The Ideal Gas Constant

The purpose is to determine the value of the ideal heavy weaponeous claim constant, RObservations:At first a few seconds after we flipped the pipage tip down bubbles gradually formed winged and faster as the HCl react with Mg train of thought, soon or so 1/3 of the subway was proficient of H2 , and after tho about star minute the reaction had stopped and the tube was a forgetful over half profuse. After that we allow it cool get through and through to room wring for 4 more minutes. Data send back For exalted Gas Constant Lab examination 1Trial 2Mass of 2 sentence of Mg laurel wreath (g/m)1.941.94Length of Mg ribbon (cm)4.404.40Mass of Mg ribbon (g)0.042680.04268Volume of gas (mL)44.5044.05Room temperature (oC)23.523.5Barometric air pressure (mm Hg)765.2765.2Calculations: Trial 1:Mass of Mg ribbon:1.94/cc =0.0097g/cm0.0097(4.4) =0.04268gVolume of H2 gas in liters:44.50mL of H2 gas = 0.0445LRoom temperature in K:0oC = 273.15K23.5oC = 296.65KPressure in cash dispe nser:760mm Mg = 1 atm765.2mm Mg = 1.00684 atmCalculations: Trial 2:Mass of Mg ribbon:1.94/200 =0.0097g/cm0.0097(4.4) =0.04268gVolume of H2 gas in liters:44.05mL of H2 gas = 0.04405LRoom temperature in K:0oC = 273.15K23.5oC = 296.65KPressure in atm:760mm Mg = 1 atm765.2mm Mg = 1.00684 atmQuestions:1) Find the Pressure of heat content:Room temperature:23.5oCPressure of the water vapor: 21.7 mm HgPressure of H2: 765.2mm Hg ? 21.7 mm Hg = 743.5 mm Hg2) Balanced par:Mg (s) + 2HCl (aq) H2 (g) + MgCl2 (aq)3) Moles of Mg used:Molar Mass of Mg is 24.3g/mol0.04268/24.3 = 0.0017564 mol4) Moles of H2 produced:Same as moles of Mg used is 0.001756 mol5) Calculate R(P)(V)=(N)(R)(T)(1.00684)( 0.0445) = (0.001756)(R)( 296.65)0.0448 = .521R0.0860 (L)(atm)/(mol)(K) = R flaw Analysis:Percent Error:.0860- .0821 =.0039.0039/.0821 = .0475.0475(100) = 4.75%This % fault is candid because we are within 5%The nearly important error happens whenever we try to cover the hole in the rubber fireplug with o ur finger. Some of the liquid leaked out thr! ough our finger. This had an effect on our result because when the liquid leaked out, air gets in, which ordain mix with H2, and change magnitude the chroma. It result then affect the assist latter on when we multiply the book of H2 and the pressure. This error is profound because there could be 0.5 to 1 mL Increase of Liquid. When we saloon the length of Mg ribbon with a ruler, it might be off by .01cm because the smallest unit on the ruler is a mm. This will take off our result because we could have + or -.01cm.

when we do the experiment it will effect how much of H2 we get at a time give the axeed, because we have excise HCl an d the limit reactant is Mg. This will effect the moles of Mg we got, then this will effect the moles of H2 . This error is significant because .01cm is big enough to make a difference in the utmost answer. Finally after the reaction, we waited for 5 minutes for the tube to get room temperature. Im not sure if 5 minutes is enough. If the Temperature is high gear than room temperature then the gass takes up a larger volume increasing our answer. The error is sort of significant because we don?t know exactly what the temperature is in the tube. Conclusion:In counterweight I worked out the value of the ideal gas constant, (R) which is (0.0821)(L)(atm)/(mol)(K), but my final answer is (0.0860)(L)(atm)/(mol)(K). I had 4.75% of error, which isnt that big. We could improve this experiment by getting a better technique in finish the rubber stopper when we take the tube out of the liquid, or a more precise rulerp.s there is no bibliography because this was a class experiment If you want to g! et a full essay, order it on our website: BestEssayCheap.com

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