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0.75 mole of a solid $X_{4}$ and 2 moles of $O_{2}$ (g) are heated in a sealed vessel, completely using up the reactants and produces only one compound.
It is found that when the temperature is used to initial temperature, the contents of the vessel exhibit a pressure equal to $\frac{1}{2}$ of the original pressure.
The formula of the product will be

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$X_{2} O_{3}$

$X_{3} O_{8}$

$X_{3} O_{4}$

${XO}_{2}$

answer is C.

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Detailed Solution

As both the reactants are consumed completely, thus the ratio of stoichiometric coefficients would be 0.75 :2 or 3 : 8.

So, $3 X_{4} + 8 O_{2} ⟶ Product$

Now, as final pressure is half of oxygen initially, thus the molecular formula will be $X_{3} O_{4}$ to balance the equation correctly.

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