Chemistry - Thermochemistry Question with Solution | TestHub
ChemistryThermochemistryEnthalpy of solution/dilution/hydrationMedium2 minQB
ChemistryMediumsingle choice
Passage / Comprehension
The integral enthalpy of solution of one mole of CaCl2 in n mole of water is given by the equation ΔH = -60n/(n+3) kJ/mol. Determine ΔH for the following solutions:
Solution IV: Solution I + 9 moles of water. (Take ΔH as the enthalpy change on adding the 9 moles of water to Solution I.)
Options:
Answer:
B
Solution:
Solution I has n = 6 moles, with a ΔH = -40.0 kJ. Adding 9 more moles results in a total of n = 15 moles. The new enthalpy change is calculated as ΔH = -900/18 = -50.0 kJ. Therefore, the enthalpy change for the dilution step is -50.0 - (-40.0) = -10.0 kJ. The answer is (b).
Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Enthalpy of solution/dilution/hydration
⏱ 2mℹ️ Source: QB
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