Chemistry - Thermochemistry Question with Solution | TestHub
ChemistryThermochemistryEnthalpy of CombustionMedium2 minQB
ChemistryMediumsingle choice
Passage / Comprehension
Study the following thermochemical equations:
2H2(g) + O2(g) → 2H2O(g); ΔH = -483.636 kJ
3H2(g) + O3(g) → 3H2O(g); ΔH = -868.2 kJ
H2(g) + H2O2(g) → 2H2O(g); ΔH = -347.33 kJ
Which oxidizing agent will generate the greatest amount of energy for 1 mole of H2(g)?
Options:
Answer:
C
Solution:
The energy per mole of H₂ is calculated as follows:
With O₂: 483.636/2 = 241.8 kJ
With O₃: 868.2/3 = 289.4 kJ
With H₂O₂: 347.33 kJ (considering 1 mole of H₂ in the equation).
The greatest energy per mole of H₂ is observed with H₂O₂. Therefore, the answer is (c).
Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Enthalpy of Combustion
⏱ 2mℹ️ Source: QB
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