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The lattice enthalpy of sodium chloride, AH° for NaCl(s) → Na* (9) + Cl¯(g) is 787 kJ/mol; the heat of solution in making up 1 M NaCI(ag) is +4.0 kJ/mol. From these data, obtain the sum of the heats of hydration of Na+ and Cl¯, That is, obtain the sum of AH° values for Na+ (g) → Na+ (ag) Cl (g) → Cl¯(aq) ΔΗ kJ/mol If the heat of hydration of CI is –338 kJ/mol, what is the heat of hydration of Nat? Heat of hydration = kJ/mol

The lattice enthalpy of sodium chloride, AH° for NaCl(s) → Na* (9) + Cl¯(g) is 787 kJ/mol; the heat of solution in making up 1 M NaCI(ag) is +4.0 kJ/mol. From these data, obtain the sum of the heats of hydration of Na+ and Cl¯, That is, obtain the sum of AH° values for Na+ (g) → Na+ (ag) Cl (g) → Cl¯(aq) ΔΗ kJ/mol If the heat of hydration of CI is –338 kJ/mol, what is the heat of hydration of Nat? Heat of hydration = kJ/mol

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter12: Solutions
Section: Chapter Questions
Problem 12.62QE
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The lattice enthalpy of sodium chloride, AH° for NaCl(s) → Na* (9) + Cl¯(g) is 787 kJ/mol; the heat of solution in making up 1 M NaCI(ag) is +4.0 kJ/mol. From these data, obtain the sum of the heats of hydration of Na+ and Cl¯, That is, obtain the sum of AH° values for Na+ (g) → Na+ (ag) Cl (g) → Cl¯(aq) ΔΗ kJ/mol If the heat of hydration of CI is –338 kJ/mol, what is the heat of hydration of Nat? Heat of hydration = kJ/mol
Transcribed Image Text:The lattice enthalpy of sodium chloride, AH° for NaCl(s) → Na* (9) + Cl¯(g) is 787 kJ/mol; the heat of solution in making up 1 M NaCI(ag) is +4.0 kJ/mol. From these data, obtain the sum of the heats of hydration of Na+ and Cl¯, That is, obtain the sum of AH° values for Na+ (g) → Na+ (ag) Cl (g) → Cl¯(aq) ΔΗ kJ/mol If the heat of hydration of CI is –338 kJ/mol, what is the heat of hydration of Nat? Heat of hydration = kJ/mol
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