Entropy

Enthalpy, Gibbs Energy, & Entropy Lab Report Student’s Name Institutional Affiliation Course Instructor Date Enthalpy, Gibbs Energy, & Entropy Lab Report PURPOSE The purpose of this experiment was to examine the two forces that drive reactions in nature, which, together, determine whether a reaction will be spontaneous. The general rule is that exothermic reaction, which imply those reactions that give off heat, are favored by nature. Therefore, the first driving force for experiments is whether it is exothermic or endothermic. Exothermic reactions tend to be spontaneous compared to endothermic ones. However, certain endothermic reactions are spontaneous, implying that there is another force that drives such reactions to occur in nature. This second force is entropy, which refers to the measure of the degree of randomness of the particles, such as molecules in a system. Nature favors an increase in entropy. Therefore, reactions that increase the system’s disorder tend to be spontaneous. The goal of this experiment is to test whether endothermic reactions can still be spontaneous and whether those that experience a decrease in their entropy can also be spontaneous. Objectives * To measure enthalpy * To calculate entropy * To calculate Gibbs Energy * To study reactions and determine the driving forces behind the reactions PROCEDURE The system in this experiment will be ammonium chloride (NH4Cl) for reaction 1 and sodium hydroxide (NAOH) for reaction 2. Reaction 1 The experimental procedure as outlined in the laboratory manual was maintained. However, the system used was ammonium chloride (10.215g) in place of ammonium nitrate. Reaction 2 In reaction 2, 5.101g of sodium hydroxide was used and the procedure followed as outlined in the manual. DATA AND OBSERVATIONS The observations for the two reactions are highlighted in the data table below. Reaction 1 Reaction 2 Initial Temp. of Water 22.00C 22.20C Final Temp. 6.50C 67.00C Temp. Change -15.50C 44.80C Weight of NH4Cl and NAOH 1...