Enthalpy of Displacement

total stir up of DisplacementSaran Singh SoundAim To determine the enthalpy stir of fracture between coat powderize and copper sulphate Zn (s) + CuSO4 (aq) Cu (s) + ZnSO4 (aq)Chemicals CuSO4 Solution ( concentration = 0.5 mol.dm3 ) coat (s) PowderData Collection put back 1 List of apparatus and Least Count and Uncertainties of Measuring Instruments UsedS. No.InstrumentUnitLeast CountUncertainty1.Butter news reportn/an/an/a2.Cardboard Lidn/an/an/a3.digital Laboratory ThermometerCelsius0.1 C0.1 C4.Digital Weighing BalanceGrams0.001g0.001g5.Measuring Cylindercm31cm30.5cm36.Polystyrene Cupn/an/an/a7.Digital StopwatchSeconds0.01s0.01sQualitative DataTimeTemperatureTable 2.1 bus of Zinc Powder hand of Zinc (s) /M/g/0.001gTrial 10.244gTrial 22.523gTrial 32.416gTable 2.2 Collected DataTime/t/s/0.01sTemperature/T/c/0.1cTrial 1Trial 2Trial 330.0028.428.660.0028.428.690.0028.428.6120.0028.428.6150.0029.133.0180.0031.238.4210.0032.941.9240.0035.044.8270.0037.546.3300.0040.047.2330.0041 .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 ObservationIt was find that when Zinc (s) powder was added to the CuSO4 solution it immediately reacted making the solution warmer .The touch of the solution at the beginning was greenish in color which then turned color little after the Zinc (s) powder had reacted. After the answer was over, it was observed that Copper had precipitated at the bottom of the cup as a result of it being displaced by Zinc (s) powder.FormulasMass = No. of Moles (aq) x submarine sandwich Mass (s)AndNo. of Moles = Concentration x VolumeAnd-H = Extrapolation Temperature Initial TemperatureAndEnthalpy Change = Mass x Specific affectionateness Capacity x -HAndMolar Enthalpy Change = AndMass of water = volume of copper sulphate solutionAnd constituent Deviation = x one hundredTrial 1Volume of CuSO4 (aq)60.0cm3Mass of Water60gSpecific incite Capacity4.18 J.g1.C-1Initial Temperature28.4 CExtrapolation temperature53.0 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 fitted 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, mass of zinc had to be taken in excess. Therefore, Mass of Zinc is great than actual mass mandatory as seen in Table 2.1-H = 28.4 53.0 = -24.60 C 0.01sEnthalpy 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 belles-lettres value of Enthalpy Change for this displacement reaction is -217kJ.mol-1Percentage Deviation = x 100 = 5.2% 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 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 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 = -830 9.84 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... Mass of Zinc (s) powder = 0.035 x 65 = 2.275gHowever for this experiment, mass of zinc had to be take n 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 surrounding culminationThe displacement reaction between Zinc (s) powder and CuSO4 solution is exothermic as heat is released to its immiediate surroundings. This is supported 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 surface area. By observing the graph it is found that after reaching the crest temperature, the new 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 manageable that the concentration of the Cuso4 solution was lower , 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 evacuant more energy. This is suggested by the calculations for Trial 1, Trial2 and Trial 3.The percentage deviation of the experimental readings to the literature value is not that high suggesting few errors in the experiment. However, we attributed them to ce rtain and possible errors.