Question

During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is
(a) $2C_4H_{10}(g) + 13O_2(g) \rightarrow 8CO_2(g) + 10H_2O(l)$; $\Delta_cH$ = -2658.0 kJ mol⁻¹
(b) $C_4H_{10}(g) + \frac{13}{2}O_2(g) \rightarrow 4CO_2(g) + 5H_2O(l)$; $\Delta_cH$ = -1329.0 kJ mol⁻¹
(c) $C_4H_{10}(g) + \frac{13}{2}O_2(g) \rightarrow 4CO_2(g) + 5H_2O(l)$; $\Delta_cH$ = -2658.0 kJ mol⁻¹
(d) $C_4H_{10}(g) + \frac{13}{2}O_2(g) \rightarrow 4CO_2(g) + 5H_2O(l)$; $\Delta_cH$ = +2658.0 kJ mol⁻¹

Answer 1

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✏ Option [C.] is Correct

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➾This option seems correct to me so I have taken it as the correct option.

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Answer 2

Option {C} is the answer.

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