Experiment 6 – ThermochemistryName name Lab Section 432Results and DiscussionFigure 1. This graph shows how the temperature increases as time increases as well. What is noticeable isthat this experiment has the lowest initial and final temperature out of the three experiments.Figure 2. In this graph there is a more abrupt increase at the beginning for the temperature, then it levelsoff and even decreases as time goes on. The final temperature is around 2 degrees Celsius higher than theprevious experiment and the initial temperature is 1 degree Celsius higher than experiment 1. Figure 3. In this graph there is a steeper increase in temperature initially and then it levels off as timegoes on once it reached 200 seconds. The final temperature is again 2 degrees Celsius higher than theprevious experiment and the same initial temperature. Table 1. Results Data TableExperiment 1 Experiment 2 Experiment 3ΔHHess-44.5 -56.13 -100.13ΔHexp40.5kJ 47.6kJ 63.6kJ%Error 8.99% 15.20% 36.48% Calculations for Experiment#3Tmin=21.0 °C Tmax=29.0°CΔT=8.0°CDensity-0.0002gmL(21.0)+1.0012g/mL=0.997g/mLMass=0.997*100=99.7gC=18.29J/°CQsoln=ΔT*C*m=(8.0°C)*(4.00J/g*°C)*99.7g=3190.4JQcal=C*ΔT=(18.29J/°C)*8.0°C=146.32JQrxn= -(qcal-qsoln)= -(146.32J+3190.4J)= -3336.72J2.101gNaOH*(1mol/40gNaOH)=0.0525molNaOHΔHrxn=qrxn/molsNaOH= -3336.72J/0.0525mol=-63556.5714J=63.6kJNaOH(s)+HCl(aq)NaCl(aq)+H2O(l)-425.6 -167.2 -407.1 -285.83∑(products-reactants) (-407.1+ -285.83)-(-425.6+ -167.2) (-692.93)-(-592.8)=-100.13%error|ΔHexp-ΔHHess/ΔHHess|*100|(63.6kJ- -100.13)/-100.13|*100=36.48%Balanced Equations:NaOH(s)Na+(aq)+OH-(aq)Na+(aq)+OH-(aq)+H+(aq)+Cl-(aq)H2O(l)+Na+(aq)+Cl-(aq)NaOH(s)+H+(aq)+Cl-(aq)H2O(l)+Na+(aq)+Cl-(aq)Conclusion: This experiment did show how the exothermic and endothermic reactions worked and heats of reaction. The reactions are exothermic since they release heat and endothermic reactions absorbs heat from it’s surroundings. The results showed how in the first trial with NaOH solid in water that the initial and final temperature were both lower compared to the other two experiments. The initial temperature in the first experiment was 20.0°C and the final temperature was 25.1°C. In the second experiment the initial temperature was 21.0°C and the final was 27.0°C. In the third experiment the initial is again 21.0°C and the final was 29.0°C. What is noticeable is that with each experiment the final temperature increases by 2°C. The results do verify the generalization of Hess’s Law of Constant Heat Summation. There was a possible source of error which is improper insulation. The temperature can be possibly affected in the trials then and may change the results. Another possible flaw is we went over once by 2 seconds for checking the temperature however that is minor. The conclusion is that yes what was experimented for was found. The results support this and it teaches students more about Hess’s law and how it works. It shows the importance of Hess’s law in thermochemistry as well as how it’s important to different reactions both exothermic and endothermic. A lot of these reactions are vital to us or helps us in some way. Some of these reactions in our bodies and some have to do with different things humans have created. Without Hess’s law we won’t have as good ofan understanding of thermochemistry and Hess’s law let’s us anticipate enthalpy changes of reactions that are done too slow to record. The calculations also show how the ΔHexp is relatively accurate although the percent error does increase with each experiment. Through doing the calculations this also demonstrates how useful Hess’s law is. So this experiment did show and prove a lot related to Hess’s law and