During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemica...
During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is
(a) 2 C_4H_10( g)+13 O_2 (g) → 8 CO_2( g)+10 H_2O(l)
Δ_cH=-2658.0 kJ mol^-1
(b) C_4H_10( g)+13/2O_2( g) → 4 CO_2( g)+5 H_2O (g)
Δ_cH=-1329.0 kJ mol^-1
(c) C_4H_10( g)+13/2O_2( g) → 4 CO_2( g)+5 H_2O(l)
Δ_cH=-2658.0 kJ mol^-1
(d) C_4H_10( g)+13/2O_2( g) → 4 CO_2 (g) +5 H_2O(l)
Δ_cH=+2658.0 kJ mol^-1
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