value may deviate largely (up to about 30% error) from the industrial value determined with more preciseequipment.Use this industrial value (theoretical value) and the averageCpvalue you obtained inExperiment 1

value may deviate largely (up to about 30% error) from the industrial value determined with more preciseequipment.Use this industrial value (theoretical value) and the averageCpvalue you obtained inExperiment 1 (experimental value) to determine the percent error in your experimental value.Theequation for percent error is:Experimental value – Theoretical value%Error100Theoretical valueShow work:Experiment 2Use the industrialCpvalue (more precisely determined value) from Experiment 1 for yourcalculations in Experiment 2.4. Record the following for each of the three trials.Be sure to record all data and calculated results withthe correct number ofsignificant figures.*Remember to use at least four significant figures for molarmass,MM.This reduces the chance for rounding errors in calculations.Trial 1Mass of the empty calorimeter (g):18.6 gInitial temperature of the HCl solution in calorimeter (°C)21.5 CFinal temperature in the calorimeter after the reaction (°C):34.5 CCalculate change in temperature, (T(Tfinal–Tinitial)13 CMass of the calorimeter containing HCl solution before reaction(g):68.600 gCalculate the mass of the HCl solution in the calorimeter (g):Calculate the moles of Mg reacted(using *MMMgwith 4 significantfigures):Trial 2Mass of the empty calorimeter (g):18.6 gInitial temperature of the HCl solution in calorimeter (°C)21.5 CFinal temperature in the calorimeter after the reaction (°C):43.2 CCalculate change in temperature, (T(Tfinal–Tinitial)21.7 CMass of the calorimeter containing HCl solution before reaction(g):68.600 gCalculate the mass of the HCl solution in the calorimeter (g):Calculate the moles of Mg reacted(using *MMMgwith 4 significantfigures):Trial 3

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