Calculate the enthalpy of formation of buta-1, 3-diene $C_{4} H_{6}$ (only magnitude in nearest integer in kj/mol).

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Solution

Formation of $C_{4} H_{6}$

$R : 4 C + 3 H_{2} \to C_{4} H_{6}; Δ H = ?$

From the given table, enthalpies of the following reactions are

$R_{1} : C + O_{2} \to C O_{2}; Δ H_{1} = - 394 k J / m o l$

$R_{2} : H_{2} + \frac{1}{2} O_{2} \to H_{2} O; Δ H_{2} = - 286 k J / m o l$

$R_{4} : C_{4} H_{6} + \frac{11}{2} O_{2} \to 4 C O_{2} + 3 H_{2} O; Δ H_{3} = - 2542 k J / m o l$

And

$R = - R_{4} + 4 R_{1} + 3 R_{2}$

$\Rightarrow Δ H = - Δ H_{4} + 4 Δ H_{1} + 3 Δ H_{2} = 2542 - 4 \times 394 - 3 \times 286 = 108 k J / m o l$

Answer $=$ 108

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