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 g of oxidizing agent?
Options:
Answer:
B
Solution:
Per mole of oxidizing agent: O₂: 483.636 kJ (32 g), O₃: 868.2 kJ (48 g), H₂O₂: 347.33 kJ (34 g).
To determine the greatest oxidizing agent per gram, we calculate the energy released per gram for each:
For O₂: 483.636 / 32 = 15.11 kJ/g
For O₃: 868.2 / 48 = 18.09 kJ/g
For H₂O₂: 347.33 / 34 = 10.22 kJ/g
Comparing these values, O₃ has the greatest energy release per gram. The answer is (b).
Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Enthalpy of Combustion
⏱ 2mℹ️ Source: QB
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