Q5Multiple choice
During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is –1
- (i)2C4H10(g) + 13O2(g) → 8CO2(g) + 10H2O( l ) ∆cH = –2658.0 kJ mol 13 –1
- (ii)C4H10(g) + O (g) → 4CO2 (g) + 5H2O (g) ∆cH = –1329.0 kJ mol 2 2 13 –1
- (iii)C4H10(g) + O (g) → 4CO2 (g) + 5H2O ( l ) ∆cH = –2658.0 kJ mol 2 2 13 –1
- (iv)C4H10 (g) + O (g) → 4CO2 (g) + 5H2O ( l ) ∆cH = +2658.0 kJ mol 2 2
Show answer
(iii) C4H10(g) + O (g) → 4CO2 (g) + 5H2O ( l ) ∆cH = –2658.0 kJ mol 2 2 13 –1