Which of CH4(g), C2H2(g), and CH3OH(l) provides the most energy ...

[jeatrice]

Question 1

The heat of combustion per mole for acetylene, C2H2(g), is -1299.5 kJ/mol. Assuming that the combustion products are CO2(g) and H2O(l), and given that the enthalpy of formation is -393.5 kJ/mol for CO2(g) and -285.8 kJ/mol for H2O(l), find the enthalpy of formation of C2H2(g).
◦ -226.7 kJ/mol
◦ -846.1 kJ/mol
◦ -620.2 kJ/mol
◦ +226.7 kJ/mol

Question 2

Which of CH4(g), C2H2(g), and CH3OH(l) provides the most energy 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

◦ C2H2 provides the most energy per gram and CH3OH the least.
◦ CH4 provides the most energy per gram and C2H2 the least.
◦ CH4 provides the most energy per gram and CH3OH the least.
◦ C2H2 provides the most energy per gram and CH4 the least.

[Zebsrer]

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