Molar Volume of a Gas Essay Example for Free

Molar Volume of a Gas leavenIntroductionIn this lab I am going to find verboten the hoi polloi of whizz mole of heat content gas at room temperature and atmospheric pressure. The room pressure only ab reveal differs from the standard, but can be taken into consideration when calculating the results. The hoagie volume is 22.41 liters per mole at STP (Standard pressure), in other words, at zero degrees centigrade.Figure 3.1 (the experiment set up)Procedure1. notice up all equipment.2. Cut a piece of Magnesium laurel wreath about 20cm in length. 3. lead the weight of the ribbon from the weight of a 1 m long ribbon.4. Measure 1.0 M Hydrochloric acidulous to a volume of 25-30ml.5. Pour the HCl to the chemical substance reply flaskful.6. Add the Mg ribbon to the answer flask and vouch the mouth of the flask as fast as possible with a hose. Make sure that the hydrogen gas cannot escape from the flask.7. Follow the temperature8. Collect the gas until no further reception i s observed in the reaction flask.9. Carefully remove the gas parade flask so that no gas escapes from the flask.10. lower the gas.11. Determine the volume of the gas.12. Calculate the molar volume of H2 gas at room temperature.a) theoretical harbor from Vm =22.44 l/mol at STP.b) experimental value from your data.Equipment* 2 flasks (volume at least 600ml)* large container (volume at least 3,5 l)* Magnesium ribbon* 30ml of Hydrochloric acid* thermometer* a hose (to cover the reaction flask)Observations* Magnesium ribbon was a little oxidized for it had lost some of its shine.* When the collection flask was turned around and move in the water system filled container, there were tiny air bubbles on the inside walls of the flask.* When Magnesium ribbon was added, it began to corrose in the HCl* Instantly after adding the Mg ribbon to the hydrochloric acid, temperature in the reaction flask started to rise as a chemical reaction took place in the flask.* Moisture and (fog) blocked th e view of the reaction* today after adding the Mg ribbon, hydrogen bubbled to the collection flask* Hydrogen bubbled to the flask for about a minute,stopping briefly after the ribbon had corrosed in to the HCl.* There was a hissing vowelize as the chemical reaction occurred in the reaction flask and the gas flowed to collection flask through a pipe.* The temperature in flask A rose quickly by a hardly a(prenominal) degrees celsius and then stayed nearly constant for the 15 minutes the temperature was measured.* The temperature did not change in flask Bhowever, it cannot be extractd for sure as it was only compared with the temperature of flask A.* The temperature in flask A rose very quickly as the reaction started* The amount of hydrogen produced from the reaction was large for large bubbles of gas rose to beaker B within few seconds after starting the experiment* The volume of the reaction flask was not measured, but it is close to the volume of the other flask (629ml)* After the reaction, when lighting the hydrogen gas, collection beaker made a popping sound but the reaction flask actually burned and formed a thin flame.* The flame from the reaction flask gave out a lot of heat, which was not noticed when lighting the gas in the collection flask.Theoretical = 22.5 l/molVm= 22.410.36 % errorThe molar volume was 0.36% too large. The error can decrease from water vapour in the collection flask 10cm water below the glass air in the collection flask temperature rise in the reaction flask water vapour in the reaction flaskEvaluationThis experiment had many error-causing factors, which probably influenced the results. Overall, the calculations showed that very little error (0.36% error) which made me a little skeptical about the results. Such a small error percentage was not expected.To depict out a few mistakes, I did not measure the difference in height of the water level from the progress of the water-filled container. This would have allowed further in vestigation about the volume of hydrogen in the flask. Also, the take up volume of the reaction flask was not measured. It was only stated by eye that the flasks looked to be the equivalent size.Other than that, the experiment was performed well. It was made sure that none or very little air was remaining in the collection flask when turning it around and placing it in the water filled container. There were a few tiny air bubbles on the walls however, the air in the reaction flask was more probably to influence the result. Having a lab partner helped with managing time, for one was able to follow the temperature while the other analyze the time. We made sure that we had read the instructions carefully and thought twice before deciding what methods to exercise when, for example, turning the flask upside down in the water.Conclusion In conclusion, the experiment turned out some successful results. When magnesium reacted with the hydrochloric acid, hydrogen was released into the flask from where it flowed through a pipe to the collection flask. The molar volume of H2 gas at room temperature is 22.79 l/mol, which is also the rate for the hydrogen gas in the collection flask. The amount of H2 gas in the flask is impossible to calculate for the amount of water vapour and air was measured when performing the experiment. The experimental value turned out unexpectably very small. 0.36% error in the experiment seems very small, unless there has been some unnoticed mistakes that have influenced the experimental value.The theoretical value is 22.5 l/mol.Temperature changes during the experiment turned out some interesting results, for the temperature seems to start falling soon after the chemical reaction has ended, yet it begins to rise a little after a few minutes and remain constant for a long time before starting to fall (figure 3.2). From the information gained during this experiment, it is difficult to state why this happened therefore, some extra research sh ould take place if performing the experiment again.Improved investigation For further investigation, temperature should be measured for longer than 15 minutes in order to find out the rate the temperature is going to fall in a closed flask. The distance between water surface in the container and the surface in the flask should also be measured. For more accurate results, factors such as air and water vapour in the flask should be taken into consideration when calculating the lowest values. Advisable would be to do some research on why the temperature changed the way it did in this experiment.