A student dissolves 12.4 g of sodium hydroxide (NaOH) in 200. g of water in a well-insulated open cup. She then observes the temperature of the wate rise from 21.0 °C to 38.8 °C over the course of 3.2 minutes. Use this data, and any information you need from the ALEKS Data resource, to answer the questions below about this reaction: NaOH(s) - Na (aq) + OH¯(aq) You can make any reasonable assumptions about the physical properties of the solution. Be sure answers you calculate using measured data are rounded 3 significant digits. Note for advanced students: it's possible the student did not do the experiment carefully, and the values you calculate may not be the same as the know and published values for this reaction. O exothermic Is this reaction exothermic, endothermic, or neither? endothermic O neither If you said the reaction was exothermic or endothermic, calculate the amount of heat that was released or absorbed by the reaction in this case. kJ Calculate the reaction enthalpy AH per mole of NaOH. rxn mol

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Thermochemistry

Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.    

Exergonic Reaction

The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.