During complete combustion of one mole of butane- 2658 kJ of heat is released- The thermochemical reaction for above change isa 2 C 4 H 10 g -13 O 2 g - 8 CO 2 g -10 H 2 O l - - c H -2658-0 kJ mol -1b C 4 H 10 g -13-2 O 2 g - 4 CO 2 g -5 H 2 O 1 - - c H -1329-0 kJ mol -1c C 4 H 10 g -13-2 O 2 g - 4 CO 2 g -5 H 2 O 1 - - c H -2658-0 kJ mol -1d C 4 H 10 g - m -2 O 2 g - 4 CO 2 g -5 H 2 O 1 - - c H -2658-0 kJ mol -1

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Heat of Reaction

During comple...

Question

During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is
(a) $2 C_{4} H_{10} (g) + 13 O_{2} (g) \to 8 C O_{2} (g) + 10 H_{2} O (l); Δ_{c} H = - 2658.0 k J m o l^{- 1}$
(b) $C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l); Δ_{c} H = - 1329.0 k J m o l^{- 1}$
(c) $C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l); Δ_{c} H = - 2658.0 k J m o l^{- 1}$
(d) $C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l); Δ_{c} H = + 2658.0 k J m o l^{- 1}$

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C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) ⟶ 4 C O_{2} (g) + 5 H_{2} O (l); Δ H = - 2878 k J

Δ H

1 a t m

298 K

C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l) △ G^{\circ} = - 2746 k J / m o l

E^{\circ}

C_{4} H_{10} (g) + \frac{13}{2} O_{2} (g) \to 4 C O_{2} (g) + 5 H_{2} O (l)

Δ G^{\circ} = - 2746 kJ/mol

E^{\circ}

2658 k J

1 b a r

298 K

C_{4} H_{10} (g) + 6.5 O_{2} (g) ⟶ 4 C O_{2} (g) + 5 H_{2} O (l); △_{r} G^{\circ} = - 2746 k J / m o l

E^{\circ}

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