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Lab report. Finding the molar enthalpy change of the reaction between Hydrochloric acid and sodium carbonate

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Introduction

lFinding the molar enthalpy change of the reaction between Hydrochloric acid and sodium carbonate by: Tommaso Fricano Data Collection: After carrying out the experiment I ended up with this raw data: Experiment A Mass of added ±0.001 (g) Initial Temperature ±0.1 () Peak Temperature ±0.1 () Change in Temperature ± 0.2 () Test 1 2.064 24.8 28.9 4.1 Test 2 2.048 24.0 28.9 4.9 Test 3 2.086 23.4 28.7 5.3 Experiment B Mass of added ±0.001 (g) Initial Temperature ±0.1 () Peak Temperature ±0.1 () Change in Temperature ± 0.2 () Test 1 3.018 24.9 17.4 -7.5 Test 2 3.021 23.6 16.3 -7.3 Test 3 3.016 23.4 16.0 -7.4 Experiment C Mass of added ±0.001 (g) Initial Temperature ±0.1 () Peak Temperature ±0.1 () Change in Temperature ± 0.2 () Test 1 3.006 24.9 20.8 -4.1 Test 2 3.012 22.8 18.6 -4.2 Test 3 3.018 22.7 18.7 -4.0 The peak temperature, which can be seen in my results was not he one I obtained from the graph I received form carrying out the experiment as so we would not be talking heat loss into account. In order to find the value of the actual peak temperature I plotted a line, which traced the actual line of the graph from the peak towards the decreasing temperature. ...read more.

Middle

Change in Temperature ± 0.2 () Test 1 2.064 24.8 28.9 4.1 Test 2 2.048 24.0 28.9 4.9 Test 3 2.086 23.4 28.7 5.3 Experiment B Mass of added ±0.001 (g) Initial Temperature ±0.1 () Peak Temperature ±0.1 () Change in Temperature ± 0.2 () Test 1 3.018 24.9 17.4 -7.5 Test 2 3.021 23.6 16.3 -7.3 Test 3 3.016 23.4 16.0 -7.4 Experiment C Mass of added ±0.001 (g) Initial Temperature ±0.1 () Peak Temperature ±0.1 () Change in Temperature ± 0.2 () Test 1 3.006 24.9 20.8 -4.1 Test 2 3.012 22.8 18.6 -4.2 Test 3 3.018 22.7 18.7 -4.0 Enthalpy Change (kj) Exp. A -34±4 Exp. B 35± 2 Exp. C 20±1 Conclusion: From our experiment we managed to conclude that the value for the molar enthalpy change is -50±7 Kj and so we can conclude that this is an exothermic reaction as heat is given off. Using values for bond enthalpies outr teacher Mr. Meisnma resulted having a theoretical value for the enthalpy change of -51 Kj , which falls inside the range of our uncertainty meaning that our experiment is valid. From our results we can also conclude that is an error of ±14% in our results, which is very high. This causes our result to be very inaccurate causing our experiment to be very unreliable From the results we can also conclude that experiment A was exothermic as heat was given off. ...read more.

Conclusion

In the future we can improve this by using a better insulator so decreasing heat loss and improving our experiment as a whole due to the more accurate results. Looking at our results we can see we still had noticeable uncertainties this was caused due to the equipment we used. Due to these uncertainties we cause our results to be less accurate but also less reliable as the range of our final results was way too high. In the future we could improve this by using more accurate equipment, an example of this would be using measuring pipettes instead of classic measuring cylinders in order to decrease the amount of systematic errors in our experiment so causing our experiment to be more reliable. Also another random error in our experiment was cause by the fact that the mass added was not the same. Although the difference was very small this still caused an uncertainty in our results causing our results to be more inaccurate so making the experiment less reliable. In the future we could improve this by making the masses added as equal as possible in order to make all the tests more equal making our experiment fairer so causing our uncertainties to decrease so causing our results to be more accurate. ...read more.

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