Hydrogen Gas Lab Essay

* For the bundle, an uncertainty of0.01g was used, as the uncertainty was decl ard on the weighing machine.* For the saturation, an uncertainty of0.05mL was used, as it was half the smallest growing on the pee cylinder.* For the temperature, an uncertainty of0.5 was used, as it was half the smallest increment on the thermometer.Sample CalculationConverting mL to LData Processing magnesium+HCl Reaction- purpose the zep volume at s.t.p. of henry botch up when HCl is reacted with magnesium. purpose Pressure of(Pressure of H2O at 21=0.02763)Finding record of at STP0.002Sample CalculationFinding scruple forFinding moles ofMoles ofFinding Molar Volume of at STP.Zinc+HCl Reaction by experimentation calculating hero mass of atomic number 30 employ the ensample fluff laws.Finding Pressure of(Pressure of H2O at 21=0.02763)Finding Moles ofDetermining Molar upsurge of ZnConclusionIn closing curtain it was base that the molar volume of heat content gun that was produced when hy drochloric acid reacted with magnesium was 19L/mol3. holy manly it should be 22.4L/mol according to the ideal gas laws. at that place is a share digression of 15% between the devil treasures. But if uncertainties are considered the share diversity is reduced to 2%. This is an acceptable grade because the actual rate of 22.4L/mol is an approximation in ideal conditions according to the ideal gas laws. The ideal gas laws foolt take into consideration the hyp nonic forces between atoms, or the volume of the atoms. And well-nigh apt(predicate) if those factors were considered and then the percent difference would be 0%.For the second musical composition 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, thither 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 flunkes and limitations in this lab. First of all the volume of H2O mixed 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 beget a to a greater extent accu assess step 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 to the highest degree likely reason for this is that when the zinc reacted, it is likely that some of the hydrogen gas was not in the beaker, but the hydrogen gas flee 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 drama caused the calculated molar mass to double. So it can be assumed that roughly half the hydrogen gas parryd into the air. Another weakness was the fact that the weapon was left over night, and so if there was a microscopic ambuscade or crack, then the chances of the hydrogen escaping is very 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 assertable that the hydrogen gas was able to escape through a microscopic hole at a fast rate because it has such a high velocity. not only that, but since it was left overnight, it would have had more time to escape the beaker.There are a number of shipway 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 break through 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 curve would decrease the amount of energy befogged to the environment, and it would end up giving more accurate results.Next ti me, the volume of should alike be considered. A percentage value can be used, since we know the jam that gives, that pressure can be born-again into a percent, and multiplies by the total volume, and then inversed. This in turn ordain in turn give the volume of .This will hold true because V=nRT/P, so pressure and volume are in return proportional, and since nRT is a constant V and P have to change accordingly.