Calculate the value of $Δ H^{o} / k J$ for the following reaction using the listed thermochemical equations:
$\begin{array}{l} 2 C (s) + H_{2} (g) \to C_{2} H_{2} (g) \\ 2 C_{2} H_{2} (g) + 5 O_{2} (g) \to 4 C O_{2} (g) + 2 H_{2} O (1) Δ H^{0} / k J = - 2600 k J \\ C (s) + O_{2} (g) \to C O_{2} (g) Δ H^{0} / k J = - 390 k J \\ 2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (1) Δ H^{0} / k J = - 572 k J \end{array}$

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$+ 214$

$+ 234$

$+ 184$

$+ 202$

answer is D.

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Detailed Solution

$\begin{array}{l} 2 C_{2} H_{2} (g) + 5 O_{2} (g) \to 4 C O_{2} (g) + 2 H_{2} O (I) (i) \\ Δ H^{0} / k J = - 2600 k J \\ C (s) + O_{2} (g) \to C O_{2} (g) Δ H^{0} / k J = - 390 k J (i i) \\ 2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (I) Δ H^{0} / k J = - 572 k J (i i i) \\ Δ_{r} H f o r 2 C (s) + H_{2} (g) \to C_{2} H_{2} c a n b e c a l c u l a t e d b y \\ Δ_{r} H = - (- 1300) + 2 (- 390) + \times (- 572) \\ Δ_{r} H = 234 \end{array}$