A tablespoon (about 15.0 mL) of sodium chloride, a common table salt, is dissolved in water. What is the change in enthalpy (in kJ) of this dissolution process? (dNaCI(s) = 2.16 g cm NaCI(s) + Nat(aa) +CI (aa) AH = 3.87 kJ mol
A tablespoon (about 15.0 mL) of sodium chloride, a common table salt, is dissolved in water. What is the change in enthalpy (in kJ) of this dissolution process? (dNaCI(s) = 2.16 g cm NaCI(s) + Nat(aa) +CI (aa) AH = 3.87 kJ mol
Chapter6: Thermochemistry
Section: Chapter Questions
Problem 104AE
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![A tablespoon (about 15.0 mL) of sodium chloride, a common table salt, is dissolved in water. What
is the change in enthalpy (in kJ) of this dissolution process? (dNaCI(s) = 2.16 g cm)
NaCI(s) –
Na* (aq) + Cl (ag)
-1
AH = 3.87 kJ mol
A: 2.14](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5c58a909-3640-4198-b28f-fcaa04bb7670%2F26d4b4ad-6840-4426-8330-2dbd36277fd7%2Frwqd4e_processed.jpeg&w=3840&q=75)
Transcribed Image Text:A tablespoon (about 15.0 mL) of sodium chloride, a common table salt, is dissolved in water. What
is the change in enthalpy (in kJ) of this dissolution process? (dNaCI(s) = 2.16 g cm)
NaCI(s) –
Na* (aq) + Cl (ag)
-1
AH = 3.87 kJ mol
A: 2.14
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