Chemistry - Thermochemistry Question with Solution | TestHub
ChemistryThermochemistryEnthalpy of solution/dilution/hydrationEasy2 minQB
ChemistryEasysingle 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 V: solution II + large excess of water. (Take ΔH as the enthalpy change of this dilution step.)
Options:
Answer:
C
Solution:
Solution II (where n = 17) has an enthalpy of -51.0 kJ. With a large excess of water, the total enthalpy tends toward -60 kJ. The enthalpy change for the dilution step is calculated as:
-60 kJ - (-51.0 kJ) = -9.0 kJ
Thus, the answer is (c).
Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Enthalpy of solution/dilution/hydration
⏱ 2mℹ️ Source: QB
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