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InterviewSolution
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For the equation `N_(2)O_(5)(g)=2NO_(2)(g)+(1//2)O_(2)(g)`, calculate the mole fraction of `N_(2)O_(5)(g)` decomposed at a constant volume and temperature, if the initial pressure is `600 mm Hg` and the pressure at any time is `960 mm Hg`. Assume ideal gas behaviour. |
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Answer» If `p` is the partial pressure of `N_(2)O_(5)` that has decomposed, then `underset(600 mm Hg-p)(N_(2)O_(2)(g))tounderset(2p)(NO_(2)(g))+underset(p//2)((1)/(2)O_(2)(g))` Pressure at any time `=(600 mm Hg-p)+2p+p//2` `=600 mm Hg+(3//2)p` Equating this tp `960 mm Hg`, we get `p=(2)/(3)(960-600)mm Hg=244 mm Hg` The mole fraction of `N_(2)O_(5)` decomposed would be `x=(244 mm Hg)/(600 mm Hg)=0.407` |
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