Enthalpy change for one mole, (AH) -58.3 kj mol Density 1 M NaCl, (4) 1.037 g mL Specific heat of 1 M NaCl solution, (C) 3.90 Jg' K Molarity of sodium hydroxide g and hydrochloric acidjg used, (c) 2.0 mol L Volume of each of sodium hydroxide,ag and hydrochloric acid,g Used, (V) 25.0 ml Average neutralisation temperature rise, (AT) 11.8 °C Unrounded Rounded Calculation Equation value value Moles of H,0 produced, (n) M(mal) = C(mol L-1) × V(1) 0.050 Enthalpy change for the reaction, (A,H A,H) = "(ma) × AH(J mol") -2.9150 -2.9 Enthalpy change for the corresponding temperature change, (A,H) A,H(u) = -A, H(a) 2.9150 2.9 m«) = V(mL) × Ple ml-1) 51.9 51.850 Mass of solution, (m) 51.850 Heat capacity of the solution, ( Caberimeter) Culta (J K-') = m(a) × Cur'k-") 202.2150 202 Heat capacity of the calorimeter, ( Calorimeter(: (J K-1) Cuwita ΔΤ
Enthalpy change for one mole, (AH) -58.3 kj mol Density 1 M NaCl, (4) 1.037 g mL Specific heat of 1 M NaCl solution, (C) 3.90 Jg' K Molarity of sodium hydroxide g and hydrochloric acidjg used, (c) 2.0 mol L Volume of each of sodium hydroxide,ag and hydrochloric acid,g Used, (V) 25.0 ml Average neutralisation temperature rise, (AT) 11.8 °C Unrounded Rounded Calculation Equation value value Moles of H,0 produced, (n) M(mal) = C(mol L-1) × V(1) 0.050 Enthalpy change for the reaction, (A,H A,H) = "(ma) × AH(J mol") -2.9150 -2.9 Enthalpy change for the corresponding temperature change, (A,H) A,H(u) = -A, H(a) 2.9150 2.9 m«) = V(mL) × Ple ml-1) 51.9 51.850 Mass of solution, (m) 51.850 Heat capacity of the solution, ( Caberimeter) Culta (J K-') = m(a) × Cur'k-") 202.2150 202 Heat capacity of the calorimeter, ( Calorimeter(: (J K-1) Cuwita ΔΤ
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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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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Transcribed Image Text:Enthalpy change for one mole, (AH)
-58.3 k) mol-1
Density 1 M NaCI, (p)
1.037 g mL-1
6,
Specific heat of 1 M NaCl solution, (C')
3.90 Jg1 K-1
Molarity of sodium hydroxide ag) and hydrochloric acid(aq) used, (c)
2.0 mol L-1
Volume of each of sodium hydroxide(ag) and hydrochloric acid(aq) used, (V)
25.0 mL
Average neutralisation temperature rise, (AT)
11.8 °C
Unrounded
Rounded
Calculation
Equation
value
value
Moles of H20 produced, (n)
n(mol)
C(mol L-1) × V(L)
0.050
Enthalpy change for the reaction, (A„H
A,H(kJ)
n(mol) X AH(kJ mol-1)
-2.9150
-2.9
Enthalpy change for the corresponding
A;H(k) = -A,H (kJ)
2.9150
2.9
temperature change, (A¿H)
51.9
Mass of solution, (m)
m(3) = V(mL)
P(g mL-1)
51.850
51.850
Heat capacity of the solution, (
Csoltn (J K-1) = m(3) × C(Jg-1K-1)
202.2150
202
Ccalorimeter)
Heat capacity of the calorimeter, (
´calorimeter (J K-1)
Csoltn
4
Cealorimeter)
AT
2.
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