Ncert Exercises & Solutions

During the complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for this change is:

1.	$2 C_{4} H_{10} (g) + 13 O_{2} (g) \to 8 {CO}_{2} (g) + 10 H_{2} O (l);$ $∆_{c} H = - 2658.0 kJ {mol}^{- 1}$
2.	$C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 {CO}_{2} (g) + 5 H_{2} O (l);$ $∆_{c} H = - 1329.0 kJ {mol}^{- 1}$
3.	$C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 {CO}_{2} (g) + 5 H_{2} O (l);$ $∆_{c} H = - 2658.0 kJ {mol}^{- 1}$
4.	$C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 {CO}_{2} (g) + 5 H_{2} O (l);$ $∆_{c} H = + 2658.0 kJ {mol}^{- 1}$