A quantity of 1.00 x 102 mL of 0.500 M HCl was mixed with 1.00 x 102 mL of 0.500 M NaOH in a constant pressure calorimeter of negligible heat capacity. The initial temperature of the HCL and NaOH solutions was same, 22.50 0C, and the final temperature of the mixed solution was 25.86 0C. Calculate the (a) heat of the reaction at constant pressure (qp) and (b) the change in enthalpy for the neutralization reaction (ΔHrxn) in kJ per mole of HCl. Assume that the densities and specific heat of the solutions are the same as for water (1.00 g/mL and 4.184 J/g.0C, respectively). NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)
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.
A quantity of 1.00 x 102 mL of 0.500 M HCl was mixed with 1.00 x 102 mL of 0.500 M NaOH
in a constant pressure calorimeter of negligible heat capacity. The initial temperature of the HCL
and NaOH solutions was same, 22.50 0C, and the final temperature of the mixed solution was
25.86 0C. Calculate the (a) heat of the reaction at constant pressure (qp) and (b) the change in
enthalpy for the neutralization reaction (ΔHrxn) in kJ per mole of HCl. Assume that the densities
and specific heat of the solutions are the same as for water (1.00 g/mL and
4.184 J/g.0C, respectively).
NaOH(aq) + HCl(aq) → NaCl(aq) + H2O(l)
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