Coffee cup calorimetry experiments can be used to obtain DHfo for magnesium oxide. To determine the heat capacity of the calorimeter, 49.6 mL of 1.01M HCl are reacted with 50.1 mL of 0.998M NaOH: HCl(aq) + NaOH(aq) --> NaCl(aq) + H2O(l). The solution’s temperature increases by 6.40 oC. Determine the heat capacity of the calorimeter. Assume that the solution’s specific heat is 4.025 J/g*oC and the enthalpy of neutralization is -55.9 kJ/mol of H2O. Assume that the density of the solution is 1.00 g/mL. Correct answer is 35.5 J/oC. Please show your work on how you get to this answer and explain your reasoning for the steps and calculation you take. For example, why do you use delta H to help solve the problem?
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.
Coffee cup calorimetry experiments can be used to obtain DHfo for magnesium oxide. To determine the heat capacity of the calorimeter, 49.6 mL of 1.01M HCl are reacted with 50.1 mL of 0.998M
NaOH: HCl(aq) + NaOH(aq) --> NaCl(aq) + H2O(l).
The solution’s temperature increases by 6.40 oC. Determine the heat capacity of the calorimeter.
Assume that the solution’s specific heat is 4.025 J/g*oC and the enthalpy of neutralization is -55.9 kJ/mol of H2O. Assume that the density of the solution is 1.00 g/mL.
Correct answer is 35.5 J/oC. Please show your work on how you get to this answer and explain your reasoning for the steps and calculation you take. For example, why do you use delta H to help solve the problem?
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