You were tasked to do a simple calorimetry experiment to determine the enthalpy of reaction of HNO3 and NaOH for your experiment in you Chem 16.1 Lab class. The method found in the lab manual was the one used for this experiment. The results, including for the calibration of the calorimeter using HCl and NaOH, are shown in your data sheet below. Complete your data sheet. CALORIMETRY DATA I. CALIBRATION OF CALORIMETER Molarity of HCI, M 1.00 Volume of HCI, mL 10.0 Molarity of NaOH, M 1.00 Volume of NaOH, mL 5.00 Initial Temperature (°C) 26.7 Temperature of mixture (°C) vs. Time (sec) 30 29 28 27 26 25 50 100 150 200 Time (sec) Temperature of mixture |(°C) Time (sec) 26.7 30 60 90 27.8 28.8 28.8 28.8 28.8 120 150 180 28.8 210 28.6 Temperature of mixture (°C)
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.
use the data in the first photo to solve for the unknowns in the 2nd photo
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