A reaction between Mg and aqueous hydrochloric acid was performed to determine the heat of the reaction. A calorimeter with a heat capacity of 6.5 J/K was used. To the calorimeter 50.0 mL of 1.0 M HCl was added, the initial temperature was recorded and then 0.250 g of magnesium metal was added. The final temperature was then recorded. (Assume density of the solution is 1.03 g/mL; q = mcAT; molar mass Mg = 24.31 g/mol; specific heat capacity of water = 4.184 J/g.K; q calorimeter = heat capacity x AT). The following data was recorded:Initial temperature:21.5°C ; Final Temperature: 45.1°c Calculate q calorimeter (J) q solution (J) total amount of heat released (J), mol Mg, enthalpy of reaction in kJ/molor (q total/mol Mg). Just put the numerical values since units are already indicated. For the question, amount of heat released, there is no need to put the negative sign.
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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