Two student chemists measured 25.0mL of 1.00 M NaOH in separate calorimeters as in the experimental procedure, Part B. Student 1 added 25.0mL of 1.10 M HCl in his solution of NaOH. Student 2 added 22.7mL of 1.10 M HCl in his NaOH solution. Each student recorded the temperature change and calculated the enthalpy of neutralization. Complete the following table to assist in answering the below questions. NOTE: Limiting reactant needs to be identified to calculate the enthalpy of neutralization. Student 1 Moles of NaOH _________ Moles of HCl added _________ Limiting reactant _________ Moles of H2O produced _________ Mass of final mixture _________ Student 2 Moles of NaOH _________ Moles of HCl added _________ Limiting reactant _________ Moles of H2O produced _________ Mass of final mixture _________ Explain why and how (higher or lower) the temperature will be different for the two students. Explain the predicted enthalpy of neutralization for the two experiments.
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.
- Two student chemists measured 25.0mL of 1.00 M NaOH in separate calorimeters as in the experimental procedure, Part B. Student 1 added 25.0mL of 1.10 M HCl in his solution of NaOH. Student 2 added 22.7mL of 1.10 M HCl in his NaOH solution. Each student recorded the temperature change and calculated the enthalpy of neutralization. Complete the following table to assist in answering the below questions.
NOTE: Limiting reactant needs to be identified to calculate the enthalpy of neutralization.
|
Student 1
Moles of NaOH _________
Moles of HCl added _________
Limiting reactant _________
Moles of H2O produced _________
Mass of final mixture _________
|
Student 2
Moles of NaOH _________
Moles of HCl added _________
Limiting reactant _________
Moles of H2O produced _________
Mass of final mixture _________
|
Explain why and how (higher or lower) the temperature will be different for the two students. Explain the predicted enthalpy of neutralization for the two experiments.
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