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Heat of Reaction

Given:[ H2 g ...

Question

Given:
$⎡ ⎢ ⎢ ⎢ ⎢ ⎢ ⎣ \begin{matrix} H_{2} (g) + \frac{1}{2} O_{2} (g) = H_{2} O (g); Δ H = - 241.8 k J C_{2} H_{2} (g) + \frac{5}{2} O_{2} (g) = 2 C O_{2} (g) + H_{2} O (g); Δ H = - 1300 k J \end{matrix} ⎤ ⎥ ⎥ ⎥ ⎥ ⎥ ⎦$
Equal volumes of $C_{2} H_{2}$ and $H_{2}$ are combusted under identical conditions. The ratio of heats evolved in the two cases is

5.37/1

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Solution

The correct option is A 5.37/1
According to Avogadro's law: Equal volumes of all gases, at the same temperature and pressure, have the same number of molecules/moles.

Lets consider equal volumes are combusted in such a manner that 1 mole of each is combusted.
$Δ H$ for 1 mole of the reactant is given in the question.
$∴$ Using the given data,
$\frac{△ H_{c o m b} (C_{2} H_{2})}{△ H_{c o m b} (H_{2})} = \frac{- 1300}{- 241.8}$ = $\frac{5.376}{1}$

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C_{2} H_{2}

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