Difference between revisions of "Lab Gas Laws"
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::*Eq. 5.17 indicate that the rate at which the gases "diffuse" is inversely proportional to the molecular mass. This means that because HCl is heavier than NH<sub>3</sub>, it will move slower and as a result the NH<sub>4</sub>Cl formed will not be in the center, but closer to the HCl side due to the fact that NH<sub>3</sub> is moving faster. If you plug your molecular masses into Eq 5.17, you will see the the ratio r(NH<sub>3</sub>)/r(HCl) ~ 1.4, so the NH<sub>3</sub> travels 1.4x the distance that HCl would have traveled. | ::*Eq. 5.17 indicate that the rate at which the gases "diffuse" is inversely proportional to the molecular mass. This means that because HCl is heavier than NH<sub>3</sub>, it will move slower and as a result the NH<sub>4</sub>Cl formed will not be in the center, but closer to the HCl side due to the fact that NH<sub>3</sub> is moving faster. If you plug your molecular masses into Eq 5.17, you will see the the ratio r(NH<sub>3</sub>)/r(HCl) ~ 1.4, so the NH<sub>3</sub> travels 1.4x the distance that HCl would have traveled. | ||
| − | + | ''Take home: the heavier the gas the slower it moves, the lighter the gas the faster it moves.'' | |
===The Amazing bottle=== | ===The Amazing bottle=== | ||
Revision as of 13:49, 30 March 2020
Gas Laws Demos
The in-person version of this lab has ~ 10 demo stations for which each group of student will rotate through. At each station are instructions. In a best case scenario, each demo should be documented in your lab notebook under the demo name heading. Some demos require additional calculations.
Chapter 5 material: The content associated with these demos comes from all different sections in this chapter. Reference will be made to the section, but you will only be responsible for the specific information discussed in the demo activity.
Diffusion of Gases
- Watch this video --> https://youtu.be/Rf9j0ztzcs4
in your notebook...
- Write out the reaction that occured...
- what is the molecular mass of HCl -->
- what is the molecular mass of NH3 -->
- Eq. 5.17 indicate that the rate at which the gases "diffuse" is inversely proportional to the molecular mass. This means that because HCl is heavier than NH3, it will move slower and as a result the NH4Cl formed will not be in the center, but closer to the HCl side due to the fact that NH3 is moving faster. If you plug your molecular masses into Eq 5.17, you will see the the ratio r(NH3)/r(HCl) ~ 1.4, so the NH3 travels 1.4x the distance that HCl would have traveled.
Take home: the heavier the gas the slower it moves, the lighter the gas the faster it moves.
The Amazing bottle
- Watch this video --> https://youtu.be/pDtWRrGj6qk
This is a fun demonstration that you could do at home if you had a balloon...try it (not required)...thicker plastic bottles work the best.
in your notebook...
- Draw a detailed picture of the "amazing bottle."
Take home: If you try and blow up a balloon inside of a bottle, the pressure inside of the bottle will increase very quickly since you are decreasing the volume of the bottle very rapidly. If the pressure inside the bottle is allowed to return back to room pressure (by putting a small hole in the bottle) then it appears that you can blow it up, but this is a trick. As shown in the video, if you cover the hole after blowing up the balloon, then you will create a vacuum (low pressure) inside of the bottle preventing the balloon from deflating. You can even "such up," as opposed to "blow up" a balloon!
Cloud in a Bottle
“Throwing” air
Liquid Nitrogen
___ Boyle’s Law
___ Charles’ Law
___ Ideal Gas Equation
___ Butane: liquid or gas?
___ Density of Gases
___ Crushing Soda Cans
___ Evacuation – sucking up a balloon
___ Methanol Combustion
___ What is it…a nebulizer?
___ Cartesian Diver