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Heat of Formation

The combustio...

Question

The combustion of one mole of benzene takes place at 298K and 1 atm after combustion $C O_{2 (g)}$ and $H_{2} O_{J}$ are produced and 3267.0 KJ of heat is liberated. Calculate the standard enthalpy of formulation $Δ H f$ of benzene. Standard enthalpy of formation of $C O_{2 (g)}$ and $H_{2} O_{J}$ are -393.5Kj and -285.83Kl/Mole

A

-48.51 KJ/Mole

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B

48.51 KJ/Mole

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C

-24.5KJ

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D

24.5KJ

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Solution

The correct option is B 48.51 KJ/Mole
$\begin{matrix} {C_{6} H_{6}}_{(B e n z e n e)} + \frac{15}{2} O_{2} \to 6 C O_{2} + 3 H_{2} O & Δ H_{r x n} = - 3267 K J Δ H_{r x n} = 6 Δ H_{f} C O_{2} + 3 Δ H_{f} H_{2} O - Δ H_{f} C_{6} H_{6} Δ H_{f} (B e n z e n e) = 6 \times (- 393.5) + 3 (- 285.8) + 3267 \Rightarrow - 3218.49 + 3267 Δ H_{f} (B e n z e n e) = 48.51 K J \end{matrix}$
Option B is correct.

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