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Standard enthalpy of formation of three combustible isomers compound A, B, C are $- 20 kcal / mol, 30$ $kcal / mol$ and $40 kcal / mol$ respectively then what will be order of their enthalpy of combustion?

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$Δ H_{c}^{\circ} [A] < Δ H_{c}^{\circ} [B] < Δ H_{c}^{\circ} [C]$

$\begin{aligned} Δ H_{c}^{\circ} [B] > Δ H_{c}^{\circ} [A] > Δ H_{c}^{\circ} [C] \end{aligned}$

$\begin{array}{r} Δ H_{c}^{\circ} [A] > Δ H_{c}^{\circ} [B] > Δ H_{c}^{\circ} [C] \end{array}$

$Δ H_{c}^{\circ} [C] > Δ H_{c}^{\circ} [A] > Δ H_{c}^{\circ} [B]$

answer is C.

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Detailed Solution

$\begin{array}{ll} A ⟶ B Δ H_{Rxn}^{\circ} = 50 kcal / mol Δ H_{C}^{\circ} [A] > Δ H_{C}^{\circ} [B] \\ B ⟶ C Δ H_{R x n}^{\circ} = 10 kcal / mol Δ H_{C}^{\circ} [B] > Δ H_{C}^{\circ} [C] \end{array}$

So order will be $Δ H_{C}^{\circ} [A] > Δ H_{C}^{\circ} [B] > Δ H_{C}^{\circ} [C]$ .

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