Chemistry - Thermochemistry Question with Solution | TestHub
ChemistryThermochemistryEnthalpy of CombustionMedium2 minQB
ChemistryMediumsingle 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 of the reaction will generate the least amount of energy on a total mass basis of reactants?
Options:
Answer:
C
Solution:
Total reactant mass: CO-O2: 56 + 32 = 88 g, giving 566/88 = 6.43 kJ/g. CO-N2O: 28 + 44 = 72 g, giving 366/72 = 5.08 kJ/g. CO-NO2: 28 + 46 = 74 g, giving 226/74 = 3.05 kJ/g. The least is CO-NO2. Ans (c).
Stream:JEESubject:ChemistryTopic:ThermochemistrySubtopic:Enthalpy of Combustion
⏱ 2mℹ️ Source: QB
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