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 H2SO4 in n mole of water is given by the equation ΔH = -75n/(n+1.8) kJ/mol. Determine ΔH for the following solutions:
Solution IV: Solution I + 5 moles of water. (Take ΔH as the enthalpy change on adding the 5 moles of water to Solution I.)
Options:
Answer:
D
Solution:
For solution I, with n = 5 moles, the enthalpy is -55.15 kJ.
When 5 additional moles are added, the total number of moles becomes n = 10, and the enthalpy is -63.56 kJ.
The change in enthalpy upon dilution is calculated as the final enthalpy minus the initial enthalpy:
Δ H = -63.56 kJ - (-55.15 kJ) = -8.41 kJ
The correct answer is (d).
Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Enthalpy of solution/dilution/hydration
⏱ 2mℹ️ Source: QB
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