For the real gases reaction,
$2 CO (g) + O_{2} (g) ⟶ 2 {CO}_{2} (g); Δ H = - 560 kJ .$ In 10 litre rigid vessel at 500 K the initial pressure is 70 bar and after the reaction it becomes 40 bar. The change in internal energy is :

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-530 kJ

-563 kJ

- 557 kJ

None of these

answer is B.

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Detailed Solution

In the reaction we have,

$\begin{array}{l} 2 CO (g) + O_{2} (g) ⟶ 2 {CO}_{2} (g); Δ H = - 560 kJ \\ Δ H = Δ U + Δ (P V) = Δ U + V Δ P \\ \Rightarrow Δ U = - 560 - \frac{10 (40 - 70) \times 100}{1000} = - 530 kJ \end{array}$

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