For the reaction, `N_(2)O_(5(g))hArr2NO_(2(g))+0.50_(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.

Explanation

`{:(,N_(2)O_(5),hArr,2NO(g)+,(1)/(2)O(g)),("Initial pressure",600,,0,0),("Final pressure",600-P,,2P,P//2):}`
`P prop` moles if `V,T` are constant (where mole equivalent to pressure `P` are decomposed)
Thus, `600 - P + 2P + P//2 = 960` or `P = 240mm Hg`
Thus, mole fraction of `N_(2)O_(5)` decomposed `= (240)/(600) = 0.4`