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Boyle's Law, established by Robert Boyle in 1662, describes the inverse relationship between gas volume and pressure at constant temperature. The document covers essential properties of gases including pressure, volume, and temperature, with standard units and conversion factors provided. Additionally, it includes various theoretical problems and examples demonstrating the application of Boyle's Law in calculating gas behavior under changing conditions.
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BOYLES LAW.pptx
BOYLES LAW.pptxJane360787
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1. The document describes various gases and their properties including pressure, volume, temperature, and mass. It provides definitions and conversion formulas for units of pressure, volume, and temperature.
2. Boyle's law is introduced, which states that the pressure and volume of a gas are inversely proportional at constant temperature. An example problem demonstrates how to use the Boyle's law equation to relate initial and final pressure and volume.
3. The relationship between pressure and volume of a gas is investigated through example problems applying Boyle's law, such as calculating new volume given a change in pressure.Roberts Boyle's Law Principles and explainations
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Robert Boyle studied the relationship between the volume and pressure of gases in 1662. Boyle's Law states that the pressure of a gas is inversely proportional to its volume when temperature is held constant. The document then provides details on the standard units used to measure gas properties like pressure, volume, and temperature. It also presents sample problems demonstrating how to use Boyle's Law to calculate changes in gas volume or pressure when one variable is altered while temperature remains constant.thegaslawscomplete-120227061412-phpapp01.pdf
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- Boyle's law states that the volume of a gas is inversely proportional to its pressure when temperature is kept constant. It describes the relationship between the pressure and volume of a gas.
- Charles' law describes how the volume of a gas changes with temperature. It states that the volume of a gas increases or decreases proportionally with an increase or decrease in its temperature.
- The combined gas law combines Boyle's and Charles' laws and describes the relationship between pressure, volume, and temperature for a gas.Gas laws (Boyle and Charles' Laws) handout
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The document summarizes four gas laws:
1. Boyle's law states that the volume of a gas is inversely proportional to its pressure when temperature is kept constant.
2. Charles' law describes the direct relationship between the volume and temperature of a gas when pressure is constant.
3. Several sample problems demonstrate how to use the formulas for each gas law to calculate volume or pressure given values for two variables.
4. Practice problems provide additional examples for readers to work through the calculations.The gas laws complete
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1) Boyle's law states that the volume of a gas is inversely proportional to its pressure when temperature is kept constant. Charles' law describes the direct relationship between volume and temperature of a gas at constant pressure. Gay-Lussac's law explains that pressure of a gas rises with increasing temperature at constant volume.
2) The combined gas law incorporates Boyle's, Charles's and Gay-Lussac's laws to describe the interrelationships between pressure, volume and temperature for a fixed amount of gas.
3) According to Avogadro's law, equal volumes of gases under same conditions of temperature and pressure contain equal numbers of molecules. Dalton's law states that total pressure of a gas mixture is the sumthe gas laws
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The document discusses several gas laws including Boyle's law, Charles' law, Gay-Lussac's law, Avogadro's law, the combined gas law, and the ideal gas law. It provides definitions of these laws and examples of calculations using each one. The key relationships covered are: the inverse relationship between pressure and volume at constant temperature (Boyle's law), the direct relationship between volume and temperature at constant pressure (Charles' law), the direct relationship between pressure and temperature at constant volume (Gay-Lussac's law), the relationship between volume and amount of gas at constant pressure and temperature (Avogadro's law), and the ideal gas law which relates pressure, volume, temperature,Boyles law module in the grade 10 science
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2. Key concepts covered include the definition of pressure, different pressure units, relationships between pressure and volume, relationships between temperature and volume, and how the number of gas molecules affects volume.
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3. The gas laws describe the macroscopic behavior of gases through relationships between pressure, volume, temperature, and amount of gas. The kinetic molecular theory qualitatively explains the gas laws based on gas particle motion and interactions.Chapter 5 notes
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Here are the densities of the gases at STP:
Hydrogen: 0.0899 g/L or 0.0899 g/m3
Oxygen: 1.429 g/L or 1.429 g/m3
Chlorine: 3.214 g/L or 3.214 g/m3
Radon: 9.73 g/L or 9.73 g/m35,gases
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PCO2
Ptotal = PN2 + PO2 + PCO2
2.50 atm = 0.90 atm + 0.60 atm + PCO2
PCO2 = 2.50 atm - 0.90 atm - 0.60 atm
PCO2 = 1 atm
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- 1. Boyles Law
- 5. Robert Boyle in 1662 studied the relationship between the volume of a gas and its pressure. Boyle varied the pressure and noticed its effect on the volume of the gas, without changing its temperature. He noticed that the volume of the gas decreased as the pressure exerted on it increased. This experience is now known as Boyles Law. Syringes of all types utilize Boyle's law on a very basic level. Experience this phenomenon by performing the
- 6. Measurable Properties of Gases 1. Pressure - the force exerted by the gas on the walls of its container divided by the surface area of the container. The common units of pressure are the following: Pascal (Pa) - standard unit of pressure under System辿 International (SI) which is equivalent to a force of one newton (1N = 1 kg m/s2) acting on an area of one square meter. Atmosphere (atm) Torr Millimeter mercury (mm Hg)
- 7. Pressure can be converted from unit to another using the following conversion: 1 atm = 760 torr = 760 mm Hg 1 torr = 1 mm Hg 1 atm = 101,325 Pa 2. Volume defined as the space occupied. The volume of the gas is equal to the volume of the vessel or container. Common Units of Volume: cubic meter (m3), cubic centimeter (cm3), liter (L) milliliter (mL) 3. Temperature defined as the degree of hotness or coldness. Units: degree Celsius (oC), degree Fahrenheit (oF), Kelvin (K)
- 8. The temperature of a gas together with its atmospheric pressure differ from place to place and from time to time. As the volume of a gas is dependent on its temperature and pressure, it is significant to have a set of standard conditions for these quantities. This set of standard condition is named as standard temperature and pressure or simply STP. The standard temperature is 0 C or 273.15 K and the standard pressure is 1 atm pressure. This is the freezing point of pure water at sea level atmospheric pressure. At STP, one mole of gas occupies 22.4 L of volume.
- 10. B. The SI unit of pressure is the Pascal, Pa, but in the V-P relationship of gases, it is necessary to be familiarized with the different units of pressures and the corresponding values for unit conversion. 1 atm = 760 torr 1 atm = 760 mm Hg 1 atm = 101,325 Pa 1 atm = 76 cm Hg
- 14. Activity 2. Gaze, Compare, and Conclude Suppose we have a theoretical gas confined in a jar with a piston at the top as seen in the illustration below. The left side indicates the initial state while that on the right shows the final state after slowly adding weights to the top of the piston. The unit of volume is in cubic meters (m3), while that of pressure is kilopascal (kPa). The
- 19. Example #1: 2.00 L of a gas is at 740.0 mmHg pressure. What is its volume at standard pressure? Example #2: 5.00 L of a gas is at 1.08 atm. What pressure is obtained when the volume is 10.0 L? Example #3: 9.48 L of a gas was at an unknown pressure. However, at standard pressure, its volume was measured to be 8.00 L. What was the unknown pressure? Example #4: If we have 6.00 cm3 of gas at a pressure of 10.0 N/cm2 and we increase the pressure to 20.0 N/cm2, what volume will the gas occupy? Example #5: What pressure is required to compress 196.0 liters of air at 1.00 atmosphere into a cylinder whose volume is 26.0 liters? Example #6: The volume of a gas is 6.10 L, measured at 1.00 atm. What is the pressure of the gas in mmHg if the volume is changed to 9.74 L? Example #7: At 46.0 属C a sample of ammonia gas exerts a pressure of 5.30 atm. What is the pressure when the volume of the gas is reduced to one-eighth (0.125) of the original value at the same temperature? Example #8: In order to measure the volume of a piece of apparatus, a chemist filled a 750. mL flask with 46.65 kPa pressure of gas, then expanded it into the apparatus. The final pressure was 14.95 kPa. Calculate the total volume occupied by the gas.
- 20. Problem #16: 4.00 L of a gas are under a pressure of 6.00 atm. What is the volume of the gas at 2.00 atm? Problem #17: A gas occupies 25.3 mL at a pressure of 790.5 mmHg. Determine the volume if the pressure is reduced to 0.804 atm. Problem #18: A sample of gas has a volume of 12.0 L and a pressure of 1.00 atm. If the pressure of gas is increased to 2.00 atm, what is the new volume of the gas? Problem #19: A container of oxygen has a volume of 30.0 mL and a pressure of 4.00 atm. If the pressure of the oxygen gas is reduced to 2.00 atm and the temperature is kept constant, what is the new volume of the oxygen gas? Problem #20: A tank of nitrogen has a volume of 14.0 L and a pressure of 760.0 mmHg. Find the volume of the nitrogen when its pressure is changed to 400.0 mmHg while the temperature is held constant. Problem #21: A 40.0 L tank of ammonia has a pressure of 8.00 atm. Calculate the volume of the ammonia if its pressure is changed to 12.0 atm while its temperature remains constant. Problem #22: Two hundred liters of helium at 2.00 atm and 28.0 属C is placed into a tank with an internal pressure of 600.0 kPa. Find the volume of the helium after it is compressed into the tank when the temperature of the tank remains 28.0 属C.
- 22. ASSIGNMENT
- 24. THANK YOU !!!