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.
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![**Chemical Reaction Energy Calculation**
**Problem Statement:**
What quantity of heat (in kJ) will be released if 1.20 mol of SrO is mixed with 0.951 mol of CO₂ in the following chemical reaction?
\[ \text{SrO (s) + CO}_{2}\text{ (g) } \rightarrow \text{SrCO}_{3}\text{ (s)} \]
**Reaction Enthalpy:**
\[ \Delta H^\circ = -234 \, \text{kJ/mol} \]
**Solution Overview:**
To find the quantity of heat released:
1. Identify the limiting reactant by comparing the mole ratio of the reactants to the stoichiometry of the reaction.
2. Calculate the heat released using the limiting reactant and the given enthalpy change (\( \Delta H^\circ \)).
**Detailed Steps:**
- Stoichiometrically, 1 mole of SrO reacts with 1 mole of CO₂ to form 1 mole of SrCO₃.
- Given 1.20 mol of SrO and 0.951 mol of CO₂, CO₂ is the limiting reactant.
- Using the enthalpy change, the heat released is calculated based on the moles of the limiting reactant:
\[ \text{Heat released} = 0.951 \, \text{mol} \times (-234 \, \text{kJ/mol}) = -222.834 \, \text{kJ} \]
**Conclusion:**
The quantity of heat released in this reaction is 222.834 kJ.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcd9affeb-cb9a-412b-bc87-c009a3e9b5ed%2F6aecae0f-7397-4d26-803e-efeec6689506%2Fa9d7k4c_processed.jpeg&w=3840&q=75)
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