Chemistry - Thermochemistry Question with Solution | TestHub
ChemistryThermochemistryBond EnthalpyMedium2 minQB
ChemistryMediumsingle choice
Passage / Comprehension
The bond dissociation enthalpy of the first H-Se bond in hydrogen selenide is 305.0 kJ/mol. The enthalpies of formation of H2Se(g) and Se(g) are +30.0 and 227.0 kJ/mol, respectively. The bond dissociation enthalpy of H-H bond is 436.0 kJ/mol.
The bond dissociation enthalpy of the free radical HSe is
Options:
Answer:
A
Solution:
For the reaction HSe → H + Se, the enthalpy change (ΔH) is calculated as follows:
ΔH = 218 + 227 - 117 = 328 kJ/mol
This corresponds to option (a).
Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Bond Enthalpy
⏱ 2mℹ️ Source: QB
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