A student mixes 67.0 mL of a 2.01 M sodium hydroxide solution with 23.2 mL of 6.45 M hydrochloric acid. The temperature of the mixture rises 24.4°C. The density of the resulting solution is 1.00 g/mol and has a specific heat capacity of 4.184 J/g*°C. The heat capacity of the calorimeter is 16.97 J/°C. Part 1 (a) Identify the limiting reagent for the reaction. ________ Part 2 (b) Calculate the heat of reaction (in J). Enter your answer in scientific notation. qrxn=_____ x 10__ Part 3 (c) Find the enthalpy of neutralization (in kJ/mol). ΔHneutralization = _________ kJ/mol
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.
Part 1
(a) Identify the limiting reagent for the reaction.
(b) Calculate the heat of reaction (in J). Enter your answer in scientific notation.
(c) Find the enthalpy of neutralization (in kJ/mol).
ΔHneutralization = _________ kJ/mol
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