Table 1.2. Enthalpy (Heat) of Neutralization for an Acid-Base ReactionPreliminary DataTrial 1Trial 21. Volume of acid, (mL)50.025.02. Temperature of acid, ("C)20.522.03. Volume of NaOH, (mL)25.050.04.Temperature of N2OH, (C)23.020.05. Maximum temperature of solution incalorimeter, (final temperature of solution,°C)22.225.06. Concentration of N2OH & HCI (M, mol/L)0.100.15Calculated Data1. Average initial temperature of NaOH andacid, (C)2. Temperature change, (C)3. Final volume of mixture, (mL)4. Mass of final mixture, (g, assume density of1.0 g/mL)5. Specific Heat of Mixture, (J/g-"C)4.1844.1846. Heat evolved, ()7. Moles of OH H reacted, (mol, whicheveris 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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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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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Concept explainers

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

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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Standard Enthalpy of Reaction 33 of 42 Learning Goal: To understand how standard enthalpy of reaction is related to the standard heats of formation of the reactants and products. Constants Periodic Table In a generic chemical reaction involving reactants A and B and products C and D, aA + bB-cC + dD, the standard enthalpy AHn of the reaction is given by The standard enthalpy of reaction is the enthalpy change that occurs in a reaction when all the reactants and products are in their standard states. The symbol for the standard enthalpy of reaction is AHn, where the subscript "rxn" stands for "reaction." The standard enthalpy of a reaction is calculated from the standard heats of formation ( AH) (subscript "f" for formation) of its reactants and products. Therefore, the standard enthalpy AHn of any reaction can be mathematically determined, as long as the standard heats of formation (AH:) of its reactants and products are AH = cAH¿ (C) + dAH; (D) -aAH; (A) – bAH (B) Notice that the…
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