Which of CH4(g), C2H2(g), and CH3OH(l) provides the most heat per gram upon combustion and which provides the least? CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ΔH° = -890 kJ 2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(l) ΔH° = -2599 kJ 2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(l) ΔH° = -1453 kJ A) C2H2provides the most heat per gram and CH4the least. B) C2H2provides the most heat per gram and CH3OH the least. C) CH4provides the most heat per gram and CH3OH the least. D) CH4 provides the most heat per gram and C2H2 the least.
Thermochemistry
Thermochemistry can be considered as a branch of thermodynamics that deals with the connections between warmth, work, and various types of energy, formed because of different synthetic and actual cycles. Thermochemistry describes the energy changes that occur as a result of reactions or chemical changes in a substance.
Exergonic Reaction
The term exergonic is derived from the Greek word in which ‘ergon’ means work and exergonic means ‘work outside’. Exergonic reactions releases work energy. Exergonic reactions are different from exothermic reactions, the one that releases only heat energy during the course of the reaction. So, exothermic reaction is one type of exergonic reaction. Exergonic reaction releases work energy in different forms like heat, light or sound. For example, a glow stick releases light making that an exergonic reaction and not an exothermic reaction since no heat is released. Even endothermic reactions at very high temperature are exergonic.
- Which of CH4(g), C2H2(g), and CH3OH(l) provides the most heat per gram upon combustion and which provides the least?
CH4(g) + 2 O2(g) → CO2(g) + 2 H2O(l) ΔH° = -890 kJ
2 C2H2(g) + 5 O2(g) → 4 CO2(g) + 2 H2O(l) ΔH° = -2599 kJ
2 CH3OH(l) + 3 O2(g) → 2 CO2(g) + 4 H2O(l) ΔH° = -1453 kJ
A) C2H2provides the most heat per gram and CH4the least.
B) C2H2provides the most heat per gram and CH3OH the least.
C) CH4provides the most heat per gram and CH3OH the least.
D) CH4 provides the most heat per gram and C2H2 the least.
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