The aluminum cup inside your calorimeter weighs 41.55 g. You add 59.21 g of 1.0 M acetic acid solution and 50.03 g of 1.0 M sodium hydroxide solution to the calorimeter. Both solutions have an initial temperature of 19.9 oC, and the final temperature after addition is 26.8 oC. What is the molar enthalpy of neutralization, in units of kJ/mol? Assume that: the calorimeter is completely insulated the heat capacity of the empty calorimeter is the heat capacity of the aluminum cup: 0.903 J g-1 oC-1. the density of the two solutions is the same as that of water: 1.00 g/mL. the heat capacity of the two solutions is the same as that of water: 4.184 J g-1 oC-1. Perform all calculations without rounding, but then provide your answer to the correct number of significant figures.
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 aluminum cup inside your calorimeter weighs 41.55 g. You add 59.21 g of 1.0 M acetic acid solution and 50.03 g of 1.0 M sodium hydroxide solution to the calorimeter. Both solutions have an initial temperature of 19.9 oC, and the final temperature after addition is 26.8 oC. What is the molar enthalpy of neutralization, in units of kJ/mol?
Assume that:
- the calorimeter is completely insulated
- the heat capacity of the empty calorimeter is the heat capacity of the aluminum cup: 0.903 J g-1 oC-1.
- the density of the two solutions is the same as that of water: 1.00 g/mL.
- the heat capacity of the two solutions is the same as that of water: 4.184 J g-1 oC-1.
Perform all calculations without rounding, but then provide your answer to the correct number of significant figures.
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