Chemistry 1 Lab Report

Experiment 12 Calorimetry and Hesss virtue Purpose The purpose of this lab is to resolve the enthalpy of chemical chemical reaction for the burning of 1 mole of magnesium in oxygen. Although the reaction is exothermic, the ? HRXN will be determined by using calorimetry and then using Hesss Law to manipulate the data roll up to yield the answer needed. Procedures Dillon, Stephanie. Calorimetry and Hesss Law. laboratory Manual. Pearson Publishing, 2012, pp. 168-177. Data and Results type A account book of cold weewee 49. 9 mL Temperature of cold piss (in loving cupful) 23. 50 C tidy sum of lively body of water 49. 9 mL Temperature of hot water(in cup) 550 CPart A Calculations cud of cold water 49. 9 g Tf from represent 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 Description of sample Metal fizzed when fade come in in HCl Volume of HCl atomic number 6 mL Initial Temperature 220 C Mass of Mg 0. 1485 g Part B Calculations Tf from represent 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 reply 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 Net Equation 2HCl(aq) + MgO(s)MgCl2(aq) + H2O(l) Calculations Conclusion In this experiment we had to abide by the rage ability of the calorimeter cup using two trials of hot and cold water. When we obtained the data after 10 minutes of recording 30 endorsement intervals of the calorimeter cup temperature, we created a line graph to show the trend line.Read this get along Test Chem 105With the trend line, we could figure out the final temperature and delta H in the process. With the comparability 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 burn find the heat of reaction of the cup and multiply 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 use Hesss Law, which is shown in the calculations division. tout ensemble the data is in the data section of the report. The percent error of Mg was to the highest degree 30%. The actual value of Mg was 601200 J/mol and the experiment we obtained was 420611 J/mol. There could present been human 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, al though in the experiment it was a gas. This could have also accounted for some error.