The addition of hydroiodic acid to a silver nitrate solution precipitates silver iodide according to the reaction: AgNO3(aq) + HI(aq) → AgI(s) + HNO3(aq) When 50.0 mL of 5.00x10-2 M AgNO3 is combined with 50.0 mL of 5.00x10-2 M HI in a coffee-cup calorimeter, the temperature changes from 22.40 °C to 22.91 °C. ▼ Part A ↑ Calculate AHxn for the reaction as written. Use 1.00 g/mL as the density of the solution and Cs = 4.18 J/(g. °C) as the specific heat capacity of the solution. Express the energy to two significant figures and include the appropriate units. X 2 AHxn= W 1 # O 3 Value C μÀ E MAR 31 $ 4 R Units % tv 5 G Search or type URL ? T 6 MacBook Pro AO Y & 7 U *00 8 + - ( 9 O R O P A + [ = O delete

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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.    

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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.