At 298 K, the standard enthalpies of formation for C2H2(g) and C6H6(l) are 227 kJ mol and 49 kJ mol, respectively a Calculate Ho for C6H6(l) 3C2H2(g) b Both acetylene (C2H2) and benzene (C6H6) can be used as fuels Which compound would liberate more energy per gram when combusted in air ...

a H 3 mol227 kJmol 1 mol49 kJmol ...

At 298 K, the standard enthalpies of formation for C2H2(g) and C6H6(l) are 227 kJ/ mol and

Question:

At 298 K, the standard enthalpies of formation for C2H2(g) and C6H6(l) are 227 kJ/ mol and 49 kJ/ mol, respectively.
a. Calculate ΔHo for C6H6(l) → 3C2H2(g)
b. Both acetylene (C2H2) and benzene (C6H6) can be used as fuels.
Which compound would liberate more energy per gram when combusted in air?