Experiment 2 – Aqueous Reactions Part IName name Lab Section 432Results and DiscussionData Table 1. Ammonium Chloride and Sodium CarbonateAmmonium chlorideNH4Cl(s)->NH4+(aq)+Cl-(aq)Sodium carbonateNa2CO3(s)->2Na+(aq) +CO32-Mass (g) 1.034g 1.029gInitial Temperature (oC) 23.2 oC 22.0 oCFinal Temperature (oC) 19.9 oC 23.0 oCMoles (mol) 0.0193molNH4Cl 0.0097molNa2CO3Change in Temperature (oC) -3.3 oC 1.0 oCT/mol (J/mol) 2.147*104J/mol -1.294*104J/mol1.034gNH4Cl*1mol/53.49g=0.193molNH4ClDH20=1g/mL @RTCH2O=4.185J/g oC-(ΔT/mol)*CH2O*mH2O=ΔH/mol in units of J/mol(3.9 oC/0.0193molNH4Cl)*4.185J/g oC*30g= 2.147*104J/molFor Sodium Carbonate(1.0 oC/0.0097molNa2CO3)*4.185J/g oC*30g= -1.294*104J/molData Table 2. Data Table 2 for Sodium Bicarbonate with Citric acid3NaHCO3(aq)+C6H8O7(aq)->3H2O(l)+3CO2(g)+Na3C6H5O7(aq)Mass (g) 3.496gMoles (mol) 0.0416molNaHCO3Final Temperature (oC) 15.0 oCInitial Temperature (oC) 22.9 oCTemperature Change (oC) -7.9 oCT/mol (oC/mol) -5.000*10-4 oC/mol(3.496gNaHCO3)(1molNaHCO3/84.006gNaHCO3)=0.0416molNaHCO30.0416molNaHCO3/-7.9 oC=-0.0005 oC/mol or -5.000*10-4 oC/molData Table 3. Hydrochloric acid and Magnesium Mg(s)+2HCl(aq)->MgCl2(aq)+H2(g)Mass (g) .050gMoles (mol) 0.0020molMgFinal Temperature (oC) 28.9 oCInitial Temperature (oC) 22.5 oCTemperature Change (oC) 6.4 oCT/mol (oC/mol) 3.000*10-4 oC/mol(.050gMg)(1molMg/24.305gMg)=0.0020molMg0.0020molMg/6.4 oC=0.0003 oCDiscussion/Conclusion:Write a conclusion to your findings in Experiment 2. Be sure to discuss specifics of your experiment for all portions of the experiment and sources of error. Refer to the UNC writing Center at (http://writingcenter.unc.edu/resources/handouts-demos/specific-writing-assignments/scientific-reports#section-22) for some help. This should be no longer than 2 paragraphs. The experiment was showing the different reactions that can occur in aqueous solutions and the data shows how the temperatures can change for each experiment. There are exothermic and endothermic reactions and the ones that were endothermic are Ammonium Chloride with water and Sodium Bicarbonate with Citric Acid. The exothermic are dissolving Sodium Carbonate in water and Hydrochloricacid and Magnesium. The solvents are water, Citric acid, and Hydrochloric acid while the solutes are Ammonium Chloride, Sodium Bicarbonate, Sodium Carbonate, and Magnesium. This experiment did help students use skills such as balancing equations, converting from grams to moles,as well as use an equation in order to find the J/mol or oC/mol for each experiment. Some possible sources of errors are perhaps not being exact in measuring the temperature while observing the thermometer and also perhaps being slightly off on the mass when weighing or the amount of the solvent being used. You can also see how the temperature change shows whether or not a reaction is endothermic or exothermic. If the temperature change is negative then it’s endothermic since its not releasing heat, however if it’s positive like for Sodium Carbonate in water and Hydrochloric acid and Magnesium then its exothermic due to it releasing