Ideal Gas Molecules
Übersicht
Every breath you take pushes back against the atmosphere, and every tyre on the road stays inflated because billions of tiny molecules slam into its inner walls each second. Gas behaviour connects the invisible world of molecules to measurable quantities like pressure, volume and temperature.
In this lesson you will explore how gas molecules create pressure, why there is a lowest possible temperature, and how to convert between the Celsius and Kelvin scales. You will then learn Boyle's law and the pressure law, practising the calculations that Edexcel tests on Papers 1 and 2.
Ziele
- Explain how molecules in a gas have random motion and that they exert a force, and hence a pressure, on the walls of a container
- Understand why there is an absolute zero of temperature, which is -273 C
- Describe the Kelvin scale of temperature and be able to convert between the Kelvin and Celsius scales
- Understand why an increase in temperature results in an increase in the average speed of gas molecules
- Know that the Kelvin temperature of a gas is proportional to the average kinetic energy of its molecules
- Explain, for a fixed amount of gas, the qualitative relationship between pressure and volume at constant temperature, and between pressure and Kelvin temperature at constant volume
- Use the relationship between the pressure and Kelvin temperature of a fixed mass of gas at constant volume: p1/T1 = p2/T2
- Use the relationship between the pressure and volume of a fixed mass of gas at constant temperature: p1V1 = p2V2
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- What is the temperature of absolute zero on the Celsius scale? A) 0 degrees Celsius B) -100 degrees Celsius C) -273 degrees Celsius D) -373 degrees Celsius Answer: C
- A fixed mass of gas is compressed at constant temperature. What happens to the pressure? A) It stays the same B) It decreases C) It increases D) It drops to zero Answer: C
- Which temperature is equivalent to 373 K? A) 373 degrees Celsius B) 100 degrees Celsius C) 0 degrees Celsius D) -100 degrees Celsius Answer: B
- A sealed container of gas is heated at constant volume. What happens to the gas molecules? A) They move faster and collide with the walls more often B) They slow down and exert less pressure C) They expand and increase in size D) They stop moving Answer: A
- A gas has a volume of 200 cm3 at a pressure of 100 kPa. If the pressure is doubled at constant temperature, what is the new volume? A) 400 cm3 B) 200 cm3 C) 100 cm3 D) 50 cm3 Answer: C
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Lehrbuchabschnitt
Kinetic Theory: Atomic and Molecular Explanation of Pressure and Temperature
We have developed macroscopic definitions of pressure and temperature. Pressure is the force divided by the area on which the force is exerted, and temperature is measured with a thermometer. We gain a better understanding of pressure and temperature from the kinetic theory of gases, which assumes t
"College Physics: Kinetic Theory: Atomic and Molecular Explanation of Pressure and Temperature" by OpenStax, OpenStax, Rice University, licensed under CC BY 4.0 (https://creativecommons.org/licenses/by/4.0/). Source: https://openstax.org/books/college-physics/pages/13-4-kinetic-theory-atomic-and-molecular-explanation-of-pressure-and-temperature. Access for free at https://openstax.org/books/college-physics/pages/1-introduction
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Lehrbuchabschnitt
The Ideal Gas Law
In this section, we continue to explore the thermal behavior of gases. In particular, we examine the characteristics of atoms and molecules that compose gases. (Most gases, for example nitrogen, N 2 N 2 size 12{N rSub { size 8{2} } } {} , and oxygen, O 2 O 2 size 12{O rSub { size 8{2} } } {} , are c
"College Physics: The Ideal Gas Law" by OpenStax, OpenStax, Rice University, licensed under CC BY 4.0 (https://creativecommons.org/licenses/by/4.0/). Source: https://openstax.org/books/college-physics/pages/13-3-the-ideal-gas-law. Access for free at https://openstax.org/books/college-physics/pages/1-introduction
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