25.00 mL of 0.200 M sulfuric acid was added to 25.00 mL of 0.200 M NAOH, in a constant volume calorimeter. The density of the resulting solution is 1.225 g/mL and its specific heat is 5.321 J/g-°C. As the reaction took place, the temperature of the solution rose from 22.0 °C to 31.3 °C. What is AH (in units of kJ/mol) for the reaction, per mole of water formed? This is a limiting reactant problem and your choice of limiting reactant must be justified through stoichiometric calculations.
25.00 mL of 0.200 M sulfuric acid was added to 25.00 mL of 0.200 M NAOH, in a constant volume calorimeter. The density of the resulting solution is 1.225 g/mL and its specific heat is 5.321 J/g-°C. As the reaction took place, the temperature of the solution rose from 22.0 °C to 31.3 °C. What is AH (in units of kJ/mol) for the reaction, per mole of water formed? This is a limiting reactant problem and your choice of limiting reactant must be justified through stoichiometric calculations.
Chemistry by OpenStax (2015-05-04)
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Chapter5: Thermochemistry
Section: Chapter Questions
Problem 69E: Using the data in Appendix G, calculate the standard enthalpy change for each of the following...
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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.
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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Transcribed Image Text:### Problem Statement:
**Question 21:**
25.00 mL of 0.200 M sulfuric acid was added to 25.00 mL of 0.200 M NaOH, in a constant volume calorimeter. The density of the resulting solution is 1.225 g/mL and its specific heat is 5.321 J/g·°C. As the reaction took place, the temperature of the solution rose from 22.0 °C to 31.3 °C. What is ΔH (in units of kJ/mol) for the reaction, per mole of water formed? This is a limiting reactant problem, and your choice of limiting reactant must be justified through stoichiometric calculations.
**Explanation:**
In this problem, you are provided with the following data:
- Volume of sulfuric acid (H₂SO₄) = 25.00 mL
- Molarity of H₂SO₄ = 0.200 M
- Volume of sodium hydroxide (NaOH) = 25.00 mL
- Molarity of NaOH = 0.200 M
- Density of the resulting solution = 1.225 g/mL
- Specific heat of the solution = 5.321 J/g·°C
- Initial temperature = 22.0 °C
- Final temperature = 31.3 °C
The task is to determine the enthalpy change (ΔH) of the reaction per mole of water produced. This involves performing a stoichiometric calculation to identify the limiting reactant and using the calorimetric data to calculate the enthalpy change.
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