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Lab Experiment on Gas Laws, Lab Reports of Chemistry

Northern State UniversityChemistry

Ideal gases: Boyle’s Law, Charles’ Law, Gay-Lussac’s Law, Avogadro’s Law, Combined Gas Law in lab activity

Typology: Lab Reports

2020/2021

Uploaded on 05/11/2021

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!!!
Experiment*#*7."Gas$Laws.!
Goal!
To!observe!gas!laws!in!the!laboratory.!
!
Introduction!
All!ideal!gasses,! regardless!of!molar! mass!or!chemical! properties,!follow!the! same!gas!laws! under!most!conditions.!!Gas!
Laws!are!derived!from!the!Kinetic!Theory!which!makes!the!assumptions:!
• Gasses!are!composed!of!small!particles!that!are!in!constant!random!motion!
• The!volume!of!particles!is!negligible!compared!to!the!space!they!occupy.!
• The!attraction!between!particles!is!negligible.!
• The!average!speed!of!the!gas!is!directly!proportional!to!its!Kelvin!temperature.!
!
If!a!gas!follows!these!assumptions,!the!gas!is!said!to!be!ideal.!!!
!
The!pressure! of! a! gas! results! from! the! collision!of! gas! particles! with! the! sides! of! the! container! –! the! more!
collisions,!the!higher!the!pressure! of!the! gas.!The!volume!of!a!gas! is!equal!to!the!volume! of!its!container.!!Unless! a!gas!
container! is! rigid,! the! container! will! change! volume! to! maintain! the! same! pressure! inside! and! outside! the! container.!!
Balloons!can! change!volume! very!easily! to!maintain! the!same!pressure! outside!and!inside! –!in!all! balloon! experiments!
the!pressure!remains!constant.!
!
Boyle’s!Law!Pressure!and!volume!are!indirectly!related!at!constant!temperature!–!as! one!increases!the!other!decreases.!!
As!the! volume! of!a!sample! of! gas!increases,!the! particles! collide! with! the! sides! of! the! container! less! often,! leading! to!
lower!pressure.!
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!=𝑃
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Charles’!Law!Volume!is!directly!related!to!temperature!of!a! gas!at!constant!pressure.!!As!the!temperature!increases,!so!
does!the!average!speed!of!the! gas!which! leads!to!more!collisions!with!the!sides!of! the!container.!! In!order!to!keep! the!
pressure!constant!as!the!temperature!rises,!the!volume!must!expand,!keeping!the!number!of!collisions!the!same.!
!
𝑉
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Gay-Lussac’s!Law!Pressure!and!Temperature!are!directly!related!at! constant!volume.!!As! the!temperature!increases!in! a!
system!with! fixed!volume,! the!molecules!move!faster!and!have!more! collisions!with! the!container! leading!to! increased!
pressure.!
𝑃
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=
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Avogadro’s!Law!!Volume!and!moles!are!directly!related!at!constant!temperature!and!pressure.!!As!the!number!of!moles!
increases,!the!volume!of!the!container!must!expand!to!keep!the!number!of!collisions!and!thus!the!pressure!constant.!
!
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Combined!Gas!Law!!The!above!laws!joined!together!become!the!combined!gas!law.!!If!more!than!two!properties!are!
changing,!this!law!is!used.!!Any!properties!that!remain!constant!will!drop!out!of!the!equation.!!(ex:!if!temperature!and!
number!of!moles!are!constant,!they!are!removed!from!the!equation!and!it!becomes!Boyle’s!Law)!
𝑃
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=
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Partial preview of the text

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Experiment # 7. Gas Laws.

Goal To observe gas laws in the laboratory. Introduction All ideal gasses, regardless of molar mass or chemical properties, follow the same gas laws under most conditions. Gas Laws are derived from the Kinetic Theory which makes the assumptions:

  • Gasses are composed of small particles that are in constant random motion
  • The volume of particles is negligible compared to the space they occupy.
  • The attraction between particles is negligible.
  • The average speed of the gas is directly proportional to its Kelvin temperature. If a gas follows these assumptions, the gas is said to be ideal. The pressure of a gas results from the collision of gas particles with the sides of the container – the more collisions, the higher the pressure of the gas. The volume of a gas is equal to the volume of its container. Unless a gas container is rigid, the container will change volume to maintain the same pressure inside and outside the container. Balloons can change volume very easily to maintain the same pressure outside and inside – in all balloon experiments the pressure remains constant. Boyle’s Law Pressure and volume are indirectly related at constant temperature – as one increases the other decreases. As the volume of a sample of gas increases, the particles collide with the sides of the container less often, leading to lower pressure. 𝑃!𝑉! = 𝑃!𝑉! Charles’ Law Volume is directly related to temperature of a gas at constant pressure. As the temperature increases, so does the average speed of the gas which leads to more collisions with the sides of the container. In order to keep the pressure constant as the temperature rises, the volume must expand, keeping the number of collisions the same. 𝑉! 𝑇!

Gay-Lussac’s Law Pressure and Temperature are directly related at constant volume. As the temperature increases in a system with fixed volume, the molecules move faster and have more collisions with the container leading to increased pressure. 𝑃! 𝑇!

Avogadro’s Law Volume and moles are directly related at constant temperature and pressure. As the number of moles increases, the volume of the container must expand to keep the number of collisions and thus the pressure constant. 𝑉! 𝑛!

Combined Gas Law The above laws joined together become the combined gas law. If more than two properties are changing, this law is used. Any properties that remain constant will drop out of the equation. (ex: if temperature and number of moles are constant, they are removed from the equation and it becomes Boyle’s Law) 𝑃!𝑉! 𝑇!

Laboratory Activity Equipment 2 x 1000 mL beaker aluminum can hot plate ice hot gloves 2 x balloons beaker tongs 250 mL Erlenmeyer flask vacuum flask rubber stopper vacuum hose small marshmallow Procedure Part A:

  1. Fill a 1000mL beaker half way with tap water. Begin heating on a hot plate
  2. Fill a second 1000mL beaker halfway with water and ice.
  3. Obtain a small balloon filled with air. Submerge the balloon in the ice water bath from for three minutes using beaker tongs. Observe any changes.
  4. Transfer the balloon to the hot water bath. Submerge with beaker tongs. Observe any changes.
  5. Save the ice-water bath for Parts C & D. Part B:
  6. Obtain a vacuum flask. One person in the group should hold the flask at all times during the experiment – the side-arm breaks easily when the flask tips over.
  7. Place a marshmallow inside and plug the top with a rubber stopper. Attach one end of the vacuum hose to the side arm of the flask and the other end to the vacuum line.
  8. Slowly turn on the vacuum and observe what happens.
  9. Turn off the vacuum before disassembling. 5. Do not eat the marshmallow. Part C:
  10. Obtain a 1 50 mL Erlenmeyer flask and place approximately 20 mL of water in the flask.
  11. Place the flask on a hotplate and heat until a steady stream of steam comes out. Do not let all the water evaporate.
  12. Hold the neck of the flask using hot gloves and stretch the mouth of a balloon over the opening, centering it on the mouth of the flask. Wait up to 3 minutes and observe the results.
  13. Using hot gloves transfer the flask to an ice bath for 3 minutes and observe the results. Part D:
  14. Obtain an empty aluminum can and add approximately 10 mL of water to it.
  15. Place the can on a hotplate set to medium and heat until a steady, substantial stream of steam flows out of the can.
  16. Using hot gloves, turn the can over into an ice-water bath so that the opening of the can is below the surface of the water for a few seconds. If nothing happens to the can after a few seconds, repeat from step 1.

Gas Laws – Report Sheet Name _______________________ Part Observations (describe what happened) Gas properties write ì,î or, –– if unchanged Explanation (why did it happen?) Gas Law Observed A P: –– V: n: –– T: ì B P: V: n: T: C (heating) (^) P: V: n: T: –– (boiling water vapor stays at 100oC) C (cooling) (^) P: V: n: T: D P: V: n: T: