Hydrogen Gas Lab Essay

* For the mass, an uncertainty of0.01g was used, as the uncertainty was stated on the weighing machine.* For the leger, an uncertainty of0.05mL was used, as it was one-one-half the smallest increment on the calibrated cylinder.* For the temperature, an uncertainty of0.5 was used, as it was half the smallest increment on the thermometer.Sample figuringConverting mL to LData ProcessingMagnesium+HCl Reaction-Finding the mill volume at s.t.p. of hydrogen swagger when HCl is reacted with magnesium.Finding public press of( compress of H2O at 21=0.02763)Finding Volume of at STP0.002Sample CalculationFinding Uncertainty forFinding seawalles ofMoles ofFinding hoagy Volume of at STP.Zinc+HCl Reaction Experimentally calculating seawallar mass of zinc using the exaltation gas laws.Finding Pressure of(Pressure of H2O at 21=0.02763)Finding Moles ofDetermining Molar concourse of ZnConclusionIn conclusion it was open up that the hero volume of hydrogen gas that was produced when hydro chloric acid reacted with magnesium was 19L/mol3. Ideally it should be 22.4L/mol according to the ideal gas laws. There is a percent variation of 15% amid the two values. But if uncertainties argon considered the percent battle is reduced to 2%. This is an acceptable value because the actual value of 22.4L/mol is an approximation in ideal conditions according to the ideal gas laws. The ideal gas laws dont take into consideration the attractive forces between atoms, or the volume of the atoms. And most likely if those concomitantors were considered then the percent expiration would be 0%.For the second part of the experiment it was experimentally found using the ideal gas laws that the molar mass of zinc is 124 g/mol. When compared with the actual value of 65g/mol, at that place is a percent difference of 90%. And even if uncertainties are considered, the percent difference is only reduced to 64%. This is too big therefore the data is rendered unreliable.There were quite a few weaknesses and limitations in this lab. First of all the volume of H2O coalesce in with the H2 gas was not considered. Had it been considered, then the volume found at STP would have been lower, and it would move over a more accurate cadence to what the experimental value is. Another weakness in this lab was the fact that the molar mass of zinc was twice as big as its accepted value. The most likely reason for this is that when the zinc reacted, it is likely that about of the hydrogen gas was not in the beaker, and the hydrogen gas chipd into the air.That is why when the formula n=PV/RT was used, the volume in the numerator was half as big as it should be, which in turn caused the calculated molar mass to double. So it shag be assumed that approximately half the hydrogen gas escaped into the air. Another weakness was the fact that the appliance was left over night, and so if there was a microscopic sight or crack, then the chances of the hydrogen escaping is actually high. This would be true because, and since hydrogen has the lowest molar mass of all the elements, it would have a very high velocity, and so it is possible that the hydrogen gas was able to escape through a microscopic hole at a devalued rate because it has such a high velocity. Not only that, only if since it was left overnight, it would have had more time to escape the beaker.There are a number of ways that this lab could be improved. First of all, a new graduated cylinder should be used to ensure that there are no cracks or holes through which the hydrogen gas can escape. Along with that the apparatus should not be left out overnight, but instead the reaction should be speeded up by heating up the apparatus, and then taking the measurements of the volume of gas every 1 minute. This in turn would decrease the amount of energy lost to the environment, and it would end up giving more accurate results.Next time, the volume of should also be considered. A percentage value can be used, since we know the public press that gives, that insisting can be converted into a percent, and multiplies by the issue forth volume, and then inversed. This in turn will in turn give the volume of .This will hold true because V=nRT/P, so pressure and volume are inversely proportional, and since nRT is a constant V and P have to change accordingly.