Chemistry 1 Lab Report

essay 12 Calorimetry and Hesss Law Purpose The purpose of this lab is to order the enthalpy of reaction for the burning of one mole of magnesium in oxygen. Although the reaction is exothermic, the ? HRXN will be determined by utilise calorimetry and thusly using Hesss Law to manipulate the data collected to furnish the answer needed. Procedures Dillon, Stephanie. Calorimetry and Hesss Law. Laboratory Manual. Pearson Publishing, 2012, pp. 168-177. Data and Results Part A intensity level of cold peeing 49. 9 mL Temperature of cold water (in form) 23. 50 C quite a little of resilient water 49. 9 mL Temperature of hot water(in cup) 550 CPart A Calculations Mass of cold water 49. 9 g Tf from graph by extrapolation 34. 90 C ?THW for hot water -20. 1 ?TCW for cold water 11. 4 qHW for hot water -4196. 5 J qcw for cold water 2380. 1 J qCal for the cup 1816. 4 J Ccup for the cup 159. 3 J Part B interpretation of sample Metal fizzed when dissolved in HCl Volume of HCl 100 mL Initia l Temperature 220 C Mass of Mg 0. 1485 g Part B Calculations Tf from graph 50 C Mass of HCl 100 g ?TCW for HCl -2092 J qHCl for solution -204. 4 J qCal for cup -2296. 4 J qRXN -47594 J ?HRXN for Mg NET REACTION 2HCl(aq) + Mg(s)MgCl2(aq) + H2(g)Part C Description of sample Volume of HCl 100 mL Temperature of HCl 220 C Mass of MgO 0. 5052 g Part C Calculations Tf from graph 240 C ?TCW for HCl 1. 50 C qHCl for HCl 627. 6 J qCal for cup 61. 32 J qRXN 608. 92 J ?HRXN for Mgo 55469 J/mol sugar Equation 2HCl(aq) + MgO(s)MgCl2(aq) + H2O(l) Calculations Conclusion In this sample we had to find the heat potentiality of the calorimeter cup using two trials of hot and cold water. When we obtained the data after(prenominal) 10 minutes of recording 30 second intervals of the calorimeter cup temperature, we created a line graph to show the trend line.Read this Practice attempt Chem 105With the trend line, we could figure out the final temperature and delta H in the process. With the equati ng we could find the heat of reation for hot water q HW = m c DTHW and using qCW = m c DTCW we could find the heat of reaction for cold water. By using qHW = qCW + qCal, we can find the heat of reaction of the cup and compute that by the change in temperature to find the heat capacity. After placing Mg into HCl and then the same thing with MgO, we could find the heat of solution of HCl with q CW = m c DTHCl.When we found the values of DHRxn for B and C we can wont Hesss Law, which is shown in the calculations section. All the data is in the data section of the report. The part error of Mg was about 30%. The actual value of Mg was 601200 J/mol and the experiment we obtained was 420611 J/mol. There could have been homo error in order to obtain the results that could have accounted for the 30% error, although this is not so high. Also, the heat of formation we used was MgO(s) for the actual value, although in the experiment it was a gas. This could have also accounted for some erro r.