Volume of a Mole of Gas Lab

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Angela Hays
Mr. Manor
Chemistry Honors P.1
Molar Volume of a Gas Lab
* Purpose: The purpose of the lab is to relate a gas to a certain number of moles. * Prediction: The prediction is that
* Procedure:
1. Obtain two to three pieces of Magnesium ribbon.
2. Measure the ribbon to the 1/100 of a centimeter.
3. Fill beaker up to 500 mL of tap water. Then, fill a graduated cylinder with 10 mm of 6 molar HCl (aq). 4. Poor HCl into gas collection tube.
5. Add distilled water from water bottle into Gas Collector Tube all the way to the top. 6. Place stopper in Gas Collector Tube.
7. The tube was inverted, and was attached to the metal frame. 8. The reaction has now begun.
9. Once the reaction stops, the Gas Collection Tube was removed from the frame, and was placed in a graduated cylinder. 10. Equalize the pressure inside the beaker and inside the Gas Collection Tube. 11. Record that volume.

* Gas Collection Tube
* 1 hole stopper
* Magnesium ribbon (2-3 pieces)
* Metal wire
* Tap water
* Water bottle
* Metal frame
* Graduated cylinder
* 500 mL beaker
Set up:
Qualitative Observations:
When the tube was inverted so that the HCl could react with the solid Magnesium, bubbles appeared in the tube, and covered the Mg ribbon. There were also swirls in the tube that were generated from the Mg ribbon. There were no more bubbles at 46.4 mm from the top. * Data:

Mass of Mg- 24.3g
Mass of 1 meter of Mg ribbon: 3.71 cm
Barometric pressure: 29.30 mmHg
1 meter of Mg: 1.2291 g
Temperature of H2O: 22.1 (Celcius)
Volume of GPC = 45.2 GPT
* Evaluation:
Mg (s) + 2HCl (aq) = H2 (g) + Mg Cl2 (aq)
H2 + Mg = 1:1 ratio
* Conclusion:
Percent error:
| Experimental value – Accepted value | * 100 = Percent Error
Accepted Value

Particle Representation:
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