Chemistry - Thermochemistry Question with Solution | TestHub
ChemistryThermochemistryEnthalpy of CombustionHard2 minQB
ChemistryHardsingle choice
Passage / Comprehension
Study the following thermochemical equations:
2CO(g) + O2(g) → 2CO2(g); ΔH = -566 kJ
CO(g) + N2O(g) → CO2(g) + N2(g); ΔH = -366 kJ
CO(g) + NO2(g) → CO2(g) + NO(g); ΔH = -226 kJ
(Relative atomic masses: C = 12, N = 14, O = 16)
Which oxidizing agent will generate the greatest amount of energy for 1 g of oxidizing agent?
Options:
Answer:
A
Solution:
Per mole of oxidizing agent: O2 566 kJ (32 g), N2O 366 kJ (44 g), NO2 226 kJ (46 g). Per gram: 566/32 = 17.69, 366/44 = 8.32, 226/46 = 4.91 kJ/g. The greatest is O2. Ans (a).
Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Enthalpy of Combustion
⏱ 2mℹ️ Source: QB
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