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 V: solution II + large excess of water.
Options:
Answer:
C
Solution:
Solution II (where n = 10) has an enthalpy of -63.56 kJ. With a large excess of water, the total enthalpy tends toward -75 kJ. The enthalpy change for the dilution step is calculated as:
-75 kJ - (-63.56 kJ) = -11.44 kJ
Therefore, the answer is (c).
Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Enthalpy of solution/dilution/hydration
⏱ 2mℹ️ Source: QB
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