Table 1.2. Enthalpy (Heat) of Neutralization for an Acid-Base Reaction Preliminary Data Trial 1 Trial 2 1. Volume of acid, (mL) 50.0 25.0 2. Temperature of acid, (°C) 20.5 22.0 3. Volume of N2OH, (mL) 25.0 50.0 4.Temperature of NaOH, CC) 23.0 20.0 5. Maximum temperature of solution in calorimeter, (final temperature of solution, *C) 222 25.0 6. Concentration of NaOH & HC1 (M, mol L) Calculated Data 1. Average initial temperature of N2OH and acid, ("C) 2. Temperature change, ("C) 3. Final volume of mixture, (mL.) 4. Mass of final mixture, (E, assume density of 1.0 g/mL.) 5. Specific Heat of Mixture, (J/g-"C) 4.184 4.184 6. Heat evolved, (1) 7. Moles of OH H' reacted, (mol, whichever is the limiting reactant) 8. Moles of H.O formed, (mol) 9. AH.4 (kJ/mol H;O) 10. Average AH, (kJ/mol HO) ||
Table 1.2. Enthalpy (Heat) of Neutralization for an Acid-Base Reaction Preliminary Data Trial 1 Trial 2 1. Volume of acid, (mL) 50.0 25.0 2. Temperature of acid, (°C) 20.5 22.0 3. Volume of N2OH, (mL) 25.0 50.0 4.Temperature of NaOH, CC) 23.0 20.0 5. Maximum temperature of solution in calorimeter, (final temperature of solution, *C) 222 25.0 6. Concentration of NaOH & HC1 (M, mol L) Calculated Data 1. Average initial temperature of N2OH and acid, ("C) 2. Temperature change, ("C) 3. Final volume of mixture, (mL.) 4. Mass of final mixture, (E, assume density of 1.0 g/mL.) 5. Specific Heat of Mixture, (J/g-"C) 4.184 4.184 6. Heat evolved, (1) 7. Moles of OH H' reacted, (mol, whichever is the limiting reactant) 8. Moles of H.O formed, (mol) 9. AH.4 (kJ/mol H;O) 10. Average AH, (kJ/mol HO) ||
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions
Section: Chapter Questions
Problem 113SCQ
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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.
Question
Transcribed Image Text:Table 1.2. Enthalpy (Heat) of Neutralization for an Acid-Base Reaction
Preliminary Data
Trial 1
Trial 2
1. Volume of acid, (mL)
50.0
25.0
2. Temperature of acid, ("C)
20.5
22.0
3. Volume of NaOH, (mL)
25.0
50.0
4.Temperature of N2OH, (C)
23.0
20.0
5. Maximum temperature of solution in
calorimeter, (final temperature of solution,
°C)
22.2
25.0
6. Concentration of N2OH & HCI (M, mol/L)
0.10
0.15
Calculated Data
1. Average initial temperature of NaOH and
acid, (C)
2. Temperature change, (C)
3. Final volume of mixture, (mL)
4. Mass of final mixture, (g, assume density of
1.0 g/mL)
5. Specific Heat of Mixture, (J/g-"C)
4.184
4.184
6. Heat evolved, ()
7. Moles of OH H reacted, (mol, whichever
is the limiting reactant)
8. Moles of H.O formed, (mol)
9. AH (kJ/mol H:O)
10. Average AH, (kJ/mol H.O)
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