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Enthalpy

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The standard heats of formation at $298 K$ for $C {C l}_{4} (g), H_{2} O (g), {C O}_{2} (g)$ and $H C l (g)$ are $- 25.5, - 57.8, - 94.1$ and $- 22.1$ $k c a l$ ${m o l}^{- 1}$ respectively. Calculate $Δ H_{298}^{o}$ for the reaction.
$C {C l}_{4} (g) + H_{2} O (g) ⟶ {C O}_{2} (g) + 4 H C l (g)$

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Solution

$C {C l}_{4} (g) + H_{2} O (g) ⟶ {C O}_{2} (g) + 4 H C l (g)$

$Δ H^{o} = Δ H_{f (p r o d u c t s)}^{o} - Δ H_{f (r e a c t a n t s)}$

$= [Δ H_{({C O}_{2})}^{o} + 4 Δ H_{(H C l)}^{o}] - [Δ H_{(C {C l}_{4})}^{o} + 2 Δ H_{(H_{2} O)}^{o}] = [- 94.1 + 4 \times (- 22.1)] - [- 25.5 + 2 \times (- 57.8)]$

$=$ $- 182.5$ $-$ ( $-$ $141.1$ )

$= - 41.4 k c a l$

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