Chem Unit7
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The document discusses various topics relating to states of matter and gas laws. It defines the three common states of matter and phase transitions. It also explains the different types of intermolecular forces and how they relate to boiling points. Several gas laws are defined, including Boyle's, Charles', and Gay-Lussac's Laws. The ideal gas law and concepts like molar mass, density, diffusion, and partial pressures are also covered.
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The document discusses various gas laws and their applications, including Boyle's Law, Charles's Law, and Dalton's Law of partial pressures. It explains the physical characteristics of gases, calculations involving gas density, moles, and the ideal gas law (PV=nRT). The document also outlines the kinetic molecular theory of gases and deviations from ideal behavior.23 gases
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Gases are composed of molecules that are far apart from each other and occupy the entire volume of their container. Gas molecules move randomly in straight lines and collide elastically with each other and the container walls. The kinetic molecular theory describes gases as having negligible intermolecular forces and volume. Pressure, volume, temperature of a gas are related by the combined gas law and ideal gas law. Gas calculations involve using stoichiometry, the ideal gas law, and gas laws like Boyle's, Charles', and Gay-Lussac's to determine volume, pressure, amount, or temperature changes.Ideal gas law practice mccpot
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1) The document discusses the ideal gas law (PV=nRT) and its applications in calculating things like moles of gas, volume at different conditions, density, and molar mass.
2) Key variables in the ideal gas law are defined such as pressure (P), volume (V), moles of gas (n), temperature (T), and the gas constant (R).
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The document summarizes key gas laws including Boyle's law, Charles' law, Avogadro's law, Dalton's law of partial pressures, and the ideal gas law. It provides examples of using these laws to calculate volume, pressure, temperature, moles, and mass in gas reactions and mixtures. Key relationships covered are that pressure and volume are inversely related at constant temperature (Boyle's law), volume and temperature are directly related at constant pressure (Charles' law), and volume and moles are directly related at constant temperature and pressure (Avogadro's law).12 Gas Laws
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The document describes several key concepts relating to gases:
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3) Several gas laws are introduced that describe the relationships between pressure, volume, temperature, and number of moles for gases including Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's law, Dalton's law of partial pressures, and the ideal gas law.Lec5 a
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Here are the key steps to solve this problem using Charles' Law:
1) Convert temperatures to Kelvin:
T1 = 297.0 K
T2 = 216.5 K
2) Use the Charles' Law equation:
V1/T1 = V2/T2
3) Solve for V2:
V2 = V1 * T2/T1
= 20.0 L * 216.5 K/297.0 K
= 14.6 L
So the volume outside at -70属F would be 14.6 L.Gas law
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- Kinetic molecular theory explains gas properties in terms of the high-speed motion and infrequent collisions of molecules separated by large distances.Gases
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- Gas laws including Boyle's, Charles', Gay-Lussac's, Avogadro's, and the ideal gas law.
- Conditions of STP and using gas laws to perform stoichiometric calculations.
- The kinetic molecular theory which explains gas properties in terms of particle motion.
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Here are the key steps to solve this problem using Charles' Law:
1) Convert temperatures to Kelvin:
T1 = 297.0 K
T2 = 216.5 K
2) Use the Charles' Law equation:
V1/T1 = V2/T2
3) Solve for V2:
V2 = V1 * T2/T1
= 20.0 L * 216.5 K/297.0 K
= 14.6 L
So the volume outside at -70属F would be 14.6 L.Gas law
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2. For each question there are 4 possible answers labeled a-d. The correct answers are not provided.
3. The questions are intended to test understanding of fundamental thermodynamic concepts and calculations involving things like heat, work, internal energy, and state functions.Ch 14 Ideal Gas Law & Kinetic Theory
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The document contains multiple choice questions about gas laws, kinetic molecular theory, and properties of gases.
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2) Other questions relate to concepts like effusion rates, van der Waals constants, and the relationship between temperature, pressure, volume, and number of gas molecules.
3) Graphs and diagrams are included that must be interpreted in the context of gas behavior and equations of state.The Ideal Gas Law
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The document discusses the ideal gas law PV=nRT and its application to real gases. It defines the four variables in the equation, describes how the ideal gas law relates these variables, and explains how to derive the gas constant R. While real gases deviate from ideal behavior, the ideal gas law can still adequately describe gases at low pressures and temperatures near room conditions. Two examples are given applying the law to calculate pressure and temperature for gas samples.Chem unit 12 presentation
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Chemistry and gases are intimately related. Many of the most important discoveries and applications in chemistry involve gases. Historically, scientists like Robert Boyle, Jacques Charles, and Joseph Gay-Lussac made seminal discoveries about gas behavior through careful experimentation. Their gas laws laid the foundation for understanding the properties and interactions of gases.
One area where gases play a huge role is in industry and energy. The Haber process converts nitrogen gas and hydrogen gas into ammonia, a key component of fertilizers that have enabled the growth of the global population. Natural gas, composed primarily of methane, heats homes and fuels power plants around the world. Greenhouse gases like carbon dioxideGas laws
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The document discusses gas laws and properties of gases. It provides examples of problems involving Boyle's law, Charles' law, Gay-Lussac's law, combined gas law, and the ideal gas law. It also discusses Avogadro's law and the kinetic molecular theory of gases. Examples include calculating gas pressures, volumes, temperatures, and moles of gas under varying conditions.Similar to Chem Unit7 (20)
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- Real gases deviate from ideal gas behavior due to intermolecular forces and molecular size. The van der Waals equation accounts for these factors.
- Kinetic molecular theory explains gas properties in terms of the high-speed motion and infrequent collisions of molecules separated by large distances.Gases
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The document discusses the properties and behavior of gases, liquids, and solids from a microscopic perspective. It explains that gases have particles with empty space between them allowing the particles to move freely, while liquids have particles close together allowing them to flow but slide past one another, and solids have particles locked in a fixed structure. The document also covers gas laws, phase changes, types of solids based on bonding, and heating curves. It provides a concise overview of the states of matter and changes between states from a molecular level.Gases
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This document provides an overview of key concepts related to gases, including:
- The properties of ideal gases and units of pressure like pascals and atmospheres.
- Gas laws including Boyle's, Charles', Gay-Lussac's, Avogadro's, and the ideal gas law.
- Conditions of STP and using gas laws to perform stoichiometric calculations.
- The kinetic molecular theory which explains gas properties in terms of particle motion.
- How real gases differ from ideal gases due to intermolecular forces.Chapter 5 notes
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1) When a hot air balloon is heated, some of the air escapes from the top, lowering the density inside and making the balloon buoyant.
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The document discusses kinetic molecular theory and the gas laws. It explains that kinetic molecular theory views gases as made of particles in constant, random motion that explains gas properties like pressure and temperature. The gas laws described are Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's law, Dalton's law of partial pressures, and the combined and ideal gas laws. Key concepts are that gas pressure, volume, and temperature are directly or inversely proportional based on these laws. Standard temperature and pressure are defined, and gas calculations can be done using the various gas laws and stoichiometry.Chapter_5_Gases.ppt
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Boyle's law states that at a constant temperature, the pressure and volume of a gas are inversely proportional. The product of pressure and volume remains constant. Charles's law describes how the volume of a gas increases as temperature increases at constant pressure. Gay-Lussac's law relates pressure and temperature at constant volume. The combined gas law incorporates these relationships. The ideal gas law (PV=nRT) relates pressure, volume, amount of gas, and temperature. Real gases deviate from ideal behavior at low temperatures or high pressures due to intermolecular forces and molecular size.Adv chem chapt 5
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The document discusses key concepts from gas chemistry including the composition and properties of the atmosphere, gas laws such as Boyle's, Charles', and Avogadro's laws, kinetic molecular theory, and concepts such as molar volume, partial pressures, and gas stoichiometry. It provides examples of calculations using the ideal gas law to determine quantities such as moles of gas, volume, pressure, and temperature changes.Ad
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Chem Unit7
- 1. States of Matter Particle vibration fluid motion rapid, random motion Rigid positions move past independent of each other each other Fixed volume fixed volume volume of container
- 2. Phases and Transitions Sublimation Condensation Evaporation Melting Freezing
- 3. Intermolecular Forces Strongest = IONIC FORCES High melting points Oppositely charged ions
- 4. Dipole-Dipole Forces Dipole: contains both positively and negatively charged regions:
- 5. Hydrogen Bonding Special case of dipole-dipole forces Causes water to have higher than expected boiling point
- 6. Water Properties Surface tension
- 7. Water Properties Capillary action
- 8. Boiling Points Molecule Boiling Point H 2 O 100属C H 2 S 60.7 属C H 2 Se 41属C H 2 Te 2属C
- 9. Hydrogen Bonding Weak bond between H and electronegative atom: Recall
- 10. Hydrogen Bonding
- 13. London (Dispersion) Forces Weak attractions between non-polar Increases with size of molecule (number of electrons) Molecular Shape (less compact > compact) > >
- 14. London (Dispersion) Forces Weak attractions between non-polar Temporary or instantaneous dipoles
- 15. Intermolecular Forces IONIC >> Dipole Dipole >> London
- 16. Intermolecular Forces Which intermolecular force is expected? CH 4
- 17. Intermolecular Forces Which intermolecular force is expected? CH 4 Non-polar covalent molecule London (dispersion) forces
- 18. Intermolecular Forces Which intermolecular force is expected? Butanol CH 3 CH 2 CH 2 CH 2 OH
- 19. Intermolecular Forces Which intermolecular force is expected? Butanol CH 3 CH 2 CH 2 CH 2 OH Dipole-Dipole
- 20. Energy of Phase Changes Energy is required for all phase changes
- 21. Phase Diagram (H 2 O)
- 22. Phase Diagram (CO 2 ) Triple Point Triple Point: where all three phases co-exist (T, p)
- 24. Properties of Matter Force Pressure = area h = 760 mm = 1 atm Torricelli barometer
- 25. Robert Boyle
- 26. Boyles Law For a gas at constant T and n V and p are inversely proportional pV = constant
- 27. Charles Law At constant pressure, V/T = constant
- 28. Charles Law
- 29. Gay Lussacs Law In a constant volume: P/T = constant
- 30. Gay-Lussacs Law
- 31. Combined Gas Law Boyles Law pV = constant Charles Law V/T = constant Gay-Lussacs Law p/T = constant Combining all three: p 1 V 1 p 2 V 2 So: T 1 = T 2
- 32. Combined Gas Law A sample of gas has a volume of 400 liters when its temperature is 20属C and its pressure is 300 mm Hg. What volume will the gas occupy at STP?
- 33. Combined Gas Law p 1 V 1 p 2 V 2 T 1 = T 2 T in Kelvin (300/760 mm Hg)(400 L) = (760 mm Hg) (V 2 ) (293 K) (273 K) V 2 = 147 Liters
- 34. Combined Gas Law A sample of He gas has a volume of 250 mL at 456 torr and 25属C. At what temperature does this gas have a volume of 150 mL and 561 torr? p 1 V 1 p 2 V 2 T 1 = T 2
- 35. Combined Gas Law A sample of He gas has a volume of 250 mL at 456 torr and 25属C. At what temperature does this gas have a volume of 150 mL and 561 torr? p 1 V 1 p 2 V 2 T 2 = p 2 V 2 T 1 T 1 = T 2 p 1 V 1
- 36. Combined Gas Law A sample of He gas has a volume of 250 mL at 456 torr and 25属C. At what temperature does this gas have a volume of 150 mL and 561 torr? p 1 V 1 p 2 V 2 (561/760)(0.15L)(298K) T 1 = T 2 T 2 = (456/760)(0.25L) = 220 K = -53属C
- 37. Ideal Gases Non-interacting Point particles Randomly moving with elastic collisions (no energy lost)
- 38. Ideal Gases Avogadros Law: Equal volumes of gas contain the same number of molecules at the same T & p. n = number of moles p 1 V 1 = constant n T 1
- 39. Ideal Gas Law p 1 V 1 = constant = 0.082 L atm = R n T 1 K mole = Universal Gas Constant One mole of gas at STP : Volume = nRT/p = (1 mole)(0.082 Latm)(273K)/1 atm = 22.4 Liters
- 40. Ideal Gas Law pV = nRT How many moles of Helium are present in a balloon that has a volume of 65 L at 20属 C and 705 torr? Given Needed V, T, p, R n n = pV/RT
- 41. Ideal Gas Law pV = nRT How many moles of Helium are present in a balloon that has a volume of 65 L at 20属 C and 705 torr? n = pV/RT = (705/760 atm)(65 L) (0.082 Latm/K)(293) = 2.5 moles He
- 42. Ideal Gas 6.2 liters of an ideal gas are contained at 3.0 atm and 37 属C. How many moles of this gas are present?
- 43. Ideal Gas 6.2 liters of an ideal gas are contained at 3.0 atm and 37 属C. How many moles of this gas are present? n = pV/RT = (3 atm)(6.2 L) (0.082 L atm/mole K ) (310 K) = 0.73 moles
- 44. Ideal Gases and Density
- 45. Density Gas density increases with molecular mass.
- 46. Density What is the density of NO 2 gas at 0.97 atm and 35属C? MW = 46 g/mole Molar mass p (46 g/mole)(0.97 atm) Density = RT (0.082 L atm/mole K) (308 K) = 1.767 g/L
- 47. Gas Diffusion Movement of particles from region of Higher density to lower density
- 48. Gas Diffusion Movement of particles from region of Higher density to lower density Depends on density (molar mass)
- 49. Grahams Law proportionality Rate of effusion inversely to square root of molar mass Smaller molecules escape FASTER than larger molecules
- 50. Daltons Law PT = P1 + P2 + P3 + . . . . Total pressure of a gas sample is the sun of the partial pressures.
- 51. Daltons Law A mixture of O 2 , CO 2 and N 2 has a p T of 0.97 atm; if p O2 = 0.7 atm and p N2 = 0.12 atm, what is p CO2 ?
- 52. Daltons Law A mixture of O 2 , CO 2 and N 2 has a p T of 0.97 atm; if p O2 = 0.7 atm and p N2 = 0.12 atm, what is p CO2 ? pT = p O2 + p N2 + p CO2 = 0.97 atm p CO2 = 0.97 atm - (0.7 atm + 0.12 atm) = 0.15 atm
- 53. Daltons Law The partial pressures of CH 4 and O 2 are 0.175 atm and 0.25 atm. At 65属C in a volume of 2 L, how many moles of each gas are present?
- 54. Daltons Law The partial pressures of CH 4 and O 2 are 0.175 atm and 0.25 atm. At 65属C in a volume of 2 L, how many moles of each gas are present? n CH4 = pV/RT = 0.175 atm (2L)/0.082 L atm/mole K (338 K = 0.126 moles n O2 = pV/RT = 0.25 atm (2L)/ 0.082 L atm/mole K (338 K) = 0.018 moles
- 55. Unit 7 Review Phases of Matter and Transitions Intermolecular Forces Phase Diagrams Boyles, Charles, Gay Lussacs Laws Ideal Gas Law pV = nRT Grahams Law of Diffusion Partial Pressure