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Unraveling the Gas Laws: Boyle and Charles Explained

Delve into the fascinating world of gas laws with Robert Boyle and Jacques Charles. Understand how pressure, volume, and temperature interplay in gas behavior. Explore Boyle's Law and Charles's Law, grasping the inverse and direct relationships between gas properties. Witness the impact of force, area, and temperature on gas behavior in various scenarios. Elevate your knowledge on gas physics and apply these principles to practical situations. Discover the wonders of gas science through the intriguing stories of Boyle and Charles.

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Unraveling the Gas Laws: Boyle and Charles Explained

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  1. What’s up with GAS?

  2. Has this ever happened to you?

  3. HA HA HA HA HA HA HA HA!

  4. Have you ever wondered about the science behind such wondrous inventions?

  5. Meet Robert Boyle. Why, hello there! He noticed that if you decrease the volume of a container of gas, the pressure of that gas will increase. Pressure is the result of a FORCE being distributed over an area!

  6. More about pressure…Predict which will sink into the grass: the stiletto heel or the athletic shoe?

  7. Greater Pressure The FORCE of the person’s weight pressing down is the same in either pair of shoes. BUT, when this force is applied to the SMALL area of dirt by the tiny stiletto heel, it results in a great deal of pressure, and the heel of the shoe sinks.

  8. Decrease the volumeof a container of gas, the pressure of that gas will increase volume pressure The inverse is also true! Increase the volume of a container of gas, the pressure of that gas will decrease  volume pressure

  9. Boyle “boiled it down” like this: BOYLE’S LAW: The volume of a gas is INVERSELY PROPORTIONAL to its pressure (if the number of particles and the temperature stays the same). Written as an equation, P1V1= P2V2 Where the left side are the amounts before a change and the right side are the amounts after a change.

  10. Remember Boyle’s Law? Boyle’s Law says that a smaller volume means a greater pressure. Our friend sat on the cushion, thus making the VOLUME decrease. To relieve the GREATER PRESSURE, the gas in the cushion escaped QUICKLY through the small opening. Gas had been slowly leaking out of the cushion, but our friend sat on it. He DECREASED the volume, and therefore INCREASED the pressure.

  11. Has this ever happened to you?

  12. A nice warm day… Tire pressure looks good! No need to fill them more.

  13. Later that day…

  14. It turns very cold… My tires look FLAT! What happened?!

  15. My tiré, she is all flat now! Uhn, Hunh! Jacques Charles, a Frenchman, noticed this sort of thing, too. OK, not EXACTLY like that…

  16. CHARLES’S LAW:The volume of a gas is directly proportional to its temperature [in Kelvins, specifically] (if the pressure and the number of particles are constant). Written as an equation, V1 / T1 = V2 / T2 Where the left side are the amounts before a change and the right side are the amounts after a change.

  17. I knew you were gonna ask that! A Kelvin is just like a degree Celsius, BUT, Kelvins start in a different spot. Zero Kelvin is about –273.15 degrees Celsius. Why? 0 K is a temperature we’ve never measured on Earth, (although we have gotten close). It is the point at which as gas is SO COLD that its VOLUME would be zero liters. 0 Kelvin is also known as ABSOLUTE ZERO.

  18. What would happen if…I increased the volume of a container of gas? • Pressure would increase • Pressure would decrease

  19. What would happen if…I increased the pressure of a container of gas? • Volume would increase • Volume would decrease

  20. What would happen if…I increased the temperature of a container of gas? • Volume would increase • Volume would decrease

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