ALWAYS in motion q Volume of individual particles is zero. q Collisions of particles with container walls cause pressure exerted by gas. q Particles exert no forces on each other. q Average kinetic energy µ Kelvin temperature of a gas.
![Diffusion describes the mixing of gases The rate of diffusion is the rate of Diffusion: describes the mixing of gases. The rate of diffusion is the rate of](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-27.jpg)
Diffusion: describes the mixing of gases. The rate of diffusion is the rate of gas mixing.
![Effusion describes the passage of gas into an evacuated chamber Effusion: describes the passage of gas into an evacuated chamber.](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-28.jpg)
Effusion: describes the passage of gas into an evacuated chamber.
![Grahams Law Rates of Effusion and Diffusion Effusion Diffusion Graham’s Law Rates of Effusion and Diffusion Effusion: Diffusion:](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-29.jpg)
Graham’s Law Rates of Effusion and Diffusion Effusion: Diffusion:
![Real Gases Must correct ideal gas behavior when at high pressure smaller volume and Real Gases Must correct ideal gas behavior when at high pressure (smaller volume) and](https://slidetodoc.com/presentation_image_h/c136497b4d19a5f6b0fb3123ab7e02bd/image-30.jpg)
Real Gases Must correct ideal gas behavior when at high pressure (smaller volume) and low temperature (attractive forces become important). corrected pressure Pideal corrected volume Videal
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