When 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M HClare mixed in a constant-pressure calorimeter, the temperatureof the mixture increases from 22.30 to 23.11 °C. The temperatureincrease is caused by the following reaction:AgNO31aq2 + HCl1aq2 ¡A gCl1s2 + HNO31aq2Calculate ΔH for this reaction in kJ>mol AgNO3, assumingthat the combined solution has a mass of 100.0 g and a specificheat of 4.18 J>g@°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.
When 50.0 mL of 0.100 M AgNO3 and 50.0 mL of 0.100 M HCl
are mixed in a constant-pressure calorimeter, the temperature
of the mixture increases from 22.30 to 23.11 °C. The temperature
increase is caused by the following reaction:
AgNO31aq2 + HCl1aq2 ¡A gCl1s2 + HNO31aq2
Calculate ΔH for this reaction in kJ>mol AgNO3, assuming
that the combined solution has a mass of 100.0 g and a specific
heat of 4.18 J>g@°C.
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