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For the reaction ,$N_2O_5(g)\iff 2NO_2(g)+0.5O_2(g)$.Calculate the mole fraction of $N_2O_5(g)$ decomposed at a constant volume and temperature,if the initial pressure at any time is 960mm Hg.Assume ideal gas behaviour.

$(a)\;0.2\qquad(b)\;0.3\qquad(c)\;0.1\qquad(d)\;0.4$

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$N_2O_5\iff 2NO(g)+\large\frac{1}{2}$$O_2$(g)
Initial pressure :
$N_2O_5\Rightarrow 600$
$2NO\Rightarrow 0$
$\large\frac{1}{2}$$O_2\Rightarrow 0$
Final pressure :
$2NO\Rightarrow 600-p$
$2p\Rightarrow 2p$
$\large\frac{1}{2}$$O_2\Rightarrow \large\frac{p}{2}$
Step 2:
$p\alpha$ moles if $V,T$ are constant.
$\therefore 600-p+2p+\large\frac{p}{2}$$=960$
$p=240mm\;Hg$
$\therefore$ Mole fraction Of $N_2O_5$ decomposed $=\large\frac{240}{600}$
$\Rightarrow 0.4$
Hence (d) is the correct answer.
answered Nov 6, 2013 by sreemathi.v
 

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