The molar enthalpy change for the neutralization reaction: HCl(aq)+NaOH(aq)⟶NaCl(aq)+H2O(l) is ΔrH° = -57.3 kJ/mol. Imagine you mix 60.7 mL of 1.00 M HCl with 75.9 mL of 1.00 M NaOH in a beaker at 24.1 °C. Calculate the final temperature of the solution after the reaction has gone to completion. You will need to assume no heat is lost to the environment, the density of the reaction solution is the same as water, 1.00 g/mL, and the specific heat capacity of the reaction solution is the same as of water, 4.184 J/g°C. Final temperature (°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.
The molar enthalpy change for the neutralization reaction:
is ΔrH° = -57.3 kJ/mol. Imagine you mix 60.7 mL of 1.00 M HCl with 75.9 mL of 1.00 M NaOH in a beaker at 24.1 °C. Calculate the final temperature of the solution after the reaction has gone to completion. You will need to assume no heat is lost to the environment, the density of the reaction solution is the same as water, 1.00 g/mL, and the specific heat capacity of the reaction solution is the same as of water, 4.184 J/g°C.
Final temperature
(°C)?
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