# Post Lab Problem 1) 66.667 ml of 3.000 M

Experiment 7: Enthalpy of ReactionName: Student ID #2Objective: To determine the heat and enthalpy of neutralization reaction Background: During the metathesis between an acid and base in addition to water and saltenergy is also released. Such processes where system gives off heat to its surroundings is calledan exothermic process. During an exothermic chemical reaction the internal energy of products isless than that of reactants. That being said, the stability of the products should be higher than thestability of the reactants. This stability difference can be simply related to the difference in thestored chemical potential energies, in term of chemical bondings. In this experiment the heat ofreaction, which will be measured in constant pressure will guide us to estimate enthalpy ofneutralization reaction: mm) + OH’taq) -> H20 (0 Materials:NaOH (aq) HCl (all) PipetteStyrofoam Coffee Cup Thermometer *Warning: Please note that the acid and base are corrosive and you need to avoid any directcontact. Procedure: *In this experiment you will use Styrofoam coffee cup as your insulated calorimeter. The cupwhich has a whole at its bottom will be used as the lid, through which the thermometer will be inserted to the solution. “We make the assumption that the density and speciﬁc heat capacity of the solution is 1.00g/ml and 4.18 J/g oC. “*We make the assurnption that the Styrofoam cup doesn’t absorb any heat. 1) Pipette 50.0 ml of your 1.0!! M HCl solution into yourStyrofoam cup. IE—E]2) Pipette 75.0 ml of your 1.05 M NaOH solution into a very cleanbeaker. 3) Measure the temperatures of both solutions to 0.1 ”C. Note thatthese temperatures are expected to be similar to each other and tothe room temperature. 4) Add the NaOH solution to the cotfee cup (containinghydrochloric acid) at once and read the temperature while gentlystirring the solution. 5) Record the highest temperature that you observed after mixing