[Reférénces] When 23.6 g of calcium chloride, CaCl2, was dissolved in water in a constant-pressure calorimeter, the temperature rose from 25.0°C to 38.7°C. If the heat capacity of the solution and the calorimeter is 1258 J/C, what is the enthalpy change when 1.21 mol of calcium chloride dissolves in water? The solution process is CaCl, (s) - Ca2+ (aq) + 2Cl (ag) Enthalpy change = kJ Submit Answer Try Another Version 1 item attempt remaining
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.
![**Calorimetry and Enthalpy Change**
When 23.6 g of calcium chloride, CaCl₂, was dissolved in water in a constant-pressure calorimeter, the temperature rose from 25.0°C to 38.7°C. If the heat capacity of the solution and the calorimeter is 1258 J/°C, what is the enthalpy change when 1.21 mol of calcium chloride dissolves in water? The solution process is
\[ \text{CaCl}_2(s) \rightarrow \text{Ca}^{2+}(aq) + 2\text{Cl}^-(aq) \]
Enthalpy change = \_\_\_\_ kJ
**Instructions:**
To find the enthalpy change, you can use the formula:
\[ q = C \times \Delta T \]
where \( q \) is the heat absorbed or released, \( C \) is the heat capacity, and \( \Delta T \) is the change in temperature. Then, convert the heat energy to enthalpy change per mole of solute dissolved.
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