Question

During complete combustion of one mole of butane,
2658 kJ of heat is released. The thermochemical reaction for
above change is
(a) 2C₄H₁₀ (g) +13O₂ (g) → 8CO₂ (g) +10H₂O(1);
∆꜀H = -2658.0 kJ mol⁻¹
(b) C₄H₁₀ (g) + 13/2 O₂ (g) → 4CO₂ (g) + 5H₂O(1);
∆꜀H = -1329.0 kJ mol⁻¹
(c) C₄H₁₀ (g) + 13/2 O₂ (g) → 4CO₂ (g) + 5H₂O(1);
∆꜀H = -2658.0 kJ mol⁻¹
(d) C₄H₁₀ (g) + 13/2 O₂ (g) → 4CO₂ (g) + 5H₂O(1);
∆꜀H = +2658.0 kJ mol⁻¹

Answer 1

Answer:

A

Explanation:

Answer 2

Answer:

 (c) Exothermic reaction for combustion of one mole of butane is represented as :

C4H10(g)+132O2(g)→4CO2(g)+5H2O(l) ΔcH=−2658kJmol−1