Enthalpy of Displacement

hot pants content of DisplacementSaran Singh SoundAim To determine the instigate content adjustment of duty period amid zinc disinteg direct and copper sulfate Zn (s) + CuSO4 (aq) Cu (s) + ZnSO4 (aq)Chemicals CuSO4 Solution ( concentration = 0.5 counterspy.dm3 ) coat (s) mill data Collection Table 1 List of apparatus and least(prenominal) Count and Uncertainties of Measuring Instruments UsedS. noneInstrumentUnit least(prenominal) CountUncertainty1.Butter Papern/an/an/a2.Cardboard Lidn/an/an/a3.digital Laboratory ThermometerCelsius0.1 C0.1 C4.Digital Weighing BalanceGrams0.001g0.001g5.Measuring Cylindercm31cm30.5cm36.Polystyrene fermentn/an/an/a7.Digital StopwatchSeconds0.01s0.01sQualitative Data convictionTemperatureTable 2.1 fix of atomic number 30 Powder surge of surface (s) /M/g/0.001g audition 10.244g ravel 22.523gTrial 32.416gTable 2.2 Collected DataTime/t/s/0.01sTemperature/T/c/0.1cTrial 1Trial 2Trial 330.0028.428.660.0028.428.690.0028.428.6120.0028.428.6150.00 29.133.0180.0031.238.4210.0032.941.9240.0035.044.8270.0037.546.3300.0040.047.2330.0041.647.4360.0042.547.1390.0042.546.6420.0042.345.9450.0042.145.4480.0041.645.0510.0041.044.4540.0040.543.4570.0040.042.8600.0039.441.9630.0038.741.0660.0038.040.6690.0037.439.8720.0036.639.2750.0036.038.4780.0035.537.6810.0034.736.8840.0034.036.0870.0033.235.6900.0032.634.6930.0033.7960.0032.9990.0032.1Qualitative manifestationIt was observed that when zinc (s) powder was added to the CuSO4 final result it immediately reacted making the termination warmer .The color of the ascendent at the beginning was greenish in color which then turned colorless after the Zinc (s) powder had reacted. After the response was over, it was observed that Copper had precipitated at the bottom of the loving cup as a result of it being displaced by Zinc (s) powder.FormulasMass = No. of Moles (aq) x Molar Mass (s)AndNo. of Moles = Concentration x VolumeAnd-H = Extrapolation Temperature initial TemperatureAnd atomic number 1 Change = Mass x Specific heat Capacity x -HAndMolar enthalpy Change = AndMass of water = volume of copper sulphate solutionAnd division Deviation = x snowTrial 1Volume of CuSO4 (aq)60.0cm3Mass of pissing60gSpecific Heat Capacity4.18 J.g1.C-1Initial Temperature28.4 CExtrapolation temperature53.0 CTime at which Zinc (s) powder was added120sThe graphical record is used to estimate the diversify in temperature of the switching reaction among CuSO4 solution and Zinc (s) powder. The side of the best tantrum line shows the rate of decrease of temperature.Calculation-No. of Moles of 60.0cm3 CuSO4 (aq) = (60/1000) x 0.5 = 0.03 mol... Mass of Zinc (s) powder = 0.03 x 65 = 1.961gHowever for this experiment, pile of zinc had to be taken in excess. at that placefore, Mass of Zinc is greater than actual mountain indispensable as seen in Table 2.1-H = 28.4 53.0 = -24.60 C 0.01s henry Change = 60 x 4.18 x -24.6 = -6169.68 J = -6.16968 kJMolar Enthalpy Change = = -205.7 kJ.mol- 1As this reaction is exothermic i.e heat is released, enthalpy change is negative.The literature value of Enthalpy Change for this displacement reaction is -217kJ.mol-1Percentage Deviation = x 100 = 5.2% Deviation.Note There were two assumptions make during this experiment.The Specific Heat Cpacity of the solution is same as waterNo Heat is lost to the touchTrial 2Volume of CuSO4 (aq)70.0cm3Mass of Water60gSpecific Heat Capacity4.18 J.g1.C-1Initial Temperature28.6CExtrapolation temperature57.0 CTime at which Zinc (s) powder was addedThe graph is used to estimate the change in temperature of the displacement reaction between CuSO4 solution and Zinc (s) powder. The gradient of the best fit line shows the rate of decrease of temperature.Calculation-No. of Moles of 70.0cm3 CuSO4 (aq) = (70/1000) x 0.5 = 0.035 mol... Mass of Zinc (s) powder = 0.035 x 65 = 2.275gHowever for this experiment, mass of zinc had to be taken in excess. Therefore, Mass of Zinc is greater than actual mass requi red as seen in Table 2.1-H = 28.6 57.0 = -28.40 C 0.01sEnthalpy Change = 70 x 4.18 x -28.40 = -8309.84 J = -8.30984 kJMolar Enthalpy Change = = -207.7 kJ.mol-1As this reaction is exothermic i.e heat is released, enthalpy change is negative.The literature value of Enthalpy Change for this displacement reaction is -217kJ.mol-1Percentage Deviation = x 100 = 4.3% Deviation.Note There were two assumptions made during this experiment.The Specific Heat Cpacity of the solution is same as waterNo Heat is lost to the surroundingTrial 3Volume of CuSO4 (aq)70.0cm3Mass of Water60gSpecific Heat Capacity4.18 J.g1.C-1Initial Temperature28.6CExtrapolation temperature57.0 CTime at which Zinc (s) powder was added120sThe graph is used to estimate the change in temperature of the displacement reaction between CuSO4 solution and Zinc (s) powder. The gradient of the best fit line shows the rate of decrease of temperature.Calculation-No. of Moles of 70.0cm3 CuSO4 (aq) = (70/1000) x 0.5 = 0.035 mol... Ma ss of Zinc (s) powder = 0.035 x 65 = 2.275gHowever for this experiment, mass of zinc had to be taken in excess. Therefore, Mass of Zinc is greater than actual mass required as seen in Table 2.1-H = 28.6 57.0 = -28.40 C 0.01sEnthalpy Change = 70 x 4.18 x -28.40 = -8309.84 J = -8.30984 kJMolar Enthalpy Change = = -207.7 kJ.mol-1As this reaction is exothermic i.e heat is released, enthalpy change is negative.The literature value of Enthalpy Change for this displacement reaction is -217kJ.mol-1Percentage Deviation = x 100 = 4.3% Deviation.Note There were two assumptions made during this experiment.The Specific Heat Cpacity of the solution is same as waterNo Heat is lost to the surroundingConclusionThe displacement reaction between Zinc (s) powder and CuSO4 solution is exothermic as heat is released to its immiediate surroundings. This is support by the calculations of all the three trials. The Zinc (s) is in powder form which reacts faster with CuSO4 solution as it has a larger surfa ce area. By observing the graph it is found that after reaching the peak temperature, the untried solutions temperature starts to decrease which means that its is loosing heat to its surrounding. The line of best fit on the graph shows the temperature change in an ideal situation. However, in reality heat is lost to the surroundings and the specific heat capacity of the solution may not be the same as water. This reaction between Zinc (s) powder and CuSO4 takes place becaude Zinc (S) powder is more reactive thancopper in CuSO4 solution. Therefore, causing copper to precipitate.It is also possible that the concentration of the Cuso4 solution was discredit , causing less energy to be released then expected.The temperature change increases as volume of CuSO4 is increased as more Zinc (s) powder is required to react therefore releasing more energy. This is suggested by the calculations for Trial 1, Trial2 and Trial 3.The percentage deviation of the experimental readings to the litera ture value is not that advanced suggesting few errors in the experiment. However, we attributed them to certain and possible errors.