Evaluation of the Gas Law Constant PROCEDURE 1) Get a piece of magnesium ribbon that has a mass between 0.0300-0.0400g. Clean thoroughly with emery cloth. After cleaning, do not handle the ribbon with your hands. 2) Obtain an eudiometer and rinse thoroughly with water ifit is not clean and dry. 3) Fill one liter beaker half full of tap water. 4) Empty the eudiometer oiny water remaining. Fill it to the 25.0mL mark with the 3.0 M hydrochloric acid. Caution: Hydrochloric acid is very caustic. Wear goggles at all times. Fill the eudiometer to the top with distilled water. Make a "v" out of the piece of magnesium ribbon and wedge it into the eudiometer in the distilled water. 5) Put your finger over the top of the eudiometer and quickly invert it and put the top into the beaker of water. Remove your finger. 6) After the ribbon has completely reacted, record the volume of the gas in the eudiometer. 7) Repeat as time permits. DATA Barometric Pressure 768 torr Vapor Pressure of Water 18.7 torr Corrected Pressure unknown atm Temp Celcius 21 degrees Temp Kelvin unknown degrees EXPERIMENT trial 1 trial 2 trial 3 mass of Mg (g) 0.0391 0.0305 0.0351 molar mass of Mg (m/mol) 24.305 24.305 24.305 number of mol of Mg (mol) 0.00160872 0.0012549 0.00144 mol of H2 (mol) 0.00160872 0.0012549 0.00144 volume of H2 (mL) 38.5 31.7 36.9 volume of H2 (L) 0.0385 0.0317 0.0369 temperature (degree C) 21 21 21 temperature (K) 294.15 294.15 294.15 barometric pressure (torr) 768 768 768 vapor pressure (torr) 18.7 18.7 18.7 pressure of H2 (torr) 749.3 749.3 749.3 pressure of H2 (atm) 0.98592105 0.9859211 0.98592 R (L atm/mol k) 0.0802145 0.0846698 0.08564 average R (L atm/mol k) 0.08350884 CALCULATIONS 1) Show calculations for the corrected pressure in atm. 2) Show calculations for R including all units.
Ideal and Real Gases
Ideal gases obey conditions of the general gas laws under all states of pressure and temperature. Ideal gases are also named perfect gases. The attributes of ideal gases are as follows,
Gas Laws
Gas laws describe the ways in which volume, temperature, pressure, and other conditions correlate when matter is in a gaseous state. The very first observations about the physical properties of gases was made by Robert Boyle in 1662. Later discoveries were made by Charles, Gay-Lussac, Avogadro, and others. Eventually, these observations were combined to produce the ideal gas law.
Gaseous State
It is well known that matter exists in different forms in our surroundings. There are five known states of matter, such as solids, gases, liquids, plasma and Bose-Einstein condensate. The last two are known newly in the recent days. Thus, the detailed forms of matter studied are solids, gases and liquids. The best example of a substance that is present in different states is water. It is solid ice, gaseous vapor or steam and liquid water depending on the temperature and pressure conditions. This is due to the difference in the intermolecular forces and distances. The occurrence of three different phases is due to the difference in the two major forces, the force which tends to tightly hold molecules i.e., forces of attraction and the disruptive forces obtained from the thermal energy of molecules.
Evaluation of the
PROCEDURE
1) Get a piece of magnesium ribbon that has a mass between 0.0300-0.0400g. Clean thoroughly with emery cloth. After cleaning, do not handle the ribbon with your hands.
2) Obtain an eudiometer and rinse thoroughly with water ifit is not clean and dry.
3) Fill one liter beaker half full of tap water.
4) Empty the eudiometer oiny water remaining. Fill it to the 25.0mL mark with the 3.0 M hydrochloric acid. Caution: Hydrochloric acid is very caustic. Wear goggles at all times. Fill the eudiometer to the top with distilled water. Make a "v" out of the piece of magnesium ribbon and wedge it into the eudiometer in the distilled water.
5) Put your finger over the top of the eudiometer and quickly invert it and put the top into the beaker of water. Remove your finger.
6) After the ribbon has completely reacted, record the volume of the gas in the eudiometer.
7) Repeat as time permits.
DATA
| Barometric Pressure | 768 torr |
| Vapor Pressure of Water | 18.7 torr |
| Corrected Pressure | unknown atm |
| Temp Celcius | 21 degrees |
| Temp Kelvin | unknown degrees |
| EXPERIMENT | trial 1 | trial 2 | trial 3 |
| mass of Mg (g) | 0.0391 | 0.0305 | 0.0351 |
| molar mass of Mg (m/mol) | 24.305 | 24.305 | 24.305 |
| number of mol of Mg (mol) | 0.00160872 | 0.0012549 | 0.00144 |
| mol of H2 (mol) | 0.00160872 | 0.0012549 | 0.00144 |
| volume of H2 (mL) | 38.5 | 31.7 | 36.9 |
| volume of H2 (L) | 0.0385 | 0.0317 | 0.0369 |
| temperature (degree C) | 21 | 21 | 21 |
| temperature (K) | 294.15 | 294.15 | 294.15 |
| barometric pressure (torr) | 768 | 768 | 768 |
| vapor pressure (torr) | 18.7 | 18.7 | 18.7 |
| pressure of H2 (torr) | 749.3 | 749.3 | 749.3 |
| pressure of H2 (atm) | 0.98592105 | 0.9859211 | 0.98592 |
| R (L atm/mol k) | 0.0802145 | 0.0846698 | 0.08564 |
| average R (L atm/mol k) | 0.08350884 |
CALCULATIONS
1) Show calculations for the corrected pressure in atm.
2) Show calculations for R including all units.
POST QUESTIONS
1) An evaluation of R was performed, following the procedure described in this experiment. The barometric pressure was 736 torr, the vapor pressure of water was 19.83 torr, the temperature was 295 K, the mass ofMg used was 0.0335 g, and the volume of Hydrogen gas collected was 35.6 m.L.
a) What would have been the calculated value of R in mL•atm/mol-K? Show work.
b) If the barometric pressure had not been corrected for the vapor pressure of water, what would have been the calculated value of R in mL•atm/mol K? Show work.
c) What would have been the% error it the calculated value of R if the barometric pressure had not been corrected for the vapor pressure of water? Show work.
2) a) What is the volume of one mole of hydrogen gas at 273 K and 760 torr?
b) What is the volume of one mole of oxygen gas under the same conditions?
c) What does this suggest concerning the
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