Limestone stalactites and stalagmites are formed in caves by the following reaction: Ca2+(aq)+2HCO−3(aq)→CaCO3(s)+CO2(g)+H2O(l)Ca2+(aq)+2HCO3−(aq)→CaCO3(s)+CO2(g)+H2O(l) If 1 molmol of CaCO3CaCO3 forms at 298 KK under 1 atmatm pressure, the reaction performs 2.47 kJkJ of P−VP−V work, pushing back the atmosphere as the gaseous CO2CO2 forms. At the same time, 38.75 kJkJ of heat is absorbed from the environment. What is the value of ΔHΔH for this reaction? Express your answer using four significant figures.
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.
Limestone stalactites and stalagmites are formed in caves by the following reaction:
Ca2+(aq)+2HCO−3(aq)→CaCO3(s)+CO2(g)+H2O(l)Ca2+(aq)+2HCO3−(aq)→CaCO3(s)+CO2(g)+H2O(l)
If 1 molmol of CaCO3CaCO3 forms at 298 KK under 1 atmatm pressure, the reaction performs 2.47 kJkJ of P−VP−V work, pushing back the atmosphere as the gaseous CO2CO2 forms. At the same time, 38.75 kJkJ of heat is absorbed from the environment.
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