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  • During complete combustion of one mole of butane, 2658 kJ of heat is released. The thermochemical reaction for above change is

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

(i)

2C_{4}H_{10}(g)+13O_{2}(g)\rightarrow 8CO_{2}(g)+10H_{2}O_{(l)}\Delta _{c}H=-2658.0\; kJ\; mol^{-1}

(ii)

C_{4}H_{10}(g)+\frac{13}{2}O_{2}(g)\rightarrow 4CO_{2}(g)+5H_{2}O(g)\Delta _{c}H=-1329.0\; kJ\; mol^{-1}

(iii)

C_{4}H_{10}(g)+\frac{13}{2}O_{2}(g)\rightarrow 4CO_{2}(g)+5H_{2}O(l)\Delta _{c}H=-2658.0\; kJ\; mol^{-1}

(iv)

C_{4}H_{10}(g)+\frac{13}{2}O_{2}(g)\rightarrow 4CO_{2}(g)+5H_{2}O(g)\Delta _{c}H=+2658.0 kJ\; mol^{-1}

Answers (1)

The answer is the option (iii).

Explanation: The definition of the enthalpy of combustion is when the substance undergoes combustion and the enthalpy change that happens per mole in that substance. All other reactants are assumed to be in their standard states at that time.

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